Class 11 Physics: Kinetic Theory Mock Test

Unlocked

Progressive Test

Complete this chapter step by step in 8 rounds. If you pass a round, continue to the next fresh question set. If you do not pass, retry the same question set to improve your score.

Start Round 1

Locked

Mistake Review

This section collects your incorrect and unanswered Progressive Test questions. Attempt them again and correct them to reduce your pending mistakes.

Complete One Round to Unlock

Locked

Certificate Challenge

Clear your weak questions first, then prove your preparation and earn your chapter certificate.

Quiz: Kinetic Theory – Certificate Challenge
Total questions: 394
Questions to attempt: 100 random
Time allotted: 100 minutes
Certificate pass score: 70%
Random questions: Yes
Certificate: Yes
Retake: Until certificate earned
Note: Challenge locks after certificate is earned

Complete Required Practice to Unlock

Progressive Test — Guest First Round

Kinetic Theory – Progressive Test

Welcome to the Progressive Test.

Click Start Test to begin the loaded practice round.

Good luck!

1 / 50

1. An ideal gas is best described as a gas whose molecules have

a) point molecules with forces only in collisions

b) large volume and strong attraction at all separations

c) no mass and no kinetic energy

d) fixed positions inside the container

2 / 50

2. A gas is heated from to . For the same gas, the rms speed changes by a factor of

3 / 50

3. Use the table below for an ideal-gas mixture in the same container at the same temperature.

Component	Amount	Partial pressure
P
Q		?

The partial pressure of gas Q is

4 / 50

4. A monatomic ideal gas has . Its and are

a) ,

b) ,

c) ,

d) ,

5 / 50

5. A diatomic ideal gas at ordinary temperature is heated by at constant volume. Taking , the heat supplied is closest to

6 / 50

6. A gas spreads through the whole available space because its molecules

a) are fixed at one point until heated

b) attract only the upper wall

c) move continuously and randomly

d) have no mass inside a container

7 / 50

7. Use the graph description below.
A Maxwell speed-distribution graph is drawn for the same gas at two temperatures and . Curve II has a lower peak, is broader, and its maximum is shifted to a higher speed compared with Curve I. The area under each curve is the same.
The best conclusion is

a) , and Curve II has a larger molar mass

b) , and the number of molecules represented by both curves is the same

c) , and Curve II represents fewer molecules

d) , and every molecule in Curve II moves faster than every molecule in Curve I

8 / 50

8. In the expression , the symbol represents

a) pressure force on one wall

b) number of moles only

c) active degrees of freedom

d) frequency of wall collision only

9 / 50

9. Consider the following statements about , , , , and .
I. .
II. .
III. .

a) II and III only

b) I, II, and III

c) I and II only

d) I and III only

10 / 50

10. In a cubical container of side , a molecule with -component travels between the two opposite walls perpendicular to the -axis. The time between two successive collisions with the same wall is

11 / 50

11. In the ideal-gas kinetic model, molecules are treated as point particles because their own volume is assumed to be

a) responsible for all intermolecular attraction

b) equal to the volume of the container

c) larger than the container volume

d) negligible compared with the gas volume

12 / 50

12. Mean free path of a gas molecule means the

a) average distance between successive collisions

b) diameter of the gas molecule itself

c) distance from Earth to the gas container

d) total distance travelled in one second by every molecule

13 / 50

13. A sealed box contains gas in equilibrium. Pressure on the side wall is not explained mainly by the weight of gas above it because

a) only the bottom wall can receive molecular impacts

b) pressure exists only when molecules are motionless

c) pressure comes from momentum transfer to every wall

d) gas molecules do not collide with side walls

14 / 50

14. A monatomic ideal gas undergoes an isothermal expansion. Its internal energy change is

a) zero; temperature is constant

b) negative because pressure decreases

c) positive because volume increases

d) equal to because the gas expands

15 / 50

15. For an ideal gas, . If the density is unchanged and is doubled, the pressure becomes

a) twice the initial pressure

b) half the initial pressure

c) unchanged

d) fourfold pressure

16 / 50

16. The kinetic-theory pressure relation obtained after summing molecular impacts and using isotropy is

17 / 50

17. A statement says, “In an ideal gas, there are no collisions because intermolecular forces are neglected.” The best correction is that

