Class 10 Physical Science

• Chapter 1 Concerns About Our Environment Long Answer Questions
• Chapter 2 Behaviour Of Gases Long Answer Questions
• Chapter 3 Chemical Calculations Long Answer Questions
• Chapter 4 Thermal Phenomena Long Answer Questions
• Chapter 5 Light Long Answer Questions
• Chapter 6 Current Electricity Long Answer Questions
• Chapter 7 Atomic Nucleus Long Answer Questions
• Chapter 8 Physical And Chemical Properties Of Matter Long Answer Questions

Chapter 8 Physical And Chemical Properties Of Matter Broad Answer Type Questions

Question 1. What are groups and sub-groups?
Answer:

Groups:

Groups Mendeleev’s periodic table shows that the elements with related chemical properties fall in one below the other forming vertical columns called groups. There are nine group from group I to group VIII and O (zero).

Sub-groups:

Sub-groups Each of the groups from I to VII has been divided into two. Sub-groups A and B.

Question 2. What are halogen elements? In which do they belong?
Answer:

Halogen elements: The four strongly electro-negative non-metals fluorine (F), chlorine (CI), bromine (Br) and iodine (1) form a family of closely allied elements known as the halogens meaning literally sea self-producer as these elements react with most metals to form compounds similar to sea-salt, sodium chloride.

Position in periodic table: Habzen elements placed in group VII B of the periodic table. The electro-negative character of the elements increases from left to right in a period. So, the strongly electro-negative elements are in the most extreme right group i.e. in group VII B of the period table.

Question 3. What are called alkali metals? In which group do they belong? State the similarity of their chemical properties.
Answer:

Alkali metals: Lithium (Li), Sodium (Na), Potassium (K), Rubidium (Rb) and Caesium (Cs). These five metals are generally known as alkali metals.

Position in the periodic table: The alkali metals are included in the A subgroup of the first group

Similarity:

1. Alkali metals are strong electropositive.
2. The oxides of these metals are strongly basic.
3. Each has valency 1.

WBBSE Class 10 Physical Science Solutions

Question 4. Discuss the position of hydrogen in the periodic table. Answer: Position of hydrogen in the periodic table :

Reasons for placing in group IA :

• Like the alkali metals, hydrogen is electropositive.
• The valence of hydrogen is I, alkali metals are also non-valent.
• During the electrolysis of a fused chloride of an alkali metal, deposits at the cathode; in the electrolysis of a dilute aqueous solution of hydrogen chloride, hydrogen collects at the cathode.
• Like alkali metals, hydrogen has a reducing property and forms stable oxides like water (H₂O).
• Like hydrogen, each of the alkali metals. Li, Na, K, Rb Cs, Fr possesses one valence-lectron.

Reasons for placing in group VIIB:

• Like halogens, hydrogen is a non-metatallic element.
• The valency of hydrogen and that of each halogen is 1.
• Halogen molecules are diatomic, a hydrogen molecule is also diatomic.
• The halogens from metallic halides like, NaCl, KBr, Kl etc. Hydrogen also produces salt-like hydrides like L, H, NaH, CaH, etc with the strongly electropositive element and hydrogen here acts as an electro-negative element.
• Atoms of halogen elements may transform to negative halide ions by taking one electron each.
• For example, x+eX; X = F, Cl, Br, I and hydrogen atom also may transform to a negative hydride ion by capturing one electron: H+e→ H.
• Like the halogens hydrogen also can produce covalent compounds reacting with electro-negative elements like S, O etc.

Due to such varied tendencies for occupying a seat in the periodic table, hydrogen is often called a naughty element or rogue element.

Question 5. Where are the inert gas elements placed and why?
Answer:

Position of inert gas elements in the periodic table:

• He, Ne, Ar, Kr, Xe, and Rn. These are inert elements. They are each gaseous and monoatomic. These are chemically non-reactive. As these elements do not react, they have zero valency.
• So they are included in the O (zero) group of the periodic table. Besides Helium, all the inert gases have eight (8) electrons in their outermost orbit. There are only 2 electrons in the outermost orbit of Helium.

Question 6. How is copper purified by the electrolysis method?
Answer:

Purification of copper by electrolysis method :

1. Electrolyte:  15% of CuSO₄, solution (aqueous) containing (5-10) % sulphuric acid at 50°C is taken in a voltameter.

2. Electrodes:

• Cathode: Pure thin copper plate.
• Anode: Thick impure copper plate.

3. Electrolysis:

• On electrolysis, copper dissolves from the anode and deposits on the cathode. Thus gradually the anode plate wears out and the cathode plate thickens.
• The copper obtained in the way 99.99% purity.

4. Reaction: \(\mathrm{CuSO}_4 \rightleftharpoons \mathrm{Cu}^{2-}+\mathrm{SO}_4^{2-}\)

• At cathode:  Cathode : Cu^2-+2e →Cu↓
• At anode: Cu – 2e → Cu^2-

WBBSE Class 10 Physical Science Solutions

Question 7. How is aluminium extracted from the electrolysis method?
Answer:

Extraction of aluminium by electrolysis method :

1. Electrolytes:

• Alumina (Al₂O₃) 20%
• Fused Cryolite (AIF₃, 2NaF 60%)
• CaF₂, 20%.

2. Electrodes:

• Cathode: Inner lining of carbon of the steel tank.
• Anode: Thick carbon rod suspended into a fused electrolyte

Reaction:

At cathode: Al³ + 3e → Al↓

At anode : 3F – 3e→ 3F

⇒ Al₂O₃ +6F → 2 AIF₃+3O

⇒  6O →3O₂

Question 8. Draw the diagram of the covalent radius of hydrogen.
Answer:

The diagram of the covalent radius of hydrogen

Question 9. Draw the diagram of the showering comparison of Vanderwaal’s radius and covalent radius.
Answer:

The diagram of the showering comparison of Vanderwaal’s radius and covalent radius

Question 10. State the contact process for the manufacture of sulphuric acid.
Answer:

Contact process for the manufacture of sulphuric acid :

Principle: 

1. Formation of SO₂: SO₂ is prepared by burning sulphur or iron pyrites in excess of air.

Equation:  S+ O₂ = SO↑ Or,

4 Fes,+ || O₂ = 2Fe₂O₃ + 8SO₂ ↑
(Iron pyrities)

2. Formation of sulphur trioxide (SO₃):  SO₃ is prepared by the oxidation of sulphur dioxide with oxygen (from air) in the presence of platinised asbestos or, V₂ O₅ as catalyst at 450°C.

Equation: \(2 \mathrm{SO}_2+\mathrm{O}_2 \rightleftharpoons 2 \mathrm{SO}_3+192.5 \mathrm{Kj}\)

3. Formation of oleum:

Now sulphur trioxide thus produced is not allowed to react with water directly sulphur trioxide absorbs concentrated sulphuric acid 98% turning it as fuming sulphuric acid or oleum.

Equation: SO₃+ H₂SO₄= H₂S₂O₇ (Oleum)

4. Dilution of oleum to sulphuric acid: Pure and concentrated sulphuric acid is produced by adding slowly a requisite amount of water in fuming sulphuric acid.

Equation:

H₂S₂O₇ >+ H₂O = 2 H₂SO₄

Question 11.

1. Write down the electronic arrangement of the element  ₁₇X ³⁵   What is the valency of the element?
2. Will the element form an onion or cation?
3. What type of valency will be exhibited when the element combines with sodium?

Answer:

The electronic configuration of the element X is: 2, 8, 7,

• As an atom of the element tends to capture or share one electron to attain stable of the octet, its valency is 1.
• It will form an anion by capturing electrons.
• The element will exhibit electro-valency when it combines with sodium since sodium is a metal, an atom which tends to release one electron.

Question 12. The atomic number of element A is 20 and that of another element B is 17. Write down their electronic configuration. Will they produce on electrova- lent compound or a covalent compound? What will be their valencies in that case?
Answer:

1. The electronic configuration of A is: 2, 8, 8, 2.
2. The electronic configuration of B is: 2, 8, 7.

They will produce an electrovalent compound.

Explanation:

An atom A will give up two (2) valence electrons. Each of the two atoms of B will capture one electron. In the process atoms of A and B attain a stable octet state and atoms of A will be positive ions and those of B will be negative ions.

• A and B thus form an electrovalent compound.
• As an atom of A loses two electrons.
• So A has valency 2 (two) and since each atom of B captures one electron, The valency of B will be one (1).

WBBSE Class 10 Physical Science Solutions

Question 13. What is the difference between ionic compounds and covalant compounds?
Answer:

Difference between ionic and covalent compounds:

Question 14. How ammonia is prepared in the laboratory?
Answer:

Laboratory preparation of Ammonia:

• Chemicals required: Ammonium chloride (NH₄, CI) and quick lime (CaO) or dry slaked lime (Ca (OH₂)^–
• Condition: Normally ammonia gas is obtained in the laboratory by heating a mixture of ammonium chloride with slaked lime. Instead of using slaked lime quick lime may also be used.
• Collection: Ammonia is lighter than air, it may be collected by the downward displacement of air.

Ammonia is not collected through the downward displacement of water because it is highly soluble in water.

Equation of the reaction:

2NH₄ CI + Ca (OH)₂ = 2NH₃ ↑ + CaCl₂+ 2H₂O
↑
2NH₄CH+CaO = 2NH₃↑ + CaCl₂+H₂O

• Precautions: The ingredients, the test tube, the delivery pipes and the gas jar should be absolutely dry. All the connections in the apparatus should be leak-proof.
• Drying of ammonia: As ammonia is a basic substance, it cannot be dried by acidic drying agents like cones. H₂SO, or P₂O₅,
• The gas is absorbed by fused CaCl₂, with the formation of an addition compound CaCl₂, 8NH₃. SO, fused CaCl₂, cannot be used to dry ammonia. It is best dried with the basic drying agent, quick lime (CaO).

Question 15. Prove by experiment that ammonia is dissolved in water and produces an alkaline solution.
Answer:

Fountain experiment:

Arrangement of the experiment: A flask is filled with dry ammonia gas and its mouth is corked. The flask is kept inverted position and is clamped to a stand.

Through a hole in the cork one end of a glass tube is introduced inside the flask. This end of the tube inside the flask is shaped into a jet. The other end of the tube dips in some red litmus solution taken in a beaker.

1. Operation: Now ice or ether is poured upon the flask.
2. Observation: A blue fountain produces inside the flask.

Explanation:

• Due to the evaporation of ether, the flask is cooled. Ammonia gas inside the flask contracts, as a result, there is a partial vacuum inside the flask.
• At this stage, if the stop cock is opened the red litmus solution rushes inside the flask and ammonia is dissolved in it.
• Due to vacuum created inside there is a formation of the fountain and the solution becomes blue.

Conclusion: This experiment proves that ammonia is highly soluble in water and the aqueous solution is alkaline.

WBBSE Class 10 Physical Science Solutions

Question 16. Draw the diagram of the formation of sodium chloride.
Answer:

The diagram of the formation of sodium chloride

Question 17. Draw the diagram of sodium fluoride :
Answer:

The diagram of sodium fluoride

Question 18. What are the main points of difference between metallic conductors on electrolytic conductors?
Answer:

Difference between metallic conductors and electrolytic conductors :

Question 19. What changes are taking place during the electrolysis of an electrolyte?
Answer:

Changes take place during the electrolysis of an electrolyte:

• When fused or dissolved in water, electrolyte splits up into oppositely charged particles called ions.
• On passing an electric current, the cations migrate towards the cathode while the anions migrate towards the anode.
• The cations on reaching the cathode gain electrons from it and from neutral atoms which get deposited on the cathode.
• The anions on reaching the anode lose electrons and get converted into neutral atoms which may be collected as such or they may undergo some secondary change to from some other products.

Question 20. What are Biodegradable and Non-biodegradable materials?
Answer:

1. Biodegradable materials: Materials of vegetable and animal origin invariable decay and decompose into CO₂, H₂O, N₂ or NH₃ by the combined action of sometimes natural agencies like air, water, subshene etc. These are called biodegradable materials.
2. Non-biodegradable materials: Synthetic materials like plastics, polythene, Teflon, PVC etc. are not decomposed by these natural agencies even for a long time. These are called non-biodegradable materials.

Question 21. Briefly explains thermite welding of iron and steel.
Answer:

Thermite welding of iron and steel

A mixture of 3 parts of ferric oxide and I part of aluminium powder is called a thermite mixture. When the mixture is ignited ferric oxide is reduced to metallic iron by aluminium. Because of the evolution of large amounts of heat, the temperature rises to Magnesium tape

2500c The molten iron thus produced is allowed to fall on the red hot broken rails broken machine parts ect can be welded without removing them from their original sites.

