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Edited By Safeer PP | Updated on Aug 09, 2022 12:21 PM IST

In chapter 13, the Kinetic Theory of Gases is dealt with. In this chapter, the learners will come to know about the gases, their molecular movement, and how these phenomenons can be understood at both macroscopic and microscopic levels. This chapter can seem to be a bit complicated for the students in the beginning. But if one focuses on the terminology, the processes, and their applications step by step alongside NCERT exemplar Class 11 Physics solutions chapter 13 it will become easier to retain. In this chapter, the students are taught about the kinetic theory gases, gas laws of ideal gases, postulates, assumptions, and the non-ideal gas behavior. This chapter and NCERT exemplar Class 11 Physics chapter 13 solutions encapsulate all the topics related to gas molecule movement in a container along with the factors of temperature, pressure, and energy.

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This Story also Contains

- NCERT Exemplar Class 11 Physics Solutions Chapter 13-MCQI
- NCERT Exemplar Class 11 Physics Solutions Chapter 13-MCQII
- NCERT Exemplar Class 11 Physics Solutions Chapter 13-Very Short Answer
- NCERT Exemplar Class 11 Physics Solutions Chapter 13-Short Answer
- NCERT Exemplar Class 11 Physics Solutions Chapter 13-Long Answer
- Topics in NCERT Exemplar Class 11 Physics Solutions Chapter 13
- What will The Student Learn from NCERT Exemplar Class 11 Physics Solutions Chapter 13 Kinetic Theory Of Gases?
- NCERT Exemplar Class 11 Physics Solutions Chapter-Wise
- Important Topics To Cover From NCERT Exemplar Class 11 Physics Solutions Chapter 13 Kinetic Theory Of Gases
- NCERT Exemplar Class 11 Solutions

Question:13.1

A cubic vessel (with face horizontal + vertical) contains an ideal gas at NTP. The vessel is being carried by a rocket which is moving at a speed of in the vertical direction. The pressure of the gas inside the vessel as observed by us on the ground

(a) remains the same because is very much smaller than v_{rms} of the gas.

(b) remains the same because the motion of the vessel as a whole does not affect the relative motion of the gas molecules and the walls.

(c) will increase by a factor equal to where vrms was the original mean square velocity of the gas.

(d) will be different on the top wall and bottom wall of the vessel.

Answer:

The answer is the option (b)In the rocket, the relative velocity of molecules does not change with respect to walls of a container as the mass of a molecule when compared to that of the whole system is negligible. So, the whole gas system moves as a single unit. The rocket moves at a constant speed which makes the acceleration zero, and hence the pressure remains the same as observed by us inside the gas vessel.

Question:13.2

1 mole of an ideal gas is contained in a cubical volume V, ABCDEFGH at 300 K (figure). One face of the cube (EFGH) is made up of a material which totally absorbs any gas molecule incident on it. At any given time,

(a) the pressure on EFGH would be zero

(b) the pressure on all the faces will be equal

(c) the pressure of EFGH would be double the pressure on ABCD

(d) the pressure on EFGH would be half that on ABCD

Answer:

The answer is the option (d)The rate of transfer of momentum on the wall exerts pressure on the wall due to the force exerted by the molecules. Elastic collision takes place, and hence the molecules bounce back. The walls absorb the magnitude of momentum transferred to it by each molecule which is equal to 2mv. So, the net rate of change of momentum is mv, and the pressure of EFGH is halved as compared to ABCD.

Question:13.3

Boyle’s law is applicable for an

(a) adiabatic process

(b) isothermal process

(c) isobaric process

(d) isochoric process

Answer:

The answer is the option (b)At constant temperature, Boyle’s law is applicable

(n, R, T are constant in this case)

So, PV = constant and

Question:13.4

A cylinder containing an ideal gas is in a vertical position and has a piston of mass M that is able to move up or down without friction ( figure). If the temperature is increased

(a) both P and V of the gas will change

(b) the only P will increase according to Charles’ law

(c) V will change but not P

(d) P will change but not V

Answer:

The answer is the option (c)In case of an ideal gas, the pressure remains the same throughout irrespective of the initial or final position. Here, and no friction acts on piston and the cylinder

We have,

Since, P, n and R, are constant here, . So, the temperature increases as volume increases and vice-versa at the same time, when pressure remains constant.

