Question 1

At what temperature is the root mean square speed of an argon atom equal to that of a helium atom at $-20^\circ C$?

Accepted Answer

Correct Option: C. Solution: The root mean square speed $v_{rms}$ is given by $v_{rms} = \sqrt{\frac{3k_BT}{m}}$. For argon and helium to have the same $v_{rms}$, $\frac{T_{Ar}}{M_{Ar}} = \frac{T_{He}}{M_{He}}$. Solving for $T_{Ar}$ with $T_{He} = 253 K$ gives $T_{Ar} = 525 K$, which is approximately $252^\circ C$.

Question 2

Consider a diatomic gas such as $O_2$. According to the kinetic theory of gases, what is the total internal energy of one mole of this gas at temperature $T$, assuming it behaves as a rigid rotator?

Accepted Answer

Correct Option: B. Solution: For a diatomic gas treated as a rigid rotator, it has 3 translational and 2 rotational degrees of freedom. According to the law of equipartition of energy, each degree of freedom contributes $\frac{1}{2}k_BT$ to the energy. Therefore, the total internal energy per mole is $E = \frac{5}{2}RT$.

Question 3

Which of the following equations represents the Ideal Gas Law?

Accepted Answer

Correct Option: A. Solution: The Ideal Gas Law is represented by the equation $PV = nRT$, where $P$ is pressure, $V$ is volume, $n$ is the number of moles, $R$ is the universal gas constant, and $T$ is temperature.

Question 4

If a diatomic gas molecule has a vibrational mode in addition to translational and rotational modes, how does this affect its specific heat capacity?

Accepted Answer

Correct Option: A. Solution: The inclusion of vibrational modes adds additional energy modes, increasing the specific heat capacity as each vibrational mode contributes $2 	imes \frac{1}{2} k_B T$ to the energy.

Question 5

Given the relation for the pressure of an ideal gas $P = \frac{1}{3}nmv^2$, where $n$ is the number density, $m$ is the molecular mass, and $v^2$ is the mean squared speed, what happens to the pressure if the mean squared speed of the gas molecules is doubled while keeping $n$ and $m$ constant?

Accepted Answer

Correct Option: B. Solution: According to the equation $P = \frac{1}{3}nmv^2$, if $v^2$ is doubled, the pressure $P$ will also double, assuming $n$ and $m$ remain constant.

Question 6

In a mixture of gases, how is the total pressure related to the partial pressures of the individual gases?

Accepted Answer

Correct Option: B. Solution: According to Dalton's law of partial pressures, the total pressure of a mixture of gases is the sum of the partial pressures of the individual gases.

Question 7

For a diatomic gas, which of the following correctly represents the specific heat capacity at constant volume, $C_v$, according to the law of equipartition of energy?

Accepted Answer

Correct Option: B. Solution: For diatomic gases, considering both translational and rotational degrees of freedom, $C_v = \frac{5}{2}R$.

Question 8

Which of the following statements is true about the specific heat capacities of monatomic and diatomic gases?

Accepted Answer

Correct Option: C. Solution: Monatomic gases have $C_v = \frac{3}{2}R$ while diatomic gases have $C_v = \frac{5}{2}R$ due to additional rotational modes.

Question 9

What is the primary reason that gases at low pressures and high temperatures behave like ideal gases?

Accepted Answer

Correct Option: B. Solution: At low pressures and high temperatures, gas molecules have high kinetic energy and negligible interactions, making them behave like ideal gases.

Question 10

If the pressure of an ideal gas is $P = \frac{1}{3}nmv^2$, and the gas is compressed to half its original volume at constant temperature, what happens to the mean squared speed $v^2$?

Accepted Answer

Correct Option: B. Solution: Since the temperature is constant, the mean squared speed $v^2$ remains constant according to the kinetic theory of gases.

Question 11

A gas is contained in a vessel at standard temperature and pressure (STP). If the mean free path of the molecules is $2.9 	imes 10^{-7} 	ext{ m}$, what is the approximate diameter of the gas molecules?