Chapter 7 Atomic Nucleus Broad Answer Type Questions

Question Explain the separation of isotopes through the diffusion method.
Answer:

The separation of isotopes through the diffusion method

Though the isotopes have identical chemical properties, some of their physical properties may be quite different because of the difference in their mass numbers.

The most important physical properties of this type are the rate of diffusion, boiling point, and radioactive properties isotopes of elements can be separated by physical methods based on their properties. They may be separated almost completely using a special type of instrument called the mass spectrometer.

Diffusion method:

Since the rate of diffusion of a gas varies inversely to the square root of its molecular mass. Gas molecules with lower atomic mass numbers diffuse more quickly than their heavier sisters.

This principle was very effected actively used by Aston for the separation of isotopes of neon. The more is the difference in the atomic mass numbers, the more effective is the separation.

Class 10 Physical Science WBBSE

Question 2. Write the cause of radioactivity.
Answer:

Cause of radioactivity:

The main reason for the radioactivity of an element, as we have noted earlier, is the instability of its nucleus. Such an unstable nucleus tries to attain stability through the expulsion of particles and rays. If there are too many protons in a nucleus they will fall apart and the element will disintegrate. Again, it the nucleus is too heavy with too many neutrons it disintegrates.

It is observed that in order to attain stability the neutron: Proton ratio must be mear about unity for the elements with low atomic masses while for the heavier elements, it must not exceed 1.5.

Thus we see that most of the radioactive elements have very high atomic masses in ₉₂U²³⁴ in comparison to their atomic numbers U has a neutron; proton ratio of 1.537 while radium has 1.56. This is why radium is much more radioactive than uranium.

Question 3. Short Note-Radioactive Equilibrium.
Answer:

Radioactive Equilibrium :

The product element formed by the radioactive disintegration of an element may also be radioactive. The process goes an until the chain is terminated by the birth of a non-radioactive stable element at the end of a series. If we keep a sample of a radioactive element or its salt for a sufficient time, a situation arises when the rate of creation and the rate of disintegration of a product element become equal.

This state for a radioactive series is called a radioactive equilibrium. We see that at the equilibrium.

⇒ \(\frac{\mathrm{dN}_1}{\mathrm{dt}}=\frac{\mathrm{dN}_2}{\mathrm{dt}}=\frac{\mathrm{dN}_3}{\mathrm{dt}}\)

∴ λ₁ N₁ = λ₂ N₂ = λ₃ N₃ = …………

Question 4. Short Note Mass spectrometric method to separate the isotope.
Answer:

Mass spectrometric method:

In this method positive particles of the required gas or vapour formed by bombardment with electrons are first passed through electrical plates with a potential difference (X) of about 1000 volts and two collimating slits. The electrical energy Xe, where e is the charge of the positive particles, is equal to the kinetic energy of the particles.

That is Xe =½ mu² where m and v are the mass and the charge of the positive particles. The positive particles energing through a slit with almost equal kinetic energy pass a magnetic field (H) between two semicircular.

Question 5. What is binding energy? Short Note-Stability of an atomic nucleus packing fraction.
Answer:

Binding energy

The amount of energy that can be obtained by the amount of mass equal to the mass defect is known as the binding energy.

1. The atomic mass of an isotope of an element is expected to be equal to the Sun of the fundamental particles present in it. In AMU the mass of a proton or a neutron is nearly equal to unity while that of an electron is negligible.
2. Atomic masses of isotopes of elements are expected to be approximately whole numbers. Called atomic mass numbers.

Packing faction =  \(\frac{\text { Actual mass of a nucleus }- \text { Mass number }}{\text { Mass number }} \times 10^4\)

WB Class 10 Physical Science Question Answer

Question 6. What are isotones? Define-nuclear isomers.
Answer:

Isotones

The are elements which differ in both their atomic numbers as well as most numbers but they have the same number of neutrons in their nuclei. They are called isotones.

Nuclear isomers

The two nuclei of an element may have the same atomic number and the same mass number yet differ in their internal nuclear energies. These nuclei are called nuclear isomers.

Question 7. Explain the separation of isotopes by distillation under low pressure.
Answer:

Separation of isotopes by distillation under low pressure

Distillation under low pressure: When a liquid like mercury is distilled under low pressure the lighter isotopes come out more quickly and condense on a cooler surface. The condensate is collected, melted and subjected to the same procedure. B repeating the process the condensate can be made richer in the lighter variety.

Question 8.  What do you mean by isobars and isotones?
Answer:

Isobars

Isobars The nuclide of different chemical elements having the same mass number but different atomic numbers are called isobars.

Examples:

1. ₁₈ Ar⁴⁰
2. ₁₉K⁴⁰
3. ₂₀Ca⁴⁰

Isotones: The nuclides of different chemical elements having the same number of neutrons but different atomic numbers are called isotones.’

Examples: ₁H³, ₂He⁴

Question 9. What are the parent and end products of different disintegration series?
Answer:

Series

Question 10. What are the differences between nuclear fission and nuclear fusion?
Answer:

Difference between nuclear fission and nuclear fusion :

Question 11. What do you mean by Curie and Becquerel?
Answer:

Curie and Becquerel

• Curie If a radioactive substance disintegrates at the rate of 3.7 × 10¹⁰ disintegrations per second, its activity is said to be 1 curie.
• Becquerel (SI unit): If a radioactive substance has 1 disintegration per second, it is said to have an activity of one Be equal.

WB Class 10 Physical Science Question Answer

Question 12. A radioactive substance decays at such a rate that after 46 days only 0.25 of its original amount is left to calculate its disintegration constant.
Answer:

Given

A radioactive substance decays at such a rate that after 46 days only 0.25 of its original amount is left

Let, the original amount be No then Amount after 46 days, Nt = 0.25 x No For a nuclear decay,

λ = \(\frac{2.303}{\mathrm{t}} \log \frac{\mathrm{No}}{\mathrm{Nt}}\)

= \(\frac{2.303}{46}\) log⁴ day^-1

= 0.0301day^-1

Question 13. A certain nuclide has a half-life of 60 min. If a sample containing 600 atoms is allowed to decay for 90 min, what will be the remaining atoms?
Answer:

Given

A certain nuclide has a half-life of 60 min. If a sample containing 600 atoms is allowed to decay for 90 min

λ = \(\frac{0.693}{60} \mathrm{~min}^{-1}\)

= \(\frac{2.30^3}{90} \log \frac{\mathrm{No}}{\mathrm{N}}\)

⇒ log \(\frac{\mathrm{No}}{\mathrm{N}}\) = 0.4514 Or,

⇒ log \(\frac{\mathrm{No}}{\mathrm{N}}\)= 2.828

∴N = \(\frac{600}{2.823}\)

N= 212

Question 14. The activity of a sample of radioactive element A100 is 6.02 curie. Its decay constant is 3.7 x 10’S’ which calculates the initial mass of the sample.
Answer:

Given

The activity of a sample of radioactive element A100 is 6.02 curie. Its decay constant is 3.7 x 10’S’

Activity = \(\lambda \times \frac{\mathrm{wt}}{\text { at. wt }} \times 6.023 \times 10^{23}\)

\(6.02 \times 3.7 \times 10^{10}=3.7 \times 10^4 \times \frac{w}{100} \times 6.023 \times 10^{23}\)

 

W= \(\frac{6.02 \times 3.7 \times 10^{10} \times 100}{3.7 \times 1.04 \times 6.023 \times 10^{23}}\)

W= \(10^{-15} \mathrm{~g}\)

Question 15. The half-life period of C is 5760 years. An old piece of wood has a disintegration rate which is 25% of the disintegration rate of an equal weight of a new piece of wood.
Answer:

Given

The half-life period of C is 5760 years. An old piece of wood has a disintegration rate which is 25% of the disintegration rate of an equal weight of a new piece of wood.

Let the rate of disintegration of the new piece = 100

The rate of migration of old pieces = 25

K = \(\frac{0.693}{\frac{t_1}{2}}=\frac{0.693}{5760}\)

t= \(\frac{2.303}{K} \log \frac{a}{a-x}\)

=\(\frac{2.303}{K} \log \left(\frac{\mathrm{lo}}{\mathrm{It}}\right)\)

∴ \(=\frac{2.30 \times 5760}{0.693} \log \frac{100}{25}\)

t= 11523 years.

Class 10 Physical Science Solution WBBSE Chapter 6 Current Electricity Broad Answer Type Questions

Question 1. State Joule’s laws of heating effect of current.
Answer:

Joule’s Laws (1841):

1.  First Law:

The amount of heat produced in a conductor in a given interval of time of proportion to the square of the current passed. Thus if H be the amount of heat generated in a conductor having resistance R when current 1 passes through it in time t, then

⇒ Hα I² (When R and t are kept constant)

2. Second law:

The amount of heat produced by a given current in a given time is proportional of the resistance of the conductor.

⇒  H α R (When I and t are kept constant)

3. Third Law:

The amount of heat produced in a given conductor by a given current is proportional to the time for which the current passes.

⇒  Hα t (When I and R are kept constant)

Combining the three laws, we have:

⇒ H α I² RT (When 1, R and t vary) or,

H = \(\frac{I^2 R T}{J}\)

IRT (J= mechanical equivalent of heat = 4.2 joule (calorie)

If I am in ampere, R in ohm, t in second, and H in calorie, then

H= \(\frac{I^2 R T}{J}\)

H= 0.241 RT calorie.

Question 2. Short Note: 

1. Ohmic resistance
2. Non-ohmic resistance

Answer:

1. Ohmic Resistance :

The resistors, which obey Ohm’s Law are said to have ohmic resistances.

Example: All metal or metallic alloy.

2. Non-ohmic resistance :

The resistors which do not obey Ohm’s law are said to have non-ohmic resistance.

Example: Electronic value.

Question 3. Two resistors of 30W and 60W are connected in parallel in an electric circuit. How does the current passing through the two resistors compare?
Answer:

Given

Two resistors of 30W and 60W are connected in parallel in an electric circuit

The potential difference across 30W = B potential difference across 60W

i.e I₁ R₁= I₂ R₂ Or,

⇒ \(\frac{I_1}{I_2}=\frac{R_2}{R_1}\)

= \(\frac{60 \Omega}{30 \Omega}\)

= 2

Question 4. Short Note-Direct Current.
Answer:

Direct Current:

If a resistor connects with the two terminals of an electric cell, then through the resistor a steady current of constant magnitude flows in the same direction (from the positive pole of the cell to the negative pole) and this is called a direct current.

Class 10 Physical Science Solution WBBSE

Question 5. A resistance of 6 Ω is connected with a cell of em. f. 1.5 and negligible internal resistance calculate the current flowing through it.
Answer:

Given

A resistance of 6 Ω is connected with a cell of em. f. 1.5 and negligible internal resistance

V= IR Or, I= \(\frac{V}{R}\)

= \(\frac{1.5}{6}\)

= \(\frac{1}{4}\)

V = 0.25 Amp

The current flowing through it is 0.25 Amp

Question 6. Find the specific resistance of the material of a wire of length 100cm, area of cross-section 0.2 cm,^2, and resistance 2 ohms.

Answer:

R = P× \(\frac{1}{\mathrm{~A}}\)

∴ P= \(\frac{\mathrm{RA}}{\mathrm{1}}\)

= \(\frac{20 \times 0.2}{100}\)

= 40 ×10^-4  Ohm^-cm

So,

R = 20hm

1 = 100 cm

A = 0.2 cm²

P= ?

Question 7. Find effective resistance of the resistors 2 ohm, 4 ohm, 5 ohm connected in

1. Series
2. Parallel.

Answer:

We know, for series combination equivalent resistance

R= r₁+ r₂+r₃

= 2+4+5

= 11 ohm.

We also know, for parallel combination equivalent resistance.

⇒ \(\frac{1}{R}=\frac{1}{r_1}+\frac{1}{r_2}+\frac{1}{r_3}\)

= \(\frac{1}{2}+\frac{1}{4}+\frac{1}{5}\)

= \(\frac{19}{20}\)

∴ \(\frac{1}{R}\)= \(\frac{19}{20}\) Or,

= \(\frac{20}{19}\)

R = 1.05 Ohm

Question 8. Short Note-Electric Circuit.
Answer:

Electric Circuit: A continuous conducting path between the terminals of a source of electricity, is called an electric circuit.

Open electric → An electric circuit in which the flow of current stops, because of an open switch is called an open electric circuit. Closed electric

Open Electric Circuit:

Closed Electric Circuit:

Circuit → An electric circuit in which a current flows continuously, because the switch is closed is called a closed electric circuit.

Question 9. There are two copper wires of equal length. The radius of one is twice the other. Find the ratio of their resistances.

Answer:

Given

There are two copper wires of equal length. The radius of one is twice the other.