Question:13.5

Volume versus temperature graphs for a given mass of an ideal gas is shown in the figure. At two different values of constant pressure. What can be inferred about the relation between and ?

(a)

(b)

(c)

(d) Data is insufficient

Answer:

The answer is the option (a)Pressure and quantity of gas are constant here.

From , we can say that,

So, = constant (slope = constant)

hence its value decreases with pressure, so,

so, slope of is smaller than and hence a is the right option.

Question:13.6

1 mole of gas is contained in a box of volume at T = 300 K. The gas is heated to a temperature of T= 3000 K and the gas gets converted to a gas of hydrogen atoms. The final pressure would be (considering all gases to be ideal)

(a) same as the pressure initially

(b) 2 times the pressure initially

(c) 10 times the pressure initially

(d) 20 times the pressure initially

Answer:

The answer is the option (d)The transfer of the rate of change of momentum by the particles to the walls is what causes exertion of pressure by the gas. As temperature rises and hydrogen molecules break into atoms, the mass of the particle becomes halved, and the number of particles becomes double. Since the velocity is strictly dependent on the temperature, at the same temperature, i.e. at 300K, the velocity of particles of as well as H remains the same. Also, the pressure does not change as the atomic form changes since the rate of transfer of momentum is also same in the case of as well as H.

Question:13.7

A vessel of volume V contains a mixture of 1 mole of hydrogen and 1 mole of oxygen (both considered as ideal). Let denotes the fraction of molecules with speed between v and (v + dv) with , similarly for oxygen. Then,

(a) obeys the Maxwell’s distribution law

(b) will obey the Maxwell’s distribution law separately

(c) neither will obey Maxwell’s distribution law

(d) will be the same

Answer:

The correct answer is the option (b)F1(v): speed of n molecules = (v+dv)

The number of molecules remains the same, which is one mole for . since the molecules differ in mass, they will also differ in speed, and hence both gases will separately obey Maxwell’s distribution.

Question:13.8

An inflated rubber balloon contains one mole of an ideal gas, has a pressure P. volume V and temperature T. If the temperature rises to 1.1 T, and the volume is increased to 1.05 V, the final pressure will be

(a) 1.1 P

(b) P

(c) less than P

(d) between P and 1.1

Answer:

The correct answer is the option (d)According to ideal gas equation, PV = nRT

Here, = constant.

So,

So, the value of is between p and 1.1 p and hence, option d is correct.

Question:13.9

ABCDEFGH is a hollow cube made of an insulator (figure) face ABCD has a positive charge on it. Inside the cube, we have ionised hydrogen.

The usual kinetic theory expression for pressure

(a) will be valid

(b) will not be valid, since the ions would experience forces other than due to collisions with the walls

(c) will not be valid, since collisions with walls would not be elastic

(d) will not be valid because isotropy is lost

Answer:

The correct answer is the option (b) and (d)The wall of ABCD is positively charged. The presence of hydrogen ions and the charge on the walls lead to an electrostatic force which acts in contrast to the collision and make the kinetic theory of gases invalid in this case. The isotropy also gets lost given the presence of hydrogen ions instead of hydrogen molecules. Hence options b and d are correct.

Question:13.10

Diatomic molecules like hydrogen have energies due to both translational as well as rotational motion. From the equation in kinetic theory , E is

(a) the total energy per unit volume

(b) only the translational part of energy because rotational energy is very small compared to the translational energy

(c) only the translational part of the energy because during collisions with the wall pressure relates to change in linear momentum

(d) the translational part of the energy because rotational energies of molecules can be of either sign and its average over all the molecules is zero

Answer:

The correct answer is the option (c)As per the kinetic theory of gases, the perpendicular forces exerted by the molecules on the walls while in motion are only responsible for the pressure exerted due to the gas molecules. So, for molecules striking at angles other than 90 degrees, no pressure will be exerted. Hence, in this case, only translational motion change leads to pressure on the wall. So, , which represents the translational motion part and hence c is the correct option.