Accepted Answer

Correct Option: B. Solution: Using the mean free path formula $l = \frac{1}{\sqrt{2\pi nd^2}}$ and knowing $n = 2.7 	imes 10^{25} 	ext{ m}^{-3}$ at STP, rearrange to solve for $d$. Substituting $l = 2.9 	imes 10^{-7} 	ext{ m}$ gives $d \approx 2.0 	imes 10^{-10} 	ext{ m}$.

Question 12

Consider a gas where the mean free path $l$ is given by the equation $l = \frac{1}{\sqrt{2\pi nd^2}}$. If the number density $n$ of the gas is doubled, what happens to the mean free path $l$?

Accepted Answer

Correct Option: B. Solution: The mean free path $l$ is inversely proportional to the number density $n$. Therefore, if $n$ is doubled, $l$ is halved.

Question 13

If the RMS speed of a nitrogen molecule ($N_2$) at 300 K is 500 m/s, what will be its RMS speed at 600 K?

Accepted Answer

Correct Option: B. Solution: The RMS speed is proportional to the square root of the temperature. Doubling the temperature from 300 K to 600 K increases the RMS speed by a factor of $\sqrt{2}$, thus $500 	imes \sqrt{2} \approx 707$ m/s.

Question 14

A mixture of ideal gases is contained in a vessel. If the partial pressures of two gases are 3 atm and 2 atm respectively, what is the total pressure inside the vessel according to Dalton's Law of Partial Pressures?

Accepted Answer

Correct Option: C. Solution: Dalton's Law of Partial Pressures states that the total pressure of a mixture of non-reacting gases is the sum of their partial pressures. Therefore, the total pressure is 3 atm + 2 atm = 5 atm.

Question 15

Which of the following statements about the kinetic theory of gases is correct?

Accepted Answer

Correct Option: B. Solution: According to the kinetic theory of gases, the pressure is due to the collisions of gas molecules with the walls of the container.

Question 16

If the number of moles of gas in a container is doubled while keeping the temperature and volume constant, what happens to the pressure of the gas according to the ideal gas law?

Accepted Answer

Correct Option: B. Solution: According to the ideal gas law, $PV = nRT$. If the number of moles $n$ is doubled while $T$ and $V$ are constant, the pressure $P$ must also double to maintain the equality.

Question 17

Given a diatomic gas with vibrational modes activated at high temperatures, what would be the expected specific heat capacity at constant volume, $C_v$?

Accepted Answer

Correct Option: C. Solution: When vibrational modes are active, each mode contributes an additional $R$ to the specific heat, making $C_v = \frac{9}{2}R$ for diatomic gases.

Question 18

According to Avogadro's hypothesis, which of the following statements is true for equal volumes of different gases at the same temperature and pressure?

Accepted Answer

Correct Option: A. Solution: Avogadro's hypothesis states that equal volumes of gases at the same temperature and pressure contain the same number of molecules.

Question 19

According to the kinetic theory of gases, which of the following statements is true about the mean free path of molecules in a gas at standard temperature and pressure (STP)?

Accepted Answer

Correct Option: C. Solution: The mean free path $l$ is given by the formula $l = \frac{1}{\sqrt{2} \pi d^2 n}$, where $d$ is the diameter of the molecule and $n$ is the number density. Thus, it is inversely proportional to the number density of the gas.

Question 20

For a diatomic gas like $O_2$, how many degrees of freedom are associated with translational and rotational motion?

Accepted Answer

Correct Option: A. Solution: A diatomic molecule like $O_2$ has 3 translational degrees of freedom and 2 rotational degrees of freedom, as it can rotate about two axes perpendicular to the line joining the two atoms.

Question 21

If the root mean square speed of gas molecules is given by $$v_{rms} = \sqrt{\frac{3k_B T}{m}}$$, what happens to $v_{rms}$ if the temperature is quadrupled?

Accepted Answer

Correct Option: A. Solution: The root mean square speed is proportional to the square root of the temperature, so if the temperature is quadrupled, $v_{rms}$ doubles.