We know, R= p \(\frac{1}{A}\)

= \(p \frac{1}{\lambda r^2}\)

(r= radius of the wire)

Since, the length and material are the same.

⇒ \(\mathrm{R} \alpha \frac{1}{\mathrm{r}^2}\)

i.e. \(\frac{R_1}{R_2}=\frac{r_2^2}{r_1^2}=\frac{\left(2 r_1\right)^2}{r_1^2}\)

= 4

∴ The thinner wire has a resistance four times the resistance of the thicker wire.

Question 10. Establish the relation between the emf, terminal voltage and internal resistance.
Answer:

The relation between the emf, terminal voltage and internal resistance

Let, a cell of emf E and internal resistance r is connected to an external resistance R

The total resistance of the circuit = R+r

So, the current drawn from the cells

I= \(\frac{e . m . f \text { of the cell }}{\text { total resistance }}\)

I= \(\frac{E}{R+r}\)

E= I (R+r)

The terminal voltage of the cell, V = IR voltage (v) drops due to internal resistance -I As the work is done carrying a unit positive charge once through a complete circuit,

E = V + v

v = E-V

Internal resistance r = \(\frac{V}{I}\)

=  \(\frac{E-V}{I}\)

= \(\frac{E-V}{V / R}\)

= \(R \cdot\left[\frac{E}{V}-1\right]\)

Question 11. A current of 0.5 ampere passes through a wire of resistance 2.5 ohm. for 1 hour. Find the heat produced.
Answer:

Given

A current of 0.5 ampere passes through a wire of resistance 2.5 ohm. for 1 hour.

We know,

H  = \(\frac{I^2 R T}{J}\)

= \(\frac{I^2 R T}{4^2}\)

∴ H \(\frac{(0.5)^2 \times 2.5 \times 3600}{4^2}\)

= 535.7 caloric

So,

I = 0.5 ampere

R = 2.5 ohm

t = 1hr.

= 3600 sec.

H =?

Question 12. The resistance of a wire of cross-section area 0.01 cm2 is 10 ohm. What is the length of the wire? The specific resistance of the wire is 50 × 10-6 ohm-cm.
Answer:

Given

The resistance of a wire of cross-section area 0.01 cm2 is 10 ohm.

We know,

R = p = \(\frac{\ell}{\mathrm{A}}\) Or,

l= \(\frac{\mathrm{RA}}{p}\) Or,

l= \(\frac{10 \times 0.01}{50 \times 10^{-6}}\)

∴ l= 2000 cm

So,

R= 10 Ohm

A= 0.01 cm²

p= 50 × 10^-6

Ohm^–cm

1= ?

Question 13. What is the difference between e.m.f and p.d?
Answer:

Difference between e.m.f. and p.d. : e.m.f (electromotive force):

Question 14. A resistance of 6Ω is connected with a cell of e.m.f., 1.5 V, and negligible internal resistance, Calculate the current flowing through it.

Answer:

Given

A resistance of 6Ω is connected with a cell of e.m.f., 1.5 V, and negligible internal resistance

V = IR

I = \(\frac{V}{R}\)

I = \(\frac{1.5}{6}\)

I = \(\frac{1}{4}\)

= 0.25 Amp.

Question 15. A cell of e.m.f. 1.8v is connected to an external resistance of 22 when p.d. recorded at its terminal is 1.6v. Find the internal resistance of cell.

Answer:

Given

A cell of e.m.f. 1.8v is connected to an external resistance of 22 when p.d. recorded at its terminal is 1.6v.

E = 1.8V, V 1.6 volt, R = 2.2

Internal resistance = \(\frac{R(E-V)}{V}\)

= \( \frac{2(1.8-1.6)}{1.6}\)

= 0.25.Ω

Physics Class 10 WBBSE Chapter 5 Light Broad Answer Type Questions

Question 1. Draw a labelled diagram to show refraction of a light ray through a prism.
Or
Path of a ray of light through a prism
Answer:

Path of a ray of light through a prism:

• Path of a ray of light through a prism Let ABC be the principal section of a prism AB and AC are two refracting surfaces. BC is the base. PQRS is the path of a ray. It is to be noticed that in i a prism.
• The refracted ray and the emer- gent ray bend towards the base of the prism, when the surrounding medium is optically rarer than the material of the prisms.
• But, if the medium outside the prism be optically denser than the prism material, the refracted and emergent rays bend oppositely i.e they bend towards the angle of the prism.

Question 2. What are the conditions of formation of pure spectrum?
Or
Production of pure spectrum
Answer:

Conditions of formation of pure spectrum:

• Slit should be very narrow to allow, rays of light to pass as minimum as possible.
• The slit should be placed at the focus so that the emergent light rays may be Parallel.
• Prism should be placed at the minimum deviation position of spec- trum i.e. at the mean deviation of yellow spectrum.
• The second lens (L₂ L₂) should be placed in such a position so that the screen may be in the focal plane of the lens.

Question 3. How will you explain twinkling of stars?
Answer:

Twinkling of stars:

The light coming from stars is refracted continuously by different layers of the atmosphere before coming to us. Due to there repeated refractions, The apparent position of a star is different from its actual position. The temperature and density of air in the atmosphere continuously changing and so apparent position of the star also changes continuously. Due to this continuous change in the apparent position of a star, it appears to be twinkling.

Question 4. A ray of light shows no dispersion on emerging from a glass slab. Explain why?
Answer:

A ray of light shows no dispersion on emerging from a glass slab

A rectangular glass slab cut diagonally into two pieces behaves like a pair of prisms placed side by side in reverse order. So the light dispersed by the first prism, recombines by the second prism. Thus there is no dispersion of light in a rectangular glass slab, bulb it is only laterally displaced.

Question 5. State the laws of reflection.
Answer:

The laws of reflection:

• The incident ray, the refracted ray and the normal to the refracting Surface at the point of incidence lie in the same plane.
• 2. For a given pair of media and for a given colour of light, sine of the angle of incidence bears a constant ratio to the sine of the angle of refraction.
• Thus if i and r be the angles of incidence and of refraction respectively when the ray passes from medium 1 to medium 2.

⇒\(\frac{sini}{sin r}\) = constant

= 1^μ2

Physics Class 10 WBBSE Question 6. Deseribe about the action of periscope.
Answer:

The action of periscope

The mirror M, forms a virtual image I₁, of the object O and this image ₁, acts as virtual object-for the mirror M₂, which forms an image I₂, which is seen by the eye the final image F₂, is also virtual. Since light rays from the object are reflected by two mirrors, the lateral inversion caused by the first mirror is reversed by the second mirror. This males the final image to appear with on lateral invession.

Question 7. State the laws of refraction.
Or
What is snell’s law?
Answer: 

1. Laws of refraction: The incident ray, the reflected ray and the normal to the refracting. Surface at the paint of incidence lie in the same plane.
2. For a given pair of media and for a given colour of light, the sine of the angle of incidence bears a constant ratio in the sine of the angle of refraction.

Thus, it i and r be the angles of incidence and of refraction respectively when the ray passes from medium 1 to medium 2.

\(\frac{sini}{sinr}\)= Constant

= 1^μ2

The second law of refraction was devolped by W, Snell and is know a Snell’s law.

Question 8. Establish the relation between 1μ₂ and 2μ₁.
Answer:

The relation between 1μ₂ and 2μ₁

From Snell’s law:  sin¹/sin^r = 2μ₁

Where 2 u₁, is the R. I. of medium 1 w.r.t. medium combining equations we get

1μ₂×2μ₁= \(\frac{sin1}{sinr}\)×\(\frac{sinr}{sin1}\) = 1

Or

1μ₂X = 1/2μ₁

Thus R.I. of medium 2 w.r.t. medium 1 is the reciprocal of R.I of medium 1 w.r.t. medum 2

Physics Class 10 WBBSE Question 9. State generalised Snell’s law.
Answer:

Generalisation Of Snell’s law

If i₁ and i₂ be the angle of incidence and of refraction respectively then we have from Snell’s law

sini₁/sini₂ =1, μ₂

We can write

1, μ₂ =μ₂ /μ₁

⇒μ₂/μ₁

∴ sini₁/sini₂= μ₂/μ₁

Or,μ₁ sini₁ = μ₂ sini₂ → Generalised Snell’s Law

Question 10. How far from a concave mirror of radius 2m would you place the object to get an image magnified 3 times?
Answer:

Given m = ± 3 \(\frac{v}{u}\) i.e.u= 7.3u

For real image v = -3u, r = -2m and u is negetive.

So, from relation \(\frac{1}{v}\)+ \(\frac{1}{u}\)= \(\frac{2}{r}\)

Or, – \(\frac{1}{3u}\) – \(\frac{1}{u}\) = – \(\frac{2}{2}\)

For virtual image u =+ 3u, r = -2m and u is negative

So =-1 or, u= = 0.67m

= \(\frac{1}{3u}\) – \(\frac{1}{u}\) = – \(\frac{2}{2}\)  Or \(\frac{1-3}{3u}\) = -1

u= \(\frac{2}{3}\)

= 0.67 m

WBBSE Class 10 Physical Science Question Answer In English Question 11. A concave mirror forms an image of 20 cm high object on a screen placed 5m away from the mirror. The height of the image is 50 cm. Find the focal lenght of the mirror and the distance between mirror and the object.
Answer:

Given

concave mirror forms an image of 20 cm high object on a screen placed 5m away from the mirror. The height of the image is 50 cm.

size of object = 20cm.

Size of the image = 50cm.

u = -5m.

= \(\frac{-10}{7}\)

= −1.43m

And distance between the mirror and the object = 2m.

Question 12. Light falls from glass of refractive index 1.5 to air. Find the angle of incidence for which the angle of deviation is 90°.
Answer:

Light falls from glass of refractive index 1.5 to air.

Refractive index of glass is 1.5. So, the critical angle of glass to air medium is given by

⇒ − q= sin^-1(\(\frac{1}{u}\)) sin^-1(\(\frac{1}{1.5}\))

= 41.8°

So, reflection in the glas medium takes only when the angle of incidence exceeds  41.8°. Now the angle of deviation. Would be 90° when the angle between the incident ray and the reflected ray becomes 90° i.e. the angle of incidence be equal to 45°.

Question 13. Where should an object be placed from a converging lens of focal length 20cm, so as to obtain a real image of magnification 2 ? u =2, or, v = + 2u, f= + 20cm
Answer:

Given m =\(\frac{u}{u}\)= 2 or  , v= +2u, f= +20cm

∴ \(\frac{1}{v}\)– \(\frac{1}{u}\) = \(\frac{1}{f}\) or,

=  \(\frac{1}{2u}\) – \(\frac{1}{u}\)

= \(\frac{1}{20}\) or,

= \(\frac{1-2}{2u}\)

∴ u= \(\frac{− 20×1}{2}\)

= – 10 cm

i.e. object to be placed 10 cm in fornt of the lens.

WBBSE Class 10 Physical Science Question Answer In English

Question 14. Two thin lens of focal lengths 15cm. and 30cm. respectively are kept in contact with each other. What is the power of the combined system?
=
Answer: Given

Two thin lens of focal lengths 15cm. and 30cm. respectively are kept in contact with each other.

f₁= 15cm, f₂ = 30cm.

Then focal length F of the equivalent lens

\(\frac{1}{F}\)= 1/f₁+1/f₂

\(\frac{1}{15}\) + \(\frac{1}{30}\)

= \(\frac{2+1}{30}\)

= \(\frac{1}{10}\)

Power of the combination = \(\frac{100}{F}\)

= \(\frac{100}{10}\)

= +10

Question 15. The dew drops deposited on hairy leaves appear glittering way?
Answer:

The hairs out the leaf and the surface tension of water create an air gap under the dew drop. Hence some of the rays trying to pass from the drop to the side air gap suffer total internal reflection. Such reflected rays may reach our eyes after refraction through the upper surface of the drop and the drop appears glittering.

16. Show that, for a spherical mirror the focal length is half of its radius of curvature.
Answer:

P = Pole

F= Focus of the mirror.

PF = f

C = Centre of curvature.

∠BP’C = ∠P’CF (alternate angles.) and

∠BP’C = ∠CP’F (law of reflections i = r)

Hence ∠’P’CF = ∠CP’F

ΔFP’ C is isosceles. Hence P’F = FC

If the aperture of the mirror is small, the point P i very close to the point P, then P’F = PF

∴ PF=  FC or, PF + PF = PF + FC

or , 2PF = PC or, PF =  ½ PC

or, f = ½ R.

Question 17. Establish relation between the angle of deviation (Dm) and the refractive index of the material of the prism (μ).
Answer:

Let, the angle of deviation be D, the refractive index of the material of the prism be μ.

For minimum deviation, we have ¡=i’

Question 18.