a) the statement is fully valid for all gases

b) collisions are included; forces are neglected between collisions

c) wall collisions are forbidden, but molecule-molecule collisions are allowed

d) collisions occur only if molecules have no speed

18 / 50

18. A sample contains of oxygen gas with molar mass . Its total mass is

19 / 50

19. A gas sample has the same volume, temperature, and pressure as another gas sample. Avogadro's hypothesis allows us to conclude that the two samples have the same

a) total mass

b) density

c) molecular mass

d) molecule count

20 / 50

20. Consider the following statements about molecular size and number density.
I. A typical molecular diameter is of the order .
II. Number density tells the number of molecules per unit volume.
III. If is fixed and increases, number density increases.

a) II and III only

b) I, II, and III

c) I and III only

d) I and II only

21 / 50

21. A gas has a longer mean free path under one set of conditions than under another. For transport phenomena, this usually means molecules can

a) carry momentum or energy farther before collision

b) remain permanently attached to the container wall

c) lose all kinetic energy after the first collision

d) stop contributing to pressure

22 / 50

22. A row in a notebook says, “Molecular mass and mass of one molecule are the same quantity.” The most useful correction is that

a) both quantities are always measured in

b) molar mass is mole-scale; one-molecule mass is particle-scale

c) the two quantities differ only for liquids and never for gases

d) mass of one molecule is measured in , while molar mass is a pure number

23 / 50

23. A gas molecule has instantaneous velocity components , , and . For the gas as a whole, kinetic theory uses only when

a) the gas has only one molecule

b) and are always zero

c) every molecule moves parallel to the -axis

d) molecular motion is random and isotropic

24 / 50

24. Select the rows whose judgements are correct.

Decision	Judgement
P. Use for a dilute gas far from liquefaction	Suitable
Q. Use simple equipartition with only active degrees of freedom	Suitable
R. Use mean-free-path formula without caution in a very dense gas	Not suitable
S. Use Celsius directly in	Suitable

a) Rows P, R, and S

b) Rows P, Q, and S

c) Rows Q, R, and S

d) Rows P, Q, and R

25 / 50

25. Match the following kinetic-theory relations with the condition or meaning they most directly represent.

Column I	Column II
P.	1. Pressure from density and molecular speed
Q.	2. Collision spacing using number density
R.	3. Ideal-gas molar heat-capacity difference
S.	4. Average translational kinetic energy per molecule

a) P-1, Q-2, R-3, S-4

b) P-1, Q-3, R-2, S-4

c) P-2, Q-1, R-4, S-3

d) P-4, Q-2, R-3, S-1

26 / 50

26. A ideal gas has and . It is heated through at constant volume. The heat supplied is closest to

27 / 50

27. Use the arrangement described below.

Two closed vessels of equal volume contain different gases at ordinary conditions. Vessel P contains helium and vessel Q contains oxygen. In both vessels, the gases fill the entire container.

The fact that both gases fill their vessels is mainly due to

a) equal molecular masses of helium and oxygen

b) absence of pressure in both vessels

c) molecules being fixed to the container walls

d) random molecular motion in gases

28 / 50

28. A gas and a solid are compared at the molecular level. In the gas, a typical molecule travels a relatively long distance before its direction is changed by collision, while in the solid, particles mainly vibrate about fixed positions. This comparison mainly explains why

a) solids have no microscopic motion

b) gases have no molecules

c) gases flow and fill containers

d) gases always have zero density

29 / 50

29. A non-linear polyatomic molecule is treated as having translational and rotational active degrees of freedom when vibrations are neglected. Its value of is

30 / 50

30. A gas in a container is heated while its volume and number of molecules remain fixed. The kinetic explanation for the pressure increase is that heating increases

a) average molecular kinetic energy and wall momentum transfer

b) the mass of each molecule in proportion to pressure

c) the number of molecules by Avogadro's constant in every second

d) the container volume to infinity

31 / 50

31. A monatomic ideal gas has active degrees of freedom. The average energy per molecule is therefore

32 / 50

32. Select the rows whose judgements are correct.

Row	Claim	Judgement
P	At the same , different ideal gases have the same average translational kinetic energy per molecule	Suitable
Q	At the same , all molecules must have exactly the same speed	Not suitable
R	Average translational kinetic energy per molecule is proportional to in	Suitable
S	Temperature is directly proportional to molecular mass at fixed energy	Suitable

a) P, Q, and R only

b) Q, R, and S only

c) P and S only

d) P, Q, R, and S

33 / 50

33. Use the arrangement described below.

A gas molecule travels inside a cubical container. Between two collisions, no force acts on it in the ideal-gas model. At the wall, it rebounds elastically.