Question 22

Which of the following statements correctly describes the law of equipartition of energy for a diatomic molecule?

Accepted Answer

Correct Option: A. Solution: According to the law of equipartition of energy, each translational and rotational degree of freedom contributes $\frac{1}{2}k_B T$ to the energy of the molecule.

Question 23

Which of the following conditions would cause a real gas to deviate most from ideal gas behavior?

Accepted Answer

Correct Option: B. Solution: Real gases deviate most from ideal behavior at high pressures and low temperatures because intermolecular forces and the volume occupied by the gas molecules become significant.

Question 24

How does the kinetic theory explain the behavior of gases at low pressures and high temperatures?

Accepted Answer

Correct Option: A. Solution: At low pressures and high temperatures, the molecules are far apart, and molecular interactions are negligible, making gases behave more like ideal gases.

Question 25

In a diffusion experiment, two gases, $A$ and $B$, diffuse through a porous barrier. If the molar mass of $A$ is 16 g/mol and that of $B$ is 64 g/mol, what is the ratio of their rates of diffusion ($r_A/r_B$)?

Accepted Answer

Correct Option: B. Solution: According to Graham's law of diffusion, the rate of diffusion is inversely proportional to the square root of the molar mass. Therefore, $r_A/r_B = \sqrt{M_B/M_A} = \sqrt{64/16} = 2:1$.

Question 26

How many rotational degrees of freedom does a diatomic molecule like $O_2$ have?

Accepted Answer

Correct Option: B. Solution: A diatomic molecule like $O_2$ has two rotational degrees of freedom as it can rotate about two axes perpendicular to the line joining the two atoms.

Question 27

Which of the following expressions correctly represents the kinetic interpretation of temperature for an ideal gas?

Accepted Answer

Correct Option: B. Solution: The kinetic interpretation of temperature is given by $T = \frac{2}{3} \frac{PV}{Nk_B}$, which relates temperature to the average kinetic energy of molecules.

Question 28

How does the specific heat capacity at constant volume ($C_v$) for a diatomic gas differ from that of a monatomic gas?

Accepted Answer

Correct Option: B. Solution: The specific heat capacity at constant volume $C_v$ is higher for a diatomic gas because it includes contributions from rotational modes.

Question 29

Which of the following statements about the specific heat capacities of gases is correct?

Accepted Answer

Correct Option: B. Solution: Diatomic gases have $C_v = (5/2)R$ and $C_p = (7/2)R$, considering both translational and rotational modes.

Question 30

Given two gases, hydrogen ($H_2$) and oxygen ($O_2$), at the same temperature, which gas will have a higher root mean square (RMS) speed?

Accepted Answer

Correct Option: A. Solution: The RMS speed is inversely proportional to the square root of the molar mass. Since $H_2$ has a lower molar mass than $O_2$, $H_2$ will have a higher RMS speed.

Question 31

Given the ideal gas equation $$PV = \mu RT$$, if the pressure $P$ is doubled while keeping the number of moles $\mu$ and the gas constant $R$ constant, what happens to the volume $V$ when the temperature $T$ is halved?

Accepted Answer

Correct Option: D. Solution: Using the ideal gas equation $$PV = \mu RT$$, if $P$ is doubled and $T$ is halved, then $V$ must be quartered to maintain the equation.

Question 32

In the kinetic theory of gases, which of the following factors does NOT affect the average kinetic energy of gas molecules?

Accepted Answer

Correct Option: A. Solution: According to the kinetic interpretation of temperature, the average kinetic energy of gas molecules is independent of the type of gas molecules and depends only on the temperature.

Question 33

In an ideal gas, if the number density $n$ is increased by a factor of 4 while keeping the mean squared speed $v^2$ and molecular mass $m$ constant, what is the effect on the pressure $P$?

Accepted Answer

Correct Option: C. Solution: The pressure $P$ is directly proportional to the number density $n$. If $n$ is increased by a factor of 4, then $P$ also increases by a factor of 4.

Question 34

For a diatomic gas, what is the specific heat capacity at constant pressure ($C_p$) considering rotational modes?