1. Write Cauchy’s equation 
2. Define-angular dispersion.

Answer:

1. The Cauchy’s equation: = А+B/ λ2

A, B = Cauchy’s constant

2. The angular dispersion is defined as the difference between the angles of deviation of the extreme colours, red and violet of the spectrum.

WBBSE Class 10 Physical Science Question Answer In English

Question 19. 

1. What is the condition for dispersion with deviation and deviation without dispersion?
2. What is the pure and impure spectrum?

Answer:

1. Condition for dispersion with deviation

⇒(μ_v-1)A = (μ’_y-1)A’

The condition for devotion without dispersion :

⇒ δ_y -δ_r (μ_y-1)A(w-w’)

2. 

• Pure spectrum: A spectrum in which the colours present do not overlap one another so that different colours occupy distinct and separate positions is called pure spectrum.
• Impure spectrum: A spectrum in which the colours present overlap one another and hence can not be seen distinctly separated from one another is called an impure spectrum.

Question 20. Light of two colours (say X, Y) are sent through a prism. Suppose X bents more than Y. Which colour travels more slowly in the material of the prism?
Answer:

Light of two colours (say X, Y) are sent through a prism. Suppose X bents more than Y.

We know, D, (μ_x-1)A

D1 = (μ_y-1)A

⇒ D_y>D_y

⇒ μ _x> μ_y

C/ V_x>C/ V_y

∴ V_y > V_x

The colour X travels more slowly in the material of the prism.

Question 21. Draw a ray diagram for the formation of a concave mirror when the object is at focus F.
Answer:

AB is an object placed at the focus F. The ray AD is incident on the mirror parallel axis and it gets reflected along DF, passing through the focus f. AE appears to be coming from the centre of curvature C, so it gets reflected back along EA. The two reflected rays DF and EA are parallel to each other.

The image is formed at infinity (very far from the mirror) which is real, inverted and highly magnified.

When the object is at focus F.

Thus when the object is at the focus F, the image is at infinity. It is

1.  Real
2. Inverted, and
3. Highly magnified.

Question 22. How the angle of minimum deviation of a glass prism changes when it is immersed in a liquid of R.I. greater than I? sin A+D m
Answer:

Minimum deviation of a glass prism:

Hence the angle of minimum deviation decreases.

Question 23. Define-Absorption Spectrum.
Answer:

Absorption Spectrum:

The missing wavelengths provide information about the absorbing material. Such a spectrum is called an absorption spectrum. The absorption spectrum may be of two types depending on the absorbing material and the conditions such as temperature.

Question 24 . An object 4 cm. high is placed at a distance of 10cm from a convex lens of focal length 20cm. Find the position, nature and size of the image.
Answer:

An object 4 cm. high is placed at a distance of 10cm from a convex lens of focal length 20cm.

O= 4cm, u=-10 cm, f= + 20cm.

\(\frac{1}{V}\) = \(\frac{1}{f}\) +\(\frac{1}{u}\)

= \(\frac{1}{20}\) – \(\frac{1}{10}\)

= – \(\frac{1}{20}\)

V= -20 cm

\(\frac{1}{o}\) – \(\frac{V}{u}\)

I = \(\frac{V}{u}\) × 4

= \(\frac{-20}{-10}\) ×4

= 8cm

Question 25. Two lenses one of focal length 20 cm. and another focal length -15cm, are placed in contact. What is the focal length and power of the combination?
Answer:

Two lenses one of focal length 20 cm. and another focal length -15cm, are placed in contact.

f, 20cm=0.2m f15cm – 0.15m

Power of the first lens, P₁ = \(\frac{1}{0.2}\) = 5D

Power of the second lens, P₂ = \(\frac{-1}{0.2}\)

= 6.67 D

Power of combination, P = P₁ + P₂ = 5 – 6.67 = -1.67D

Focal length, f= \(\frac{1}{1.67}\)  0.599m

The -ve sign indicates that the combination acts as a concave lens.

Question 26. An object 4 cm. high is placed at a distance of 10cm from a convex lens of focal length 20cm. Find the position nature and size of the image.
Answer:

An object 4 cm. high is placed at a distance of 10cm from a convex lens of focal length 20cm.

0=  4cm, u = -10cm, f= + 20cm,

\(\frac{1}{V}\) =\(\frac{1}{F}\)+ \(\frac{1}{u}\)

= \(\frac{1}{20}\) – \(\frac{1}{10}\)

= – \(\frac{1}{20}\)

V= – 20 cm

\(\frac{I}{O}\)= \(\frac{V}{u}\) or, \(\frac{V}{u}\)×0

= \(\frac{-20}{-10}\)×4

= 8cm

Class 10 Physical Science WBBSE Chapter 4 Thermal Phenomena Broad Answer Type Questions

Question 1. What is an anomalous expansion of water?
Answer:

Anomalous expansion of water: Usually liquids expand on heating. But in the case of water, we find a deviation from this general behaviour of the liquids within a certain range of temperature. The volume of water is minimum at 4°C and hence its density is maximum at 4°C. This phenomenon is called the anomalous expansion of water.

Question 2. What is thermo-metric conductivity?
Answer:

Thermometric conductivity: The rate of rise of temperature during the variable state is proportional to \(\frac{K}{P_s}\)(where K = thermal conductivity of the material, PS specific heat.)

This ratio is known as thermometric conductivity or the thermal conductivity per thermal capacity per unit volume.

Question 3. What is the fundamental principle of calorimetry? What are the conditions?
Answer:

Fundamental principle of calorimetry Heat lost by hot body = Heat gained by cold body.

Conditions:

• During the process of heat transfer, there is no heat exchange with the surroundings.
• No chemical reaction takes place between the bodies.

Question 4. Give a few applications of conductivity.
Answer:

Applications of conductivity:

Ice is packed in sawdust because air which is a bad conductor of heat being trapped in the sawdust prevents the transfer of heat from the surroundings to the ice. So, ice does not melt.

Question 5. Establish the relation: Coefficient of linear \((\Delta \mathrm{l})=\alpha \mathrm{l} \Delta \mathrm{t}\)
Answer:

Let us suppose that a rod has initial l₁ at t₁° and when it is heated to t₂, its length increases to l₂.

\(\begin{aligned}
& \left(l_2-l_1\right) \alpha l_1 \\
& \left(l_2-l_1\right) \alpha\left(t_2-t_1\right) \\
& \left(l_2-l_2\right) \alpha l_1\left(t_2-t_1\right) \\
& \left(l_2-l_1\right)=\alpha l_1\left(t_2-t_1\right)
\end{aligned}\)

(α = constant of proportionality)

This constant is called the coefficient of linear expansion of the solid.

\(\alpha=\frac{\mathrm{l}_2-\mathrm{b}_1 / \mathrm{l}_2}{\left(\mathrm{t}_2-\mathrm{t}_1\right)}\)

\(l_2=l_1\left\{1+\alpha\left(t_2-t_1\right)\right\}\)for a small increase in temperature At, if the length I of a rad increases by Al, then,

\(\begin{aligned}
& \alpha=\frac{\Delta \mathrm{l} / \mathrm{l}}{\Delta \mathrm{t}} \\
& \Delta \mathrm{l}=\alpha \mathrm{l} \Delta \mathrm{t}
\end{aligned}\)

WB Class 10 Physical Science Question Answer

Question 6. Establish the relation: ΔS = ΔβSΔt for superficial expansion.
Answer:

If S₁ be the initial surface area of a solid substance at t₁° and S₂, be that at t2 (t₂>t₁), the coefficient of superficial expansion is denoted by β.

\(\beta=\frac{\left(S_2-S_1\right) / S_1}{\left(t_2-t_1\right)}\) \(s_2=s_1\left\{1+\beta\left(t_2-t_1\right)\right\}\)

For a small increase in temperature Δt, if the surface area s of a solid increases by ΔS, then

\(\beta=\frac{\Delta s / s}{\Delta t}\)

Δs = βsΔt

Question 7. Establish the relation: ΔV = yVΔt of cubical expansion.
Answer:

If V₁ and V₂ are the volumes of a solid at t₁° and t₂°, (t₂>t₁) respectively, and y is the coefficient of cubical expansion.

\(y=\frac{\left(v_2-v_1\right) / v_1}{\left(t_2-t_1\right)}\)

V₂ = V₁ {1+y (t₂-t₁)}

For a small rise in temperature Δt, if the volume V of a solid increases by ΔV

\(y=\frac{\Delta V / V}{\Delta t}\)

ΔV=YVΔt

Question 8. Establish the relation : \(V_t=V_0\left(1+\frac{t}{273}\right)\) for Charle’s law.
Answer:

Let, Vo denote the volume of a given mass of a gas at 0°C.

V_t = The volume of the same mass of gas at t°C.

The pressure in both cases is the same.

For Charle’s law, the increase in volume of the gas

= \(\frac{\text { volume at } 0^{\circ} \mathrm{C}}{273} \times \text { rise in temp }=v_t-v_0=\frac{v_0}{273} \times t\)

\(v_t=v_0(1+y p t)\)

Question 9. Establish the relation V_t = V₀ (1+ y_pt) for the volume coefficient of a gas.
Answer:

If V₀ and V₂ are the volume of a given mass of a gas at 0°C and t°C respectively.

\(\mathrm{y}_{\mathrm{p}}=\frac{\text { fractional increase in volume }}{\text { rise of temperature }}=\frac{\left(\mathrm{v}_{\mathrm{t}}-\mathrm{v}_{\mathrm{o}}\right) / \mathrm{v}_{\mathrm{o}}}{\mathrm{t}}\)

V_t = V₀ (1+ y_pt)

Question 10. The thickness of an iron plate is 4mm. and its area is 150 sqm. The temperature of the two sides is 100°C, 30°C and 3940. Caloric heat is conducted in one second from one side to the other. Determine the thermal conductivity of heat.
Answer:

Given

The thickness of an iron plate is 4mm. and its area is 150 sqm. The temperature of the two sides is 100°C, 30°C and 3940. Caloric heat is conducted in one second from one side to the other.

\(\frac{\mathrm{Q}}{\mathrm{t}}=3940 \mathrm{cal} / \mathrm{s}\) , A = 150 cm^{2 ,}

x = 4mm = 0.4 cm², θ₁ = 30°C, θ₂ = 100°C

Thermal conductivity of iron.

\(\mathrm{K}=\frac{\mathrm{Qx} / \mathrm{t}}{\mathrm{A}\left(\theta_2-\theta_1\right)}=\frac{3940 \times 0.4}{150(100-30)} \text { c.g.s unit. }=0.15 \text { c.g.s. unit. }\)

Question 11. The thermal conductivity of aluminium is 0.50 cal/sec. cm degree. Express the same in units of watt/m degree.
Answer:

Given

The thermal conductivity of aluminium is 0.50 cal/sec. cm degree.

K 0.5 cal/5 cm degree

= 0.5 x 4.2 Joule/s Cm degree

= 0.5 × 4.2 × 100 Joule/s m degree

= 210 watt/m degree.

Question 12. A pond is covered with ice 5cm. thick and the temperature of overlying air is -10°C. Find the rate of conduction of heat by the ice per unit square centimetre area. (Given the Thermal conductivity of ice) = 5 x 10^-3 c.g.s unit)
Answer:

Given

A pond is covered with ice 5cm. thick and the temperature of overlying air is -10°C.

k =5 x 10^-3 c.g.s unit, A = 1 cm²,

x = 5cm, θ₂-θ₁, 0-(-10)

or 10°C.

Rate conduction of heat \(\frac{Q}{t}\)

\(=\frac{\mathrm{KA}\left(\theta_2-\theta_1\right)}{\mathrm{X}}=\frac{5 \times 10^{-3} \times 1 \times 10}{5} \mathrm{cal} / \mathrm{s} .\)

Physics Class 10 WBBSE Question 13. At what temperature will the volume of a given mass of gas be double of what is at 30°C, if the pressure remains constant?
Answer:

Let, t°C = the required temperature

Applying Charles’s law,

\(\frac{\mathrm{V}}{\mathrm{V}^1}=2=\frac{273+\mathrm{t}}{273+30}\) \(2=\frac{273+t}{303}\)

273+ t = 606

t=333°C

Question 14. The volume of a liquid is 830 m³ at 30°C and it is 850 m3 at 90°C. Find the coefficient of volume expansion of the liquid.
Answer:

Given

The volume of a liquid is 830 m³ at 30°C and it is 850 m3 at 90°C.

If V₁ and V₂ are the volume of a liquid at temperatures t1°C and t°C respectively.

