Class 11 Physics: Kinetic Theory Mock Test

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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
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Kinetic Theory – Progressive Test

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1 / 50

1. Study the table and identify the row that correctly uses .

Row	Change	Effect on
P	doubled, unchanged	doubles
Q	unchanged, doubled	quadruples
R	halved, doubled	doubles
S	doubled, halved	doubles

a) Rows P, R, and S

b) Rows P, Q, and S

c) Rows Q, R, and S

d) Rows P, Q, and R

2 / 50

2. A gas has , , molecular diameter , and molar mass . Using , , and , the collision frequency is closest to

3 / 50

3. A small amount of steam escapes from a pressure cooker. Its ability to push against the surroundings is best connected with

a) the colour of water vapour

b) collisions and momentum transfer

c) the absence of molecules in steam

d) the steam having no kinetic energy

4 / 50

4. An ideal gas has at . Taking , its molar mass is closest to

5 / 50

5. The root mean square speed of gas molecules is defined as

6 / 50

6. A vessel contains gas molecules in a volume of . What is the number density of the gas?

7 / 50

7. Nitrogen gas has molar mass . Taking , the mass of one nitrogen molecule is closest to

8 / 50

8. A rigid vessel contains helium and nitrogen at in volume . Taking , the partial pressure of helium and total pressure are closest to

a) and

b) and

c) and

d) and

9 / 50

9. 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) the mass of each molecule in proportion to pressure

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

c) average molecular kinetic energy and wall momentum transfer

d) the container volume to infinity

10 / 50

10. A - graph for a fixed amount of gas at constant pressure is drawn using in . The graph is a straight line because

a) is independent of

11 / 50

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

a) I, II, and III

b) I and III only

c) I and II only

d) II and III only

12 / 50

12. Consider the following statements about molecular speed distribution.
I. At a fixed temperature, all molecules of a gas have exactly the same speed.
II. Raising temperature shifts the distribution toward higher speeds.
III. For a fixed number of molecules, the area under the speed-distribution curve remains fixed.

a) II and III only

b) I and III only

c) I, II, and III

d) I and II only

13 / 50

13. A table gives two ways of writing the ideal-gas equation. Select the fully consistent row.

Row	Counting scale	Equation	Constant used
P	Moles
Q	Molecules
R	Moles
S	Molecules

a) P and Q only

b) Q and R only

c) P, Q, R, and S

d) R and S only

14 / 50

14. Match the quantities with their meanings.

Quantity	Meaning
P.	1. Number of molecules in the sample
Q.	2. Amount of gas in moles
R.	3. Molar mass of the gas
S.	4. Mass of one molecule

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

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

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

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

15 / 50

15. 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 is exactly zero

b) inaccurate, because all molecules must have diameter

c) accurate, because molecules are larger than the container

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

16 / 50

16. In the expression , the symbol represents

a) frequency of wall collision only

b) number of moles only

c) active degrees of freedom

d) pressure force on one wall

17 / 50

17. A fixed mass of gas at constant pressure occupies at . Its volume at is

18 / 50

18. A monatomic ideal gas and a diatomic ideal gas at ordinary temperature have the same and the same temperature rise . The ratio of their constant-volume heat requirements is

19 / 50

19. A gas of molar mass is at . Another gas of molar mass has the same . Its temperature is

20 / 50

20. Study the table for a fixed amount of monatomic ideal gas. Select the row that gives the correct sign of .

Row	Temperature change	Sign of
P		Positive
Q		Zero
R		Negative
S		Always negative

a) Rows Q, R, and S

b) Rows P, R, and S

c) Rows P, Q, and S

d) Rows P, Q, and R

21 / 50

21. A molecule has mass , and its gas has molar mass . The correct relation between , , and is

22 / 50

22. Brownian motion supports the molecular theory of matter because it shows that

a) gases alone contain molecules, while liquids do not

b) all particles in a liquid are arranged in a perfect crystal

c) suspended particles are hit by invisible moving molecules

d) molecules in a fluid are always at rest

23 / 50

23. A gas is heated through the same temperature rise once at constant volume and once at constant pressure. For the same amount of ideal gas, the heat required at constant pressure is larger because

a) some heat is used for expansion work

b) is always smaller than

c) the gas has no molecular motion at constant pressure

d) temperature cannot change at constant pressure

24 / 50

24. A container has molecules of gas P and molecules of gas Q at the same temperature and volume . For an ideal mixture, the total pressure is

d) always

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. 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) remains unchanged because pressure is constant

c) becomes zero because temperature is higher

d) increases because number density decreases

27 / 50

27. A fixed amount of ideal gas is heated so that its absolute temperature becomes times the initial value. If its volume simultaneously becomes times the initial value, the final pressure is