Question:13.11

In a diatomic molecule, the rotational energy at a given temperature

(a) obeys Maxwell’s distribution

(b) have the same value for all molecules

(c) equals the translational kinetic energy for each molecule

(d) is the translational kinetic energy for each molecule

Answer:

The correct answer is the option (a) and (d)If we assume a diatomic molecule along the z-axis, its energy along that axis will be zero. The total energy of a diatomic molecule can be expressed as:

The number of independent terms in the expression =5. The above expression obeys Maxwell’s distribution as their velocities can be predicted with Maxwell’s findings. In this case, for each molecule 3 translational and 2 rotational energies are associated. So, at any temperature, rotational energy = translational KE

Question:13.12

Which of the following diagrams (figure) depicts ideal gas behaviour?

Answer:

The correct answer is the option (a) and (c)a)

where R and T are constant.

Since P is constant, as given in the graph of option a.

Hence, option is correct.

c) In case where, V = constant

, which is a straight line. Hence option c is correct.

Question:10.13

When an ideal gas is compressed adiabatically, its temperature rises the molecules on the average have more kinetic energy than before. The kinetic energy increases,

(a) because of collisions with moving parts of the wall only

(b) because of collisions with the entire wall

(c) because the molecules get accelerated in their motion inside the volume

(d) because of the redistribution of energy amongst the molecules

Answer:

The correct answer is the option (a)The number of collisions per second between the molecules and walls increases and the mean free path becomes smaller as an ideal gas compressed. This, in turn, increases the temperature of the gas, which increased the overall kinetic energy of the gas molecules as KE depends on the temperature.

Question:13.14

Calculate the number of atoms in 39.4 g gold. The molar mass of gold is 197 g mole^{-1}.

Answer:

Number of atoms on 197 g gold =Number of atoms in 1g of gold, n

Hence, number of atoms in 34g of gold =

atoms

Question:13.15

The volume of a given mass of a gas at , 1 atm is 100 cc. What will be its volume at ?

Answer:

Let, = 1 atm, = 1 atm, , = ? ,From the ideal gas equation, we have

Hence,

Question:13.18

Answer:

Degree of freedom is necessary to be known if we need to find the total energy of a particular molecule.An oxygen molecule has 2 atoms, so the degree of freedom = 2 rotational + 3 translational = 5

Total internal energy for 2 moles of oxygen =

Neon gas has a degree of freedom equal to 3, since it is a monoatomic gas-only translational degree of freedom is present. So, the total internal energy per mole.

For 4 moles of neon gas, total internal energy =

Hence total internal energy of 2 moles oxygen + 4 moles Neon = 5 + 6 = 11 RT

Question:13.20

Answer:

According to the ideal gas situation, we have PV = nRTFor chamber 1 and chamber 2,

and

When we remove the partition, and

According to kinetic theory, Translational gas kinetic energy. E per mole

So, the translational KE for both cases will be,

and

Adding,

hence by combining the results we get,

Question:13.22

Answer:

The volume of a sphere = the volume of one moleculeHere

So, volume =

For 0.5 g of hydrogen gas, no of moles =

Hence the volume of hydrogen molecules =

For a constant temperature, ideal gas à Pi Vi = Pf Vf

Hence,

The gas here will not obey the ideal gas behaviour as the kinetic energy of the molecules will not interact with each other due to compression.

Question:13.23

Answer:

The volume of a gas is inversely proportional to the pressure of the gas at a constant temperature as stated by Boyle’s law. When air is continuously pumped inside the tyre, the number of moles of gas (i.e. the mass of the gas) increases. Since Boyle’s law is only applicable for a constant mass of gas, it will not hold true in this case.Question:13.24

A balloon has 5.0 mole of helium at . Calculate

(a) the number of atoms of helium in the balloon.

(b) the total internal energy of the system.