During the free part of its motion between collisions, the molecule is assumed to move

a) with uniform velocity in a straight line

b) along a spiral path due to attraction by all walls

c) with zero speed at every point

d) only in the vertical direction

34 / 50

34. A gas sample is at with rms speed . It is heated to . The new rms speed is

35 / 50

35. At constant pressure, the temperature of an ideal gas is increased while molecular diameter remains unchanged. The mean free path generally

a) decreases because molecular diameter increases

b) increases because number density decreases

c) remains unchanged because pressure is constant

d) becomes zero because temperature is higher

36 / 50

36. One mole of any substance contains approximately

a) particles

b) particles

c) particles

d) particles

37 / 50

37. A gas is described by the relation . If its pressure is kept constant while its density becomes one-fourth of the original value, the new rms speed becomes

a) times the original value

b) of the original value

c) times the original value

d) of the original value

38 / 50

38. A gas at constant pressure is heated from to . Molecular diameter is unchanged. If its initial mean free path is and initial collision frequency is , the final mean free path and collision frequency are

a) and

b) and

c) and

d) and

39 / 50

39. Two flasks of equal volume are kept at the same temperature and pressure. One contains nitrogen and the other contains carbon dioxide. According to Avogadro's hypothesis, the two flasks contain the same

a) mass of gas

b) molecule count

c) molecular mass

d) density

40 / 50

40. Assertion: At ordinary temperature, a diatomic gas is often assigned active degrees of freedom.
Reason: Its translational and rotational modes are counted, while vibrational modes are usually neglected in the simple treatment.

a) Assertion is true, but Reason is false

b) Assertion is false, but Reason is true

c) Both Assertion and Reason are true, and Reason explains Assertion

d) Both Assertion and Reason are true, but Reason does not explain Assertion

41 / 50

41. A statement about gases says, “The molecules in a gas are far apart, so there is no interaction of any kind.” The most accurate correction is that

a) far-apart molecules cannot have mass

b) gas molecules are actually fixed at regular points

c) gas molecules must all move with the same speed

d) far apart on average, yet collisions still occur

42 / 50

42. A monatomic ideal gas is heated from to . At the same time, its volume doubles. The change in internal energy is, using ,

43 / 50

43. A gas is compressed isothermally from volume to , with the number of molecules and molecular diameter unchanged. The mean free path becomes

a) multiplied by 1

b) multiplied by 9

c) multiplied by 3

d) divided by 3

44 / 50

44. A gas has molecules, each of mass , in volume . If the pressure is , its rms speed is closest to

45 / 50

45. Helium and oxygen are kept at the same pressure and temperature. Taking their molar masses as and , respectively, the correct comparison is

a) and

b) and

c) and

d) and

46 / 50

46. A gas sample has density , pressure , and molar mass . Using , its temperature is closest to

47 / 50

47. A statement says, “Because a molecule has diameter about , a gas molecule has no size at all.” The statement is best judged as

a) accurate, because molecules are larger than the container

b) inaccurate, because all molecules must have diameter

c) accurate, because is exactly zero

d) inaccurate, because molecular size is small but not zero

48 / 50

48. In gas equations, the symbol is best interpreted as

a) number of molecules in the gas sample

b) mass of one molecule in

c) molecular speed in

d) amount of gas measured in

49 / 50

49. A gas molecule of mass is in a gas whose pressure is and number density is . Its rms speed is closest to

50 / 50

50. Mayer's relation for an ideal gas connects the molar heat capacities as

Your score is

Complete at least one Progressive Test round with incorrect or unanswered questions to unlock Mistake Review.

Complete at least 25% of the Progressive Test to unlock the Certificate Challenge Section.

Kinetic Theory Mock Test – Class 11 Physics

Progressive Test

Mistake Review

Certificate Challenge

Progressive Test — Guest First Round

Kinetic Theory – Progressive Test

Share your achievement!

Related MCQs