\(y=\frac{\text { Increase in volume }}{\text { Original volume } \times \text { Rise in temperature }}=\frac{V_2-V_1}{V_1\left(t_2-t_1\right)}\)

[V₁ = 830m³, t₁= 30C, V₂ = 850m3, t² = 90c]

\(y=\frac{850-830}{830(90-30)}=\frac{20}{830 \times 60}=4 \times 10^{-4 /{ }^{\circ} \mathrm{C}}\)

Physics Class 10 WBBSE Question 15. The coefficient of cubical expansion of as metal is 7.2×10-5 °C^-1. Find the

1. Coefficient of linear expansion
2. Coefficient of superficial expansion. (Given = 7.2 × 10-5/°C)
   Answer:

1. Coefficient linear expansion

\(\alpha=\frac{1}{3} y=\frac{1}{3} \times 7.2 \times 10^{-5}=2.4 \times 10^{-5} /{ }^{\circ} \mathrm{C}\)

2. Coefficient of superficial expansion

\(\beta=\frac{2}{3} y=\frac{2}{3} \times 7.2 \times 10^{-5}=4.8 \times 10^{-5} /{ }^{\circ} \mathrm{C}\)

Question 16. The base of an iron saucepan has a diameter of 20 cm at 15°C. What will be the increased area of the base of the saucepan when it is filled with boiling water? (Given the coefficient of linear expansion of iron 12 x 10^-6 °C)
Answer:

Given

The base of an iron saucepan has a diameter of 20 cm at 15°C.

The radius of the base = 20/2 cm = 10 cm.

S₂ – S₁ = S₁ x B x (t₂ – t₁), the formula is necessary to define the coefficient of surface expansion.

S₁ = π x 10² Cm², β = 2α = 2 x 12 × 10^-6 per°C

(t₂ – t₁) (100 – 15)°C = 85°C

the required increase in area = (π x 10² x 24 x 10-6 × 85)

= 0.6404 Cm².

Question 17. The coefficient of apparent expansion of a liquid is 18 x 10-5°C when an iron vessel is used and 14.46 x 10-5°C when an aluminium vessel is used. If the coefficient of iron be 12 x 10-6/0C. Find that of aluminium.
Answer:

Given

The coefficient of apparent expansion of a liquid is 18 x 10-5°C when an iron vessel is used and 14.46 x 10-5°C when an aluminium vessel is used. If the coefficient of iron be 12 x 10-6/0C.

The coefficient of volume expansion of iron = 8 × 12 × 10^-6 °C

= 3.6 × 10^-5 °C.

The coefficient of real expansion of the liquid is given by

Yr = (18 x 10-5 +3.6 x10^-5 )/°C

= 21.6 x 10^-5C

If the coefficient of linear expansion of aluminium is a, then

21.6 x 10^-5 = 14.46 x 10^-5 + 3α

\(\alpha=\frac{7.14}{3} \times 10^{-5 /{ }^{\circ} \mathrm{C}}\)

= 2.33 x 10^-5/°C

Class 10 Physical Science WBBSE Chapter 3 Chemical Calculations Broad Answer Type Questions

Question 1. What steps should be followed to solve a problem based on the chemical equation by the weight-weight method?
Answer:

The following steps are followed :

• First, write down the complete balanced chemical equation.
• The molecular weight of the reactants and products is to be calculated from their respective formulae by adding the atomic weights of the concerned elements.
• The unknown weight of the substance asked for in the question is to be calculated from the calculated weight in the equations
• The same units are to be used for all quantities.

Question 2. What is the information available from the formula CaCO₃?
Answer:

The formula CaCO₃ conveys the following information :

• It stands for calcium carbonate.
• It tells that calcium carbonate is composed of calcium, carbon, and oxygen elements.
• It represents a molecule of calcium carbonate.
• It represents that a molecule of calcium carbonate is made up of one atom each of calcium and carbon and three atoms of oxygen.
• It stands for 100 parts by weight of calcium carbonate i.e. its molecular weight and signifies that the ratio of calcium, carbon, and oxygen by weight in it is 40:12:48.

Question 3. What is meant by the balancing of a chemical equation? Why it is necessary?
Answer:

Balancing of a chemical equation: It means making both sides of the equation equal with respect to the kind and number of the atoms of the elements involved.

Balancing of a chemical equation is necessary: Due to the conservation of mass and indestructibility of matter, no atoms can be created or destroyed in a chemical reaction Hence, The same kind of atoms in the same numbers must be present on both sides of the chemical equation.

Question 4. Write the following as balanced equations.

Cu+HNO₃ → Cu (N0₃) + O₂

Pb (N0₃)₂ → PbO + NO₂ + O₂

Al + NaOH + H₂O → NaAlO₂ + H₂

CuO + NH₃ → Cu + N₂ + H₂O

Answer:

Balanced equations are:

3Cu + 8HNO₃ = 3Cu (NO₃)₂  + 2NO – 4H₂O

2Pb (NO₃)₂  = 2pb0+ 4NO₂ +O₂

2Al + 2NaOH + 2H₂O = 2NaAIO₂ + 3H₂

2NH₃ +3CuO = 3Cu + 2n₂ + 3H₂0

Question 5. What are the limitations of a chemical equation?
Answer:

Limitation of a chemical equation :

Under what conditions a chemical reaction occurs i.e. pressure, temperature, catalyst are not-known.

• A reaction whether exothermic or endothermic is not known from a chemical equation.
• The chemical equations cannot provide information about the completion of the reaction or the attainment of equilibrium.
• A chemical equation does not give any idea about the reversibility of the reaction.
• From the chemical equation, the time required for the completion of the equation is not known.
• A reaction whether slow or fast is not known from the equation.
• The equation does not provide information regarding the nature of the reactants and products viz. solid, liquid, or gas.

Question 6. Balance the equation KCI0₃ → KCI + O₂ by trial and error method.
Answer:

KCI0₃ KCI + O₂: It is seen that the number of atoms of oxygen on the left-hand side is 3 whereas in the right-hand side it is 2. To equalize the number of atoms of oxygen on both sides it requires to multiply KCIO₃ by 2 and oxygen by 3.

2KCIO₃ → KCI +30₂ SO as to balance this equation if KCI is multiplied by then the equation is proper balance the equation if KCI is multiplied by 2 then the equation is proper. balanced.

2KCIO₃ = 2KCI + 30₂

Question 7. What information is obtained from the chemical equations?
Answer:

A chemical equation gives the following information:

1. Qualitative informations:

• From the chemical equation, the naming of elements and compounds taking part in the reaction and also the products are known.
• From the chemical equation, the symbols and the formulae of the reactants and products are also known.

2. Quantitative information:

• A number of atoms or molecules of the reactants and products involved in the reaction are known.
• How many parts of elements and compounds take part in the reaction and production is also known.
• If the reactants and products are all gaseous then at the same temperature and pressure. The ratio in volumes is known.

Question 8. Explain the method of balancing a chemical equation by trial and error method.
Answer:

Balancing of a chemical equation by trial and error method :

• In the method, the proper numbers are put before reactants and products so that the number of atoms on both sides is equal.
• In doing so, we must be cautious to see that all the reactants and products exist as molecules and not as atoms as the free existence of atomic is not possible.

Class 10 Physical Science WBBSE

Question 9. What is the method of writing chemical equations?
Answer:

Method of writing chemical equation :

Initially, the symbols of atoms of elements and formulae of molecules of reactants and products are written.

• Symbols and formulae of the reactants are written on the left side and those for products are on the right side. An arrow (→) is placed between reactants and products. For more than one reactants and product a plus sign (+) is to be given between the reactants and also between the products.
• The number of atoms of the reactants on the left-hand side must be equal to the number of atoms of the products on the right-hand side so as to maintain the law of conservation of mass. To equalize both sides, proper multiplication is required so that the number of atoms on both sides are same.
• Now the equation is expressed by replacing the arrow sign with a sign of equal (=).

Question 10. What information is obtained from the equation: 3H₂ + N₂ = 2NH₂
Answer:

The following information is obtained from the equation: 3H₂+N₂ = 2NH₂

Qualitative information: The reactants are hydrogen and nitrogen, and ammonia is the product.

Quantitative information :

• Three molecules of hydrogen combine with one molecule of nitrogen to produce two molecules of ammonia.
• Three volumes of hydrogen and one volume of nitrogen combine to produce two volumes of ammonia at the same temperature and pressure and their ratio is 3:1:2.
• Three moles of hydro and one mole of nitrogen combine chemically to produce two moles of ammonia.

Question 11. What information is obtained from the equation? C + O₂ = CO₂
Answer:

The following information is obtained from an equation: C + O₂= CO₂

Qualitative informations :

• From the above equation, it is known that carbon combines with oxygen producing carbon dioxide.
• Their respective symbols and formulas are also known

Quantitative information:

• One carbon atom combines with one oxygen molecule producing one carbon dioxide molecule.
• Hence the total number of atoms on the left-hand side is (1+2) = 3 and the number of atoms on the right-hand side is also 3.
• One gram-atom carbon reacts with one gram-molecule of oxygen giving rise to one gram-molecule of carbon dioxide.
• 12g carbon combines with 32g oxygen yielding 44g carbon dioxide.
• Hence, the total mass on the left-hand side (12+32) g = 44g is equal to the total mass on the right-hand side 44g. It proves the law of conservation of mass.
• Again 12g carbon combines with 32g oxygen producing 22.4 litre of carbon dioxide at STP.

Question 12. How many grams of oxygen evolve when 122.5g potassium chlorate is heated? (Given K = 39, CI = 35.5 0 = 16)
Answer:

The balanced equation is : \(\begin{array}{ll}
2 \mathrm{KClO}= & 2 \mathrm{KCl}+3 \mathrm{O}_2 \\
2(39+35.5+3 \times 161 \mathrm{~g} & 3[2 \times 16] \mathrm{g} \\
=245 \mathrm{~g} & =96 \mathrm{~g}
\end{array}\)

By heating 245g KCIO₃ 96g O₂ is obtained

∴ By heating 122.5g KCIO₃ \(\frac{96 \times 122.5}{245} \mathrm{~g}\) is obtained.

Physics Class 10 WBBSE

Question 13. 2.6g zinc is treated with excess dil H₂SO₄ How many grams of oxygen combine with the evolved hydrogen?
Answer:

The balanced equation for the production of hydrogen is:

\(\underset{65 \mathrm{~g}}{\mathrm{Zn}}+\mathrm{H}_2 \mathrm{SO}_4=\mathrm{ZnSO}_4+\underset{(2 \times 1) \mathrm{g}=2 \mathrm{~g}}{\mathrm{H}_2}\)

So, 65g of Zinc produces 2g of hydrogen

∴ 2-6 Zinc produces \(\frac{2 \times 2.6}{65} \mathrm{~g}=0.089\) hydrogen

Now, the reaction where hydrogen and oxygen combine is: 2H₂ + O₂ = 2H₂O

So, 4g hydrogen combined with 32g oxygen

0.08g hydrogen combined with \(\frac{32 \times 0.08}{4} \mathrm{~g}=0.64 \mathrm{~g}\)

Question 14. What is the observed loss in weight of 5g? calcium carbonate when it undergoes thermal decomposition?
Answer:

The balanced equation is : \(\begin{aligned}
& \mathrm{CaCO}_3=\mathrm{CaO}+\mathrm{CO}_2 \\
& (40+12+16 \times 3) \mathrm{g}(12+16 \times 2) \mathrm{g} \\
& =100 \mathrm{~g} \quad=44 \mathrm{~g} \\
&
\end{aligned}\)

Loss in weight in the weight of CO₂ that escapes 100g CaCO₃ produces 44g CO₂

∴ 5g CaCO₃ produces \(\frac{44 \times 5}{100} \mathrm{~g}=2.2 \mathrm{gCO}_2\)

Question 15. What is the percentage of ammonia in that quantity of ammonium chloride that can produce 5g? ammonia?
Answer:

The balanced equation is :

\(\begin{aligned}
& 2 \mathrm{NH}_4 \mathrm{Cl}+\mathrm{CaO}=2 \mathrm{NH}_3+\mathrm{CaCl}_2+\mathrm{H}_2 \mathrm{O} \\
& 2[14+1 \times 4+35.5)_{\mathrm{g}} 2[14+1 \times 3]_{\mathrm{g}} \\
& =107 \mathrm{~g}
\end{aligned}\)

So, 34g ammonia is obtained from 107g NH₂CI.

Question 16. What weight of potassium chlorate of 96% purity will yield 4.8g oxygen on complete thermal decomposition? (Given, K = 39, CI = 35.5, O = 16)
Answer:

The balance equation is: 2KCIO₃ (245g) = 2KCI + 3O₂(96g)

∴ 96g oxygen is obtained from 245g KCIO₂ of 100% purity.