Answer:

Helium gas, n = 5 moles and T = 280 Ka) number of atoms of He = atoms of He

b) the degree of freedom for a helium atom is 3 since it is monoatomic

so, average T per molecule

average

hence total energy =

Question:13.25

Calculate the number of degrees of freedom of molecules of hydrogen in 1 cc of hydrogen gas at NTP.

Answer:

Degree of freedom of HNumber of molecules in 1cc of hydrogen gas at NTP à 22.4 L = 22400 cc H

So, 1cc of H

Hence the total degree of freedom =

Question:13.26

Answer:

Since the gas is monoatomic, only translational degree of freedom will be applicable. KE per molecule = . when the container which is insulated has suddenly stopped, a transfer of kinetic energy takes place to the gas molecules. Let be the slight increase in temperature and n be the number of moles of gas.The resultant increase in translational KE can be presented as,

Increased KE due to velocity,

Hence,

So,

Question:13.27

Explain why

(a) there is no atmosphere on the moon.

(b) there is a fall in temperature with altitude.

Answer:

a) The acceleration on the moon due to gravity is one-sixth that of Earthescape velocity on the moon can be written as:

mass of hydrogen, m = 1.67 x 10-24 kg

v(RMS) is larger than the escape velocity as the gravitational force is small. The sun-moon distance is fairly equal to that of the earth. The energy of the sun reaches in a larger intensity to the moon due to its lower density of the atmosphere. So, the molecules of sunlight have a larger RMS speed and hence can escape out fairly easily. Hence, the moon has lost its atmosphere over time.

b) The kinetic energy of the air molecule gives the characteristic temperature to the atmosphere. At greater heights, atmospheric pressure is low, which makes air molecules rise higher, which in turn leads to an increase in their potential energy and decrease in their kinetic energy. Since the overall kinetic energy decreases, the temperature also decreases. Also, the lower atmospheric pressure causes expansion of the gas, which also provide a cooling effect.

Question:13.28

Consider an ideal gas with the following distribution of speeds.

Speed | % of molecules |

200 | 10 |

400 | 20 |

600 | 40 |

800 | 20 |

1000 | 10 |

(i) Calculate V rms and hence T. ()

(ii) If all the molecules with speed 1000 m/s escape from the system, calculate new Vrms and hence T.

Answer:

(i)(ii)

Molecules escape at rate of 1000m/s, we can calculate the v

Question:13.3

Answer:

Let v1 = volume of box = 1 mLet p1 be the initial pressure = 1.5 atm

Let p2’ be the final pressure =1.5 - 0.1 = 1.4 atm

t1 = initial temperature = 300K, t2 = final temperature = 300 K

let a be the area of hole =

The pressure difference initially between the tyre and atmosphere, ΔP = (1.5 -1) = 0.5 atm

Mass of N2 molecule

Now since

Hence,

For a gas molecule, Kinetic energy =

Now,

(A)

The N2 molecules striking the wall in time outwards

(A) outwards.

The temperature of the air and inside the box is equal to T.

The N2 molecules striking the wall in time inwards = (A) inwards.

Here, Pn2 = density of air molecules

So, we can calculate the net number of molecules going outward as:

We know that,

Pn1 = total number of molecules in the box/ volume of the box

per unit volume.

After a time, T, the pressure reduces to (1.5-0.1) = 1.4 atm = P’2

The new density of the Na molecules per unit volume.

The number of molecules going out from volume

= where P’2 = final pressure of the box

The total number of molecules which exit the hole in time t’ is:

The net number of molecules exiting in time t' is

Now we can write from the above results,

seconds.

Question:13.31

Answer:

We assume ‘p’ to be the number of molecules per unit volume. Hence ‘p’ is the per unit volume molecular density. Let v be the velocity of gas molecules.The molecules of the gas strike the front face and the back face of the box when it moves. The back face relative velocity =

Change in momentum on the front face of the box = and the change in momentum on the back face of the box =

Nf =Total number of molecules striking the box’s front face =

Nb = Total number of molecules striking the box’s back face

Nb

Total change in momentum at the front face can be calculated s below:

in the backward direction.