28 / 50

28. A gas at and has mean free path . If the same gas is taken to and , with molecular diameter unchanged, the new mean free path is

29 / 50

29. A molecule-molecule collision in the kinetic theory of an ideal gas is taken to be perfectly elastic. This means

a) molecules stick together after every collision

b) total kinetic energy and momentum are conserved

c) the molecules stop moving after collision

d) kinetic energy is completely lost as heat in each collision

30 / 50

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

31 / 50

31. A sealed container filled with air is kept on a table. The pressure exerted by the air on the side walls is mainly due to

a) attraction between the walls and the table

b) the downward weight of air molecules only

c) molecules becoming motionless near the wall

d) momentum transfer in wall collisions

32 / 50

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

a) half the initial pressure

b) fourfold pressure

c) twice the initial pressure

d) unchanged

33 / 50

33. A molecule of mass has -component of velocity in a cubical vessel of side . Its average force contribution on one wall perpendicular to the -axis is

34 / 50

34. A fixed amount of gas has pressure when its volume is . At the same temperature, its volume becomes . The new pressure is

35 / 50

35. Study the table and select the row that correctly connects an observation with its molecular explanation.

Row	Observation	Molecular explanation
P	Brownian motion of smoke particles	Random impacts by air molecules
Q	Gas pressure on a wall	Momentum transfer during molecular collisions
R	Gas filling a vessel	Random molecular motion through available space
S	Brownian motion increases with temperature	Molecules become less agitated at higher

a) P, Q, R, and S

b) P, Q, and R only

c) Q, R, and S only

d) P and S only

36 / 50

36. A diatomic ideal gas at ordinary temperature has at . If , its internal energy and are closest to

a) and

b) and

c) and

d) and

37 / 50

37. Use the arrangement described below.

A molecule of effective diameter moves through a gas. During its motion, it can collide with other molecules whose centres come within an effective collision width related to .

If is made larger while number density is unchanged, the mean free path generally

a) becomes equal to

b) decreases as the collision cross-section increases

c) becomes independent of molecular size

d) increases because larger molecules avoid collisions

38 / 50

38. 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) remain permanently attached to the container wall

b) stop contributing to pressure

c) carry momentum or energy farther before collision

d) lose all kinetic energy after the first collision

39 / 50

39. A monatomic ideal gas has . Its and are

a) ,

b) ,

c) ,

d) ,

40 / 50

40. A molecule has the same speed in two cases but different directions. In Case 1, it moves almost parallel to a chosen wall; in Case 2, it moves nearly perpendicular to that wall. The pressure contribution on that wall is larger in

a) Case 1, because parallel motion gives maximum normal momentum change

b) neither case, because wall pressure does not depend on collisions

c) Case 2, because the normal velocity component is larger

d) both cases equally, because only total speed matters for one wall

41 / 50

41. 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) absence of pressure in both vessels

b) molecules being fixed to the container walls

c) equal molecular masses of helium and oxygen

d) random molecular motion in gases

42 / 50

42. In a gas at fixed temperature, pressure is reduced to one-fourth of its original value. Assuming ideal-gas behaviour and unchanged molecular diameter, the mean free path becomes

43 / 50

43. A vessel contains of an ideal gas at . The gas is heated at constant pressure until its volume becomes times the original volume. If the gas is monatomic and , the increase in internal energy is closest to

44 / 50

44. A gas pushes normally on a wall with a total force of over an area of . What pressure does the wall experience?

45 / 50

45. Two ideal gases at the same pressure and temperature have molar masses and . Their densities are in the ratio

46 / 50

46. A sealed transparent box contains a gas. Imagine marking one molecule and observing only its motion for a very short time. Its path would most likely appear irregular because

a) collisions repeatedly change its direction

b) gravity forces it to move in a perfect circle

c) it must travel only parallel to one wall

d) it has no velocity between two collisions

47 / 50

47. A gas has molar mass and amount . Its total mass is

48 / 50

48. A collision-cylinder model is used to understand mean free path. The model is useful because it connects collision rate with

a) the colour of the gas

b) swept volume per unit path length

c) the gravitational weight of the container

d) the number of thermometer markings

49 / 50

49. 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 every molecule in Curve II moves faster than every molecule in Curve I

c) , and Curve II represents fewer molecules

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

50 / 50

50. Assertion: A gas appears continuous to the eye even though it is made of molecules.
Reason: The number of molecules in an ordinary gas sample is extremely large and each molecule is too small to be seen individually.

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

b) Assertion is false, but Reason is true

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

d) Assertion is true, but Reason is false

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Kinetic Theory Mock Test – Class 11 Physics

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