∴ 4.8g oxygen is obtained from \(\frac{245 \times 4.8}{96} \mathrm{~g}\)

Let x gram of 96% purity contain 12.25g KCIO₃ of 100% parity

∴ \(\frac{96}{100} \times 12.56 \text { or, } x=\frac{12.25 \times 100}{96}=12.76 \text { (approx) }\)

So, the required quantity of KCIO₃ = 12.76g

Physics Class 10 WBBSE

Question 17. On strong heating, limestone decomposes into quicklime and carbon dioxide. How much quantity of limestone will produced on complete decomposition, 30g of quicklime by the above reaction?
Answer:

The balanced equation is: \(\begin{array}{ll}
\mathrm{CaCO}_3=\mathrm{CaO}+\mathrm{CO}_2 & \\
(40+12+3 \times 16) \mathrm{g} & {[40+16] \mathrm{g}} \\
=100 \mathrm{~g} & =56
\end{array}\)

So 56g, CaO is obtained by the complete decomposition of 100g CaCO₃

∴ 30g CaO is obtained by the complete decomposition of \(\frac{100 \times 30}{56} \mathrm{~g} \mathrm{CaCO}_3=53.6 \mathrm{~g} \mathrm{CaCO}_3\)

Thus 53.6g of limestone will have to be decomposed.

Question 18. How many grams of magnesium metal will give 1.2g hydrogen in a complete reaction with dilute H₂SO₄ (Mg= 24, H = 1) The balanced equation is:
Answer:

\(\begin{aligned}
\mathrm{Mg}+\mathrm{H}_2 \mathrm{SO}_4= & \mathrm{Mg} \mathrm{SO}_4+\mathrm{H}_2 \\
24 \mathrm{~g} & (1 \times 2) \mathrm{g}=2 \mathrm{~g}
\end{aligned}\)

So 2g H₂ is obtained from 24g Mg

∴ 1.2g H₂ is obtained from \(\frac{24 \times 1.2}{2} \mathrm{~g} \mathrm{Mg}=14.4 \mathrm{gMg} .\)

So, 14.4g will be required

Question 19. Calculate the number of moles in 1.5 gm of ammonia.
Answer:

We know, number of mole = \(\frac{\text { Mass given }}{\text { gram molecular mass }}\)

\(\begin{aligned}
& =\frac{1.5}{1.7} \\
& =0.88
\end{aligned}\)

Question 20. The vapor density of a gas is 40. Calculate the volume of 20 gm of this gas at 27°C and 950 mm pressure.
Answer:

Given

The vapor density of a gas is 40.

The molecular weight of the gas = 2 x vapor density

= 2 × 40 = 80

The volume of 80 gm of gas at S.T.P. is 22.4 Lit

The volume of 10 gm of gas at S.T.P.

\(=\frac{22.4 \times 10}{80}=2.8 \mathrm{Lit}\)

Let the volume of this 2.8 liter of gas at 27°C and 950 mm pressure be V Litre

\(\frac{\mathrm{V} \times 950}{273+27}=\frac{2.8 \times 760}{273}\)  ⇒V = 7.79 Litre

Hence the volume of the gas at 27°C and 950 pressure is 4.9 Litre.

WBBSE Class 10 Physical Science Solutions Chapter 2 Behaviour Of Gases Long Answer Type Questions

Question 1. Establish-relation between the pressures and density of a gas at a constant temperature.
Answer:

Relation between the pressures and density of a gas at a constant temperature

Let the volume of the mass m of gas at a constant temperature be V₁ when the pressure is P₁ and V₂ when the pressure is P₂.

From Boyle’s law, P₁ V₁ = P₂ V_{2 →}(1)

Let the densities of the gas at the pressure P₁ and P₂ be P₁ and P₂ respectively. Substituting in equation (1) we get,

\(\frac{P_1 m}{P_1}=\frac{P_2 m}{P_2}\)

\(\frac{P_1}{P_1}=\frac{P_2}{P_2}\) ⇒ Ρ α Ρ

The density of a gas at constant temperature is proportional to pressure.

Question 2. What are the characteristic properties of gases?
Answer:

Characteristic properties of gas:

1. Shape and Volume: Since particles of gases are not held in fixed positions and move freely, gases neither have definite shapes nor definite volumes.
2. Homo generous nature: All parts of a gas or a gaseous mixture have similar composition throughout.
3. Density: Due to the large separation of molecules, gases have large volumes and thus low density.
4. Compressibility: On increasing pressure gases can be readily compressed due to the presence of large empty spaces.
5. Random motion: The molecules or atoms of a gas are in a state of continuous zig-zag motion in all directions.
6. Pressure: Due to their random motion, the molecules of the gas collide on the walls of the container and thus exert a certain force on the walls of the container. The force per unit area is called the gas pressure.
7. Diffessure: Gases mix (diffuse) with each other freely due to the free movement of their molecules.
8. Liquefaction: On cooling and applying. Pressure and gases can be liquefied. However, gas has to be cooled below a certain characteristic temperature called critical temperature before it can be liquefied by the application of pressure alone.

Question 3. What are the postulates of the kinetic theory of gases?
Answer:

Postulates of Kinetic theory of gases :

1. All gases consist of a very large number of tiny particles called molecules that are in constant rapid motion.
2. The gas molecules are perfectly round, very hard and separated by large distances. Their actual volume is thus, negligible as compared to the total volume of the gas.
3. The collisions between the gas molecules are perfectly elastic, i.e. there is no loss of energy during these collisions.
4. The distance between gas molecules being very large, there is no effective force of attraction or repulsion between them.
5. The average kinetic energy of the gas molecules is directly proportional to the absolute temperature of the gas.
6. The gas molecules collide with one another and with the walls of the container. The pressure exerted by a gas is due to the bombardment of its molecules on the walls of the vessel.
7. The gas molecules move freely in all directions. Their speed and direction change continuously due to collisions among them. As a result, their motion becomes zig-zag or random.

WB Class 10 Physical Science Question Answer

Question 4. A sample of helium has a volume of 520 cm3 at 373 k. Calculates the temperature at which the volume will become 260 Cm³. Assume that the pressure is constant.
Answer:

Given

A sample of helium has a volume of 520 cm3 at 373 k.

According to Charle’s law,

 

 

 

 

 

Question 5. Find the volume of N, at 27°C at a pressure of 760 torr, if it occupies 40 mL at STP.
Answer:

Given

at 27°C at a pressure of 760 torr, if it occupies 40 mL at STP.

According to Charle’s law,

 

 

 

 

 

Question 6. A sample of oxygen has a volume of 880 mL and a pressure of 740 torr. What additional pressure is required to reduce the volume to 440mL?
Answer:

Given

A sample of oxygen has a volume of 880 mL and a pressure of 740 torr.

According to Boyle’s law,

 

 

 

 

 

Question 7. 7.0g of a gas at 300K and 1 atmospheric pressure occupies a volume of 4.1 litters. What is the molecular mass of the gas?
Answer:

Given

7.0g of a gas at 300K and 1 atmospheric pressure occupies a volume of 4.1 litters.

Applying the ideal gas equation,

 

 

 

 

 

 

Question 8. A steel tank contains carbon dioxide at 27°C and a pressure of 10.0 atm. Calculate the internal gas pressure when the tank and the gas are heated to 100°C.
Answer:

Given

A steel tank contains carbon dioxide at 27°C and a pressure of 10.0 atm.

According to Gay Lussac’s law,

 

 

 

 

 

Question 9. A bottle of Volume 1 litre contains gas at 10 atmospheric pressure. How many bottles each of a 1-litre capacity can be filled with the gas at 2 atmospheric pressure at constant temperature?
Answer:

Given

A bottle of Volume 1 litre contains gas at 10 atmospheric pressure

According to Boyle’s law

WB Class 10 Physical Science Question Answer

Question 10. The volume of a certain mass of gas at 400k and pressure 202600 pascal is 2 cubic metres. What would be the volume of the gas at 327°C and 152cm of mercury Pressure? [given 1.013 x 10⁵ Pascal 1 atmospheric pressure]
Answer:

Given

The volume of a certain mass of gas at 400k and pressure 202600 pascal is 2 cubic metres.

According to Charle’s law

Question 11. An iron cylinder contains helium at a pressure of 250 K pa at 300k. The cylinder can withstand a pressure of 1×10⁶ pa. The room in which the cylinder is placed catches fire. Predict whether the cylinder will blow up before it melts or not. (M.P. of the cylinder 1800K)
Answer:

Given

An iron cylinder contains helium at a pressure of 250 K pa at 300k. The cylinder can withstand a pressure of 1×10⁶ pa. The room in which the cylinder is placed catches fire.

According to Gay-Lussac’s law.

 

 

 

 

 

Question 12. A certain quantity of gas occupies a volume of 1000 cm3 at 760 mm and 27°C. Find the volume of the gas if the pressure and temperature are 1520 mm and 327°C.
Answer:

Given

A certain quantity of gas occupies a volume of 1000 cm3 at 760 mm and 27°C.

By combining Boyle’s low and Charle’s low we get.

 

 

 

 

 

Question 13. A gas having a temperature 0°C is heated so that its pressure and volume are doubled. What will be the final temperature of the gas?
Answer:

Given

A gas having a temperature 0°C is heated so that its pressure and volume are doubled.

By combining Boyle’s low and Charle’s low we get

 

 

 

 

 

Question 14. 10g of Oxygen are introduced in a vessel of 5 lit capacity at 27°C calculate the pressure of the gas in the atmosphere in the container.
Answer:

Given

10g of Oxygen are introduced in a vessel of 5 lit capacity at 27°C

Applying the ideal gas equation,

 

 

 

 

 

Question 15. The volume of 1 gram mole of oxygen gas is 22400 ml at 760 mm. Calculate the temperature of the gas (Given R = 0.082L-atm mol^-1 K^-1)
Answer:

Given

The volume of 1 gram mole of oxygen gas is 22400 ml at 760 mm.

We know from the ideal gas equation for 1 mole of an ideal gas.

 

 

 

 

 

 

Question 16. Establish the equation:

\(V-t=V_0\left(1-\frac{t}{273}\right)\)
Answer:

Let, Vo denote the volume of a given mass of a gas at 0°C and Vt be the volume of the same mass of the gas at t°C, the pressure in both cases is the same.

From Charle’s law,

The increase in volume of the gas = \(\frac{\text { Volume at } 0^{\circ} \mathrm{C}}{273} \times \text { rise in temperature }\)

∴ \(V_t=V_0+\frac{V_0}{273} \times t\)

\(V_t=V_0\left(1-\frac{t}{273}\right)\)

If we consider a temperature lower than 0ºC, say tºC, then the volume of gas is \(v_{-1}=V_0\left(1+\frac{t}{273}\right)\)

WBBSE Class 10 Physical Science Solutions

Question 17. Establish: \(\frac{P}{T}=a\)constant for pressure law.
Answer:

If the pressure of a given mass of a gas at temperature t°c and the by P and P’ respectively, then volume remains constant.

We have Pressure law,

\(P=P o\left(1+\frac{t}{273}\right)=\frac{P o T}{273}\) \(p^{\prime}=P_0\left(1+\frac{t^{\prime}}{273}\right)=\frac{P_{o T}}{273}\)

Po = pressure of the gas.

TK = absolute temperature corresponding to the temperature t°c.

T1K= absolute temperature to the temperature t1 °C

\(\frac{P}{P^{\prime}}=\frac{T}{T^{\prime}} \)  ⇒ \(\frac{P}{T}=\frac{P^{\prime}}{T^{\prime}}\)

⇒ \(\frac{P}{T}\)= Constant when V = constant

∴ P α T

Question 18. Establish the relation PV KT for an ideal gas.
Answer:

Let, P = pressure of a gas

V = Volume of a gas

T= absolute temperature

From Boyle’s law,

\(V \propto \frac{1}{P}\) (T = Constant)

From Charle’s law,

V α T (P= constant)

When P and T both vary

\(V \propto \frac{T}{P}\)

⇒ \(V=K \frac{T}{P}\)

\(\frac{P V}{T}=K\)

PV = KT

Question 19. What is the general equation is obtained by combining Boyle’s law and Charle’s law. Define-universal gas constant. The general equation is obtained by combining Boyle’s law and Charles’s law.
Answer:

\(\frac{P_1 V_1}{T_1}=\frac{P_2 V_2}{T_2}\)

P₁ = Pressure of first gas

P₂ = pressure of second gas

V₁ = Volume of the first gas

V₂ = Volume of the second gas

T₁ = temperature of the first gas

T₂ = temperature of the second gas

Universal gas constant: One gram molecule of all gases occupy the same volume under identical conditions of temperature and pressure the volume of R is the same for all gases R is known as the universal gas constant.