Force on front end = Ff = Pf = in the backward direction

In the same way, the force on the back face, Fb =

So, the net force can be calculated as:

It can be expanded and simplified as,

The magnitude of dragging force=

Kinetic energy for a molecule of gas can be calculated as:

Hence,

So, we can write the drag force as

NCERT questions are one of the most crucial ones if one wants to score high in their exams and also want to learn better for entrance exams. We have solved all the questions given in the main exercise as per the CBSE pattern and marking scheme. This will help the student learn better keeping in mind how to answer for better scoring. Our NCERT exemplar Class 11 Physics solutions chapter 13 pdf download are also downloadable so that one can access them offline in the PDF format. Simply, click on the given link and it is done.

**Also, Read NCERT Solution subject wise -**

- NCERT Solutions for Class 11 Maths
- NCERT Solutions for Class 11 Physics
- NCERT Solutions for Class 11 Chemistry
- NCERT Solutions for Class 11 Biology

**Also, check NCERT Notes subject wise -**

- NCERT Notes for Class 11 Maths
- NCERT Notes for Class 11 Physics
- NCERT Notes for Class 11 Chemistry
- NCERT Notes for Class 11 Biology

- 1. Introduction
- 2. Molecular nature of matter
- 3. Behaviour of gases
- 4. Kinetic theory of ideal gases
- 5. Law of equipartition of energy
- 6. Specific heat capacity
- 7. Mean free path

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Download EBookKinetic theory of gases is the chapter that derives all its topics from the idea that in the gas, the molecules are smaller than the distance between the gas molecules. They move around the container and collide with each other on the walls. Now, this movement of the molecules with the effect of temperature, pressure, and other factors will help in describing the physical properties of the gas. The learner will learn about kinetic theory, its assumptions, and postulates. There are around 9 assumptions like the gas is made of particles, particles have zero volume, there is no interaction between particles, etc.

Students will also learn about the ideal gas’s gas laws like Avogadro’s law, Amonton’s law, Boyles’ law, Charles law, and Graham's law of diffusion. At the end of the chapter and NCERT exemplar Class 11 Physics chapter 13 solutions the learner will come across the Maxwell and Boltzmann energy and velocity distribution law, which has a lot of significance from an exam point of view.

· For a better understanding of the kinetic theory of gases, the first thing that one should pay attention to is the gas laws. 5 gas laws explain how an ideal gas behaves when one factor is kept constant. The formulas of these laws will help in solving numerical based questions in the exam.

· Secondly, a student should pay attention to non-ideal gas behaviour. In this topic, the real gases are discussed who do not follow the ideal gas behaviour under low pressure and high-temperature conditions as per NCERT exemplar Class 11 Physics solutions chapter 13.

· Lastly, learners should pay attention to the Maxwell and Boltzmann law of velocity and energy distribution. In this, the root means square and average velocity is discussed, of the gaseous particles which act under proportional kinetic energy and temperature.

Chapter 1 | Physical world |

Chapter 2 | Units and Measurement |

Chapter 3 | Motion in a straight line |

Chapter 4 | Motion in a Plane |

Chapter 5 | Laws of Motion |

Chapter 6 | Work, Energy and Power |

Chapter 7 | System of Particles and Rotational motion |

Chapter 8 | Gravitation |

Chapter 9 | Mechanical Properties of Solids |

Chapter 10 | Mechanical Properties of Fluids |

Chapter 11 | Thermal Properties of Matter |

Chapter 12 | Thermodynamics |

Chapter 13 | Kinetic Theory |

Chapter 14 | Oscillations |

Chapter 15 | Waves |

1. What are the benefits of these solutions?

Our solutions are detailed and created most exhaustively, and this will help in understanding the topic, solving questions, and is also learning how to answer questions in the exam.

2. Who can take advantage of these solutions?

A student who is preparing for exams, for entrance exams like NEET or JEE or any other engineering and medical exam can make the most from these solutions.

3. Are these solutions as per the CBSE pattern?

Yes, these NCERT exemplar class 11 physics solutions chapter 13 are as per the CBSE pattern, as they are solved step by step and according to the marking scheme.

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