WBBSE Class 10 Physical Science Solutions

Question 20. Establish a Relation between the pressure, temperature and density of a gas.
Answer:

Relation between the pressure, temperature and density of a gas

Let, P = Pressure of a gas

V = Volume of a gas

T = temperature of a gas

P= density of a gas

m = mass of a gas

M = Molecular weight of the gas

From the ideal gas equation,

\(\frac{P V}{T}=\frac{m}{M} R\) [R= universal gas constant]

\(\frac{\mathrm{PV}}{\mathrm{mT}}=\frac{\mathrm{R}}{\mathrm{M}}\) = Constant

But, \(\mathbf{P}=\frac{\mathbf{M}}{\mathbf{V}}\)

\(\frac{\mathbf{P}}{\mathrm{PT}}\)

 

Question 21. Why the absolute zero of temperature is called absolute?
Answer:

• We have seen that the concept of absolute zero of temperature is regardless of the kind, amount and initial pressure or volume of the gas. It is not possible to attain a temperature lower than this.
• But in other scales of temperature in the Celsius scale, the concept of 0°C depends on the behaviour of a particular material such as water. Temperature lower than 0°C are possible.
• So, the concept of absolute zero is more universal and more fundamental. Hence it is termed absolute.

Question 22. Explain the relation between the pressure-volume of a gas-When the temperature is kept constant.
Answer:

Relation between the pressure-volume of a gas-When the temperature is kept constant

• Pressure is increased.
• When the temperature of a fixed mass of a gas is kept constant and the pressure is increased systematically the volume correspondingly increases.
• Pressure is decreased.
• When the temperature of a fixed mass of a gas is kept constant and the pressure is decreased systematically the volume correspondingly increases.

Question 23. Explain the relation between temperature and volume of gas When the pressure is kept constant.
Answer:

Relation between temperature and volume of gas When the pressure is kept constant

• Temperature increased
• When the pressure of a fixed mass of gas is kept constant and the temperature of the gas is increased systematically the volume correspondingly increases.
• Temperature decreased:
• When the pressure of a fixed mass of gas is kept constant and the temperature of the gas is decreased slowly the volume correspondingly decreases.

Question 24. Write four assumptions of the kinetic theory of gases.
Answer:

Four assumptions of the kinetic theory of gases:

1. All gases are made of molecules moving randomly in all directions.
2. The size of a molecule is much smaller than the average separation between the molecules.
3. The molecules exert no force on each other or on the walls of the container except during collision.
4. The molecules obey Newton’s Laws of Motion.

Question 25. Establish: Vr ms = \(\sqrt{\frac{3 \mathrm{PV}}{\mathrm{M}}}\)
Answer:

The square root of mean square speed is called the root mean square speed or rms speed.

\(\mathrm{Vrms}=\sqrt{\Sigma v^2 / N}\)

V^{2 = (Vrms)}

We know that, P = \(\frac{1}{3} \mathrm{PV}^2 \mathrm{rms}\)

\(\text { Vrms }=\sqrt{\frac{3 p}{p}}=\sqrt{\frac{3 P V}{M}}\)

WBBSE Class 10 Physical Science Solutions

Question 26. Explain briefly the translational kinetic energy of a gas.
Answer:

The total translational kinetic energy of all the molecules of the gas is

\(K=\Sigma \frac{1}{2} m V^2\)

= \(\frac{1}{2} m \mathrm{~N} \frac{\Sigma \mathrm{V}^2}{\mathrm{~N}}\)

= \(\frac{1}{2} \mathrm{Mv}^2 \mathrm{rms}\)

The Average kinetic energy of a molecule

\(\frac{K}{N}=\frac{1}{2} \frac{M}{N} V^2 \mathrm{rms}\)

We know, \(\mathrm{pV}=\frac{1}{2} \mathrm{MV}^{-2}\) → (1)

From equation → (1)

\(\mathrm{pV}=\frac{2}{3} \frac{1}{2} \mathrm{Mv}^2 \mathrm{rms}\) \(p V=\frac{2}{3} K\) \(K=\frac{3}{2} p V\)

 

Question 27. State Avogadro’s law
Answer:

Avogadro’s law: At the same temperature and pressure, equal volumes of all gases contain equal numbers of molecules. This is known as Avogadro’s law.

Question 28. Establish Avogadro’s law.
Answer:

Avogadro’s law

Consider equal volumes of two gases kept at the same pressure and temperature.

m₁ = mass of a molecule of the first gas

m₂ = mass of a molecule of the second gas

N₁ = number of molecules of the first gas

N₂ = number of molecules of the second gas

P = Common pressure of the two gases

V = Common pressure of the two gases

∴ \(p V=\frac{1}{3} N_1 m_1 V_1^2\)

\(P V=\frac{1}{3} N_2 m_2 V_2\)

_{V1 V2} = rms speeds of the molecules of the first and second gas

\(N_1 m_1 V_1^2=N_2 m_2 V_2^2\) → (1)

As the temperature of the gases is the same, the average kinetic energy of the molecules is the same for the two gases.

\(\frac{1}{2} m_1 v_i==\frac{1}{2} m_2 v_2=\) → (2)

From, (1) and (2)

N₁ = N₂ Avogadro’s law

Question 29. Establish the relation: Dalton’s law of partial pressure: P=P, +P,+P, +……..
Answer:

In kinetic energy, the pressure exerted by a gas on the walls of a container is due to the collisions of the molecules of the walls.

The total force on the wall is the sum of the forces exerted by the individual molecules.

Suppose there are N₁ molecules of gas

1, N₂ molecules of gas 2 in the mixture.

The force on a wall of surface area A,

F= force by N₁ molecules of gas 1+ force by N₂ molecules of gas 2 + ….. = F+F+…

The pressure, \(P=\frac{F_1}{A}+\frac{F_2}{A}+\ldots \ldots\)

If the first gas alone is kept in the container, its N₁ molecules will exert a force F₁ on the wall.

If the pressure in this case P₁ , P₁ = \(\frac{F_1}{A}\)

Similar is the case for other gases Thus, P = P₁+P₂+P₃ +…

Question 30. Prive : \(\frac{r_1}{r_2}=\sqrt{\frac{p_2}{p_1}}\) for Graham’s law of diffusion.
Answer:

The rate of diffusion is proportional to the rms speed of the molecules of the gas.

If r₁ and r₂ be the rates of diffusion of the two gases,

\(\frac{r_1}{r_2}=\frac{V_1, r m s}{V_2, r m s}\) → (1)

\(\text { Vrms }=\sqrt{\frac{3 p}{P}}\)

If the pressure of the two gases is the same

\(\frac{\mathrm{V}_1, \mathrm{rms}}{\mathrm{V}_2 \mathrm{rms}}=\sqrt{\frac{\mathrm{p}_2}{\mathrm{p}_1}}\)

From equation → (1),

\(\frac{r_1}{r_2}=\sqrt{\frac{p_2}{p_1}}\) ..Graham’s law of diffusion

WBBSE Class 10 Physical Science Question Answer In English

Question 31. Prove Ideal gas equation ⇒ PV = nRT
Answer:

Consider a sample of an ideal gas at pressure P, volume V and temperature T.

Let, m = the mass of each molecule

V = rms speed of the molecule

Vtr = rms speed of the gas at the triple point 273. 16K

R = NaK = universal point

= universal gas point

R = 8.314 J K^-1 mol^-1

This is known as the equation of state of an ideal gas.

Question 32. Write the mathematical form of Max Well’s speed distribution law.
Answer:

The mathematical form of Maxwell’s speed distribution law :

\(d N=r \pi N\left(\frac{m}{2 \pi K T}\right)^{\frac{3}{2}} V^2 e^{-m V^2 / 2 K T}\)

 

Question 33. Write the mathematical expression of Vander Waal’s equation.
Answer:

The mathematical expression of the van der Waals equation.

\(\left(P+\frac{a}{V^2}\right)(V-b)=n R T\)

[a, b = constant

a = average force of attraction between the molecules

b = total volume of molecules]

1. A given sample of a substance has a number of parameters which can be physically measured. When these parameters are uniquely specified. So we say that the thermodynamic state of the system is specified.

We know. \(p V=\frac{1}{3} \mathrm{NmV}^2\) →(1)

\(\mathrm{T}=\left(\frac{273.16 \mathrm{k}}{\mathrm{V}^2 \mathrm{tr}}\right) \mathrm{V}^2\) \(V^2=\left(\frac{V_2 {tr}}{273.16 k}\right) T\)

Putting this Expression for V² in q^{n →}(1)

\(\mathrm{pV}=\mathrm{N}\left(\frac{1}{3} \frac{\mathrm{mV}^2 \mathrm{tr}}{273.16 \mathrm{k}}\right) \mathrm{T}\)

\(\frac{1}{2} \mathrm{mV}_{\mathrm{tr}}^2\) = average kinetic energy of a molecule at the triple point 273.16K.

As the average kinetic energy of a molecule is the same for all gases at a fixed temperature, mV2 tr is a universal constant. Accordingly. The quantity in the bracket in the equation.

2. above is also a universal constant writing this constant as a k equation.

3. becomes.

pV = NKT → (3)

The Universal constant K = Boltzmann Constant The value of K = 1.38 x 10^-23 JK^-1

If the gas contains n moles, the number of molecules is N = n^X_A

(NA 6.02 x 10²³mol^-1)

NA Avogadro’s Constant

Using eq (3) becomes p = x^N_A KT

PV = nRT → (4)

Question 34. Draw the graph Pressure (P) and volume (V) at a constant temperature.
Answer:

 

 

 

 

 

 

 

Chapter 1 Concerns About Our Environment Broad Answer Type Questions

Question 1. What is good fuel?
Answer:

Good fuel: Good fuel should have many desirable characteristics. Some of these are as follows:

1. It should produce a high amount of energy for each limit of mass or volume.
2. It should be easily available and should be easy to transport.
3. It should be economical.

Question 2. What are the advantages of nuclear energy?
Answer:

The advantages of nuclear energy

The advantages of nuclear energy are as follows: A small amount of radioactive material can generate a huge amount of energy. It does not produce air pollution. A nuclear power plant is more efficient than other power plants.

Question 3. Hydrogen has been used as a rocket fuel would you consider it a cleaner fuel than LPG? Why and why not?
Answer:

Hydrogen is a much cleaner energy source than CNG. CNG is derived from biomass and hence burning the CNG causes air pollution, although on a much smaller scale than coal and petroleum. The use of hydrogen as an energy source does not pollute gases.

Question 4. Can any source of energy be pollution free? Why and why not?
Answer:

Many sources of energy can be pollution free when the burning of biomass is not involved in the production of energy, then there is no chance of pollution. For example, wind energy, solar energy, hydel energy, etc are pollution free.

Class 10 Physical Science WBBSE

Question 5. What are the limitations of the energy that can be obtained from the oceans?
Answer:

Limitations of energy that can be obtained from the oceans:

These forms of energy can be used only in coastal areas, which would leave a vast portion of human habitation. The technologies for using these energies are still at the experimental stage and hence are very costly and less efficient.

Question 6. Why are looking for an alternate source of energy?
Answer:

Because of the growing population, the energy demand is rising. Fossil fuels are going to be exhausted in the near future and burning them is causing air pollution. Hence, we need to find an alternate source of energy which renewable and environmentally friendly.

Question 7. How has the traditional use of wind and water energy been modified for our convenience?
Answer:

• Before the beginning of the Industrial Revolution, wind and water energy were used for serving many purposes but the ways of their use were not efficient. For example, windmills were used to power smaller mills like flour mills or sawmills.
• The flow of water was used for transporting wooden logs. Now a day, both wind energy and water energy are being widely used to produce electricity, which means better and more efficient use of these forms of energy.

Question 8. What kind of mirror, concave or convex, or plain would be best suited for use in a solar cooker? Why?
Answer:

Explanation: A concave mirror is best suited for use in a solar cooker. The reason for this is the ability of a concave mirror to converge the solar energy at a point. This enables the concave mirror to produce a larger amount of heat compared to other types of mirrors.

Question 9. Short Note-Ozone Layer.
Answer:

-Ozone Layer:

• The ozone layer is contained within the stratosphere. In this layer, ozone concentrations are about 2 to 8 parts per million which is much higher than in the lower atmosphere but very small compared to the main components of the atmosphere.
• It is mainly located in the lower portion of the stratosphere from about 15:35 km though the thickness varies seasonally and geographically. About 90% of the ozone in the Earth’s atmosphere is contained in the atmosphere.

Question 10. What is ultraviolet light? How can the ozone Layer deplete?
Answer:

Ultraviolet light:

Although the concentration of ozone in the ozone layer is very small. It absorbs biologically harmful ultraviolet radiation coming from the sun: Extremely short or vacuum UV is screened out by nitrogen. UV radiation is capable of penetrating nitrogen.

• The Ozone layer can be depleted by free radical catalysts including nitric oxide, hydroxyl, atomic chlorine, and atomic bromine. While there are natural sources for all of these species.
• The concentrations of chlorine and bromine increased markedly in recent decades due to the release of large quantities of man-made organohalogen compounds, especially chloroform carbons, and bromoform carbons.

Question 11. Short Note-Exosphere.
Answer:

Exosphere: The exosphere is the outermost layer of Earth’s atmosphere. It extends from the exobase, Which is Located at the top of the Thermosphere at an altitude of about 700 km. above sea level, to about 10,000 km.

The exosphere merges with the emptiness of outer space, where there is no atmosphere. This layer is mainly composed of extreme hydrogen, helium, and several heavier molecules including nitrogen, oxygen, and carbon dioxide closer to the exobase.

Question 12. Draw a diagram of a solar cell.
Answer:

Diagram of a solar cell

WB Class 10 Physical Science Question Answer

Question 13. Short Note. Thermosphere.
Answer:

Thermosphere:

The thermosphere is the second highest layer of Earth’s atmosphere. It extends from the Mesopause at an altitude of about 80 km. upto the thermopause at an altitude range of 500-1000km.

• The height of the thermopause varies considerably due to changes, in solar activity. This layer is completely cloudless and free of water vapor.
• However non-hydrometeorological phenomena such as aurora Borealis and aurora australis are occasionally seen in the thermosphere. The Internation Space Station orbits in this layer, between 320 and 380 km.

Question 14. Short Note-Mesosphere.
Answer:

Mesosphere:

The mesosphere is the third highest layer of Earth’s atmosphere, occupying the region above the stratosphere and below the thermosphere. It extends from the stratopause at an altitude of about 50 km. to the mesopause at 80-85 km above Sea level.

• Temperatures drop with increasing altitude to the mesopause that marks the top of this middle layer of the atmosphere. It is the coldest place on earth and has an average temperature around-85°C.
• The mesosphere is the layer where most meteors burn up upon the atmospheric entrance. It is too high above Earth to be accessible to aircraft and balloons and too low to permit orbital spacecraft. The mesosphere is mainly accessed by sounding rocks.

Question 15. Short Note-Stratosphere.
Answer:

Stratosphere :

The Stratosphere is the second lowest layer of Earth’s atmosphere. It lies above the troposphere and is separated from it by the tropopause. This layer extends from the top of the troposphere at 12km about the earth’s surface to the stratopause at an altitude of about 50 to 55 km.

• The atmospheric pressure at the top of the stratopause is 1/1000 the pressure at sea level. It contains the ozone layer, which is the part of Earth’s atmosphere that contains relatively high concentrations of gas.
• The stratospheric temperature profile creates very stable atmospheric conditions, So The layer lacks the weather-producing air turbulence that is prevalent in the troposphere.

Question 16. Short Note-Green House Effect.
Answer:

Green House Effect: The earth’s atmosphere is transparent to the visible light and infrared radiations of short wavelengths coming from the sun.

• The high-energy radiations (gamma rays. X-rays, Ultraviolet rays) are absorbed by the ozone layer while the low-energy radiations (infrared radiation) of long wavelengths and radiowaves are reflected back into space by the ionosphere.
• The solar radiations which pass through the atmosphere of the earth are absorbed by the clouds, earth, surface, and seawater due to which the earth’s surface gets heated up.
• Now earth’s surface radiates infrared radiations of long wavelengths, but these radiations are reflected back by the clouds and absorbed by the gases present in the atmosphere of the earth and thus the clouds and gases prevent them from escaping into space. Thus keeping the earth’s atmosphere warm.

WB Class 10 Physical Science Question Answer

Question 17. Briefly describe the thermal power plant.
Answer:

Thermal power plant :

A power plant in which the heat required to make steam to drive turbines is obtained by burning fuels is called a thermal power plant.

• Coal is burned in a furnace F to produce heat. This heat boils the water in a boiler B to form steam.
• The steam formed from the boiling water builds up. a pressure. The hot steam at high pressure is introduced into turbine chamber C having a steam (Picture) turbine T, The steam passes over the blades of the turbine as a high-pressure jet making the turbine rotate.
• The shaft S on cooling, stem condenses to form water. This water is again sent to the boiler to form fresh steam. The process is repeated again and again.
• Since it is easier to transmit electricity over long distances than to carry coal over the same distance, therefore, many thermal power plants are established near coal fields.
• We produce a major part of our electricity by burning fossil fuels. Due to this, large amounts of fossil fuels are being burnt every day at thermal power plants to generate electricity.
• Because our supplies of coal, oil, and gas are running out at a rapid rate and because of the pollution caused by burning fossil fuels, other ways of generating electricity must be found.
• Please note that electricity is not fuel. It is a form of energy. At thermal power plants. It is the chemical energy of fossil fuels that is transformed into electrical energy.

Question 18. What is the cause of global warming? What are the effects of global warming? Write the advantages of generating hydroelectricity.
Answer:

The cause of global warming :

• The concentration of chlorofluorocarbons has increased by 5% per year.
• The concentration of methane has doubled due to agricultural sources (vice cultivation, animal husbandry, natural gas exploration, burning of biogas)
• The concentration of carbon dioxide has increased up to 25% due to industrial growth, combustion of fossil fuel, and clearing of forests.

The effect of global warming :

• It will increase the frequency and intensity of extreme weather events (floods, droughts, heat waves, hurricanes) because of changes in the pattern of winds and ocean currents.
• It will result in low agricultural yield.

The advantages of Generating Hydroelectricity?

• The generation of electricity from flowing water does not produce any environmental pollution.
• The construction of dams on rivers helps in controlling floods, and in irrigation.
• Flowing water is a renewable source of electric energy that will never get exhausted.

Chapter 2 Behaviour Of Gases MCQs

Question 1. In the ideal gas equation PV = nRT, the value of R depends upon :

1. Unit of measurement
2. Temperature of gas
3. Pressure of gas
4. Nature of gas

Answer: 1. Unit of measurement.

Question 2. An ideal gas is one which :

1. Obeys gas laws
2. Obeys Boyle’s law
3. obeys Chaple’s law
4. Avogadro’s law

Answer: 1. Obeys gas laws.

Question 3. The volume of any gas at this temperature becomes zero :

1. + 273°C
2. – 273°C
3. 273K
4. 273K

Answer: 2. -273°C.

Question 4. P₁ V₁ = P₂ V₂ , is related to:

1. Boyle’s law
2. Charle’s law
3. Regnault’s law
4. None of these

Answer: 1. Boyle’s law.

WBBSE Class 10 Physical Science Question Answer In English

Question 5. Normal pressure is :

1. 1.013 x 106 dyne/cm²
2. 2.013 x 106 dyne/cm²
3. 1.05 x 10% dyne/cm²
4. 1.09 x 106 dyne/cm²

Answer: 1. 1.013 × 10% dyne/cm²

Question 6. The relation between the pressure, temperature and density of a gas is:

1. \(\frac{\mathrm{PT}}{\mathrm{D}}=\text { constant }\)
2. \(\frac{\mathrm{P}}{\mathrm{DT}}=\text { constant }\)
3. \(\frac{P D}{T}=\text { constant }\)
4. None of these

Answer: 2. \(\frac{\mathrm{P}}{\mathrm{DT}}=\text { constant }\)

Question 7. What will be the value of 127°C on the kelvin scale?

1. 127K
2. 400K
3. 146 K
4. 200 K

Answer: 2. 400K.

Question 8. The relation between Celsius and absolute scale is :

1. T = t + 273
2. T = t – 273
3. t=T+273
4. t = T 273

Answer: 1. T t + 273.

WBBSE Class 10 Physical Science Question Answer In English

Question 9. The boiling point of water in the Kelvin scale is :

1. OK
2. 373 K
3. 100 K
4. 273 K

Answer: 2. 373 K.

Question 10. For the liquefaction of gas, the favourable conditions are :

1. low temperature and low pressure
2. low temperature and a catalyst
3. low temperature and high pressure
4. low temperature, high pressure and a catalyst

Answer: 2. low temperature and high pressure.

Question 11. The pressure of real gases is less than the pressure of an ideal gas because of:

1. Increase in the number of collisions
2. Finite-size of the molecules
3. Increase in kinetic energy
4. Intermolecular forces

Answer: 4. Intermolecular forces.

Question 12. P, V, and T stand for the pressure, volume and temperature of a gas. Which of the following will express Boyle’s law?

1. V x T when P is constant
2. \(V \times \frac{1}{P} \text { when } T \text { is constant }\)
3. PV = RT
4. PV = nRT

Answer: 2. \(V \times \frac{1}{P} \text { when } T \text { is constant }\)

WBBSE Class 10 Physical Science Question Answer In English

Question 13. The number of gram molecules of oxygen is 6.02 × 1024 Co molecules is:

1. 8g molecules
2. 5g molecules
3. 2g molecules
4. 0.5g molecules

Answer: 2. 5g molecules.

Question 14. The volume of 4.4g of CO₂ at STP is

1. 22.4
2. 2.24L
3. 224 L
4. 44.8 L

Answer: 2. 2.24L.

Question 15. The kinetic theory of gases proves :

1. Only Boyle’s law
2. Only Charles’ law
3. Only Avogadro’s law
4. All of these

Answer: 4. all of these.

Question 16. Gas deviates from ideal gas nature because of molecules :

1. Are colourless
2. Attract each other
3. Contain covalent band
4. Show Brownian movement

Answer: 2. attract each other.

Question 17. One of the following is not the postulate of the kinetic theory of gases :

1. The actual volume of the molecules is negligible compared to the volume of the gas.
2. The molecules remain in ceaseless motion.
3. There are sufficient attractive forces between the molecules.
4. The average kinetic energy of the gas molecules is directly proportional to the absolute temperature.

Answer: 3. There are sufficient attractive forces between the molecules.

Class 10 Physical Science Solution WBBSE

Question 18. The critical temperature of a gas is the temperature :

1. Below which it cannot be liquefied
2. Which it solidifies
3. Above which it cannot be liquefied
4. Above which it can no longer remain in the gaseous state.

Answer: 4. Above which it cannot be liquefied.

Question 19. A pressure cooker reduces cooking time because :

1. The heat is more easily distributed
2. The higher pressure tenderizes the food
3. The boiling point of water inside is elevated
4. A large flame is used.

Answer: 3. The boiling point of water inside is elevated.

Question 20. Which of the following is valid at absolute zero?

1. The kinetic energy of the gas becomes zero, but the molecular motion does not become zero
2. The kinetic energy of the gas becomes zero and the molecular motion also becomes zero
3. The kinetic energy of the gas decreases but does not become zero
4. None of the above

Answer: 4. None of the above.

Question 21. The temperature at which a real gas obeys the ideal gas laws over an appreciable pressure range is called the :

1. Critical temperature
2. Inversion temperature
3. Boyle’s temperature
4. Transition temperature

Answer: 3. Boyle’s temperature.

Question 22. What will be the value of 127°C on the Kelvin scale?

1. 127 K
2. 400 K
3. 146 K
4. 200 K

Answer: 2. 400 K.

Question 23. The relation between 100°C and 373 K is

1. 100° C > 373 K
2. 100°C < 373 K
3. 100°C = 373 K
4. None of these

Answer: 3. 100°C = 373 K.

Class 10 Physical Science Solution WBBSE

Question 24. At NTP, if the volume of any gas is 10 lit then at 27°C and 750 mm pressure what will be its volume :

1. 11.1 lit
2. 15 lit
3. 8.1 lit
4. 8.2 lit

Answer: 1. 11.1 lit.

Question 25. At constant mass and constant volume, the relation between pressure and temperature is?

1. Boyle’s law
2. Charle’s law
3. Gay Lussac’s law
4. None of these

Answer: 3. Gay Lussac’s Law.

Question 26. At constant, mass and constant temperature the relation between volume and pressure is:

1. Chaple’s law
2. Boyle’s law
3. Gay Lussac’s law
4. None of these

Answer: 2. Boyle’s law.

Question 27. A gas having a temperature of 0°C is heated so that its pressure and volume are doubled. What will be the final temperature of the gas?

1. 1092 K
2. 1002 K
3. 999 K
4. 980 K

Answer: 1. 1092 K.

Class 10 Physical Science Solution WBBSE

Question 28. A gas will approach ideal behaviour at :

1. At low temperatures and low pressure
2. Low temperature and high pressure
3. High temperature and low pressure
4. High pressure and high temperature

Answer: 3. High temperature and low pressure.

Question 29. Attractive forces and size effects in a gas can be neglected at:

1. Low temperature
2. High pressure
3. Low pressures and high temperatures
4. Low temperatures and high pressures

Answer: 3. Low pressures and high temperatures.