Accepted Answer

Correct Option: C. Solution: For a diatomic gas, $C_p = (7/2)R$ considering both translational and rotational modes.

Question 35

According to the kinetic theory, what happens to the average kinetic energy of gas molecules when the temperature is increased?

Accepted Answer

Correct Option: C. Solution: The average kinetic energy of gas molecules is directly proportional to the absolute temperature. Therefore, as the temperature increases, the average kinetic energy also increases.

Question 36

A gas cylinder contains a mixture of neon and oxygen gases. If the partial pressures of neon and oxygen are in the ratio 3:2, what is the ratio of the number of moles of neon to oxygen?

Accepted Answer

Correct Option: B. Solution: The partial pressure of a gas is directly proportional to the number of moles. Therefore, if the partial pressures are in the ratio 3:2, the ratio of the number of moles of neon to oxygen is also 3:2.

Question 37

What is the formula for calculating the mean free path ($l$) of molecules in a gas?

Accepted Answer

Correct Option: A. Solution: The mean free path is given by the formula $l = \frac{1}{\sqrt{2} \pi n d^2}$, where $n$ is the number density and $d$ is the molecular diameter.

Question 38

A gas mixture contains 3 moles of nitrogen ($N_2$) and 2 moles of oxygen ($O_2$). If the total pressure of the mixture is 5 atm, what is the partial pressure of oxygen?

Accepted Answer

Correct Option: B. Solution: The partial pressure of a gas is given by the mole fraction times the total pressure. For $O_2$, $$P_{O_2} = \frac{2}{3+2} 	imes 5 = 2 	ext{ atm}$$.

Question 39

In a certain gas, the mean free path is observed to be $3 	imes 10^{-7} 	ext{ m}$. If the molecular diameter $d$ is $2 	imes 10^{-10} 	ext{ m}$, what is the number density $n$ of the gas molecules?

Accepted Answer

Correct Option: A. Solution: Using the formula $l = \frac{1}{\sqrt{2\pi nd^2}}$, rearrange to find $n = \frac{1}{\sqrt{2\pi l d^2}}$. Substituting $l = 3 	imes 10^{-7} 	ext{ m}$ and $d = 2 	imes 10^{-10} 	ext{ m}$ gives $n = 1.5 	imes 10^{25} 	ext{ m}^{-3}$.

Question 40

For a diatomic gas like $O_2$, which of the following statements about degrees of freedom is correct according to the kinetic theory?

Accepted Answer

Correct Option: C. Solution: A diatomic molecule like $O_2$ has 3 translational and 2 rotational degrees of freedom, as it can rotate about two axes perpendicular to the bond axis.

Question 41

According to the kinetic theory of gases, what is the relationship between the temperature of a gas and the average kinetic energy of its molecules?

Accepted Answer

Correct Option: A. Solution: The kinetic theory of gases states that the temperature of a gas is a measure of the average kinetic energy of its molecules.

Question 42

According to the kinetic interpretation of temperature, what does the temperature of a gas measure?

Accepted Answer

Correct Option: B. Solution: The temperature of a gas is a measure of the average kinetic energy of its molecules, independent of the gas type.

Question 43

In a mixture of non-reactive gases, how is the total pressure determined according to Dalton's Law of Partial Pressures?

Accepted Answer

Correct Option: A. Solution: Dalton's Law of Partial Pressures states that the total pressure of a mixture of non-reactive gases is the sum of the partial pressures of each individual gas if it were to occupy the entire volume alone.

Question 44

Consider a gas where the molecular mass $m$ is halved while keeping the number density $n$ and mean squared speed $v^2$ constant. How does this affect the pressure $P$ of the gas?

Accepted Answer

Correct Option: C. Solution: The pressure $P$ is directly proportional to the molecular mass $m$. Halving $m$ will halve the pressure $P$.

Question 45

If the average kinetic energy of a gas molecule is given by $\frac{3}{2} k_B T$, what does $T$ represent in this equation?

Accepted Answer

Correct Option: C. Solution: In the expression $\frac{3}{2} k_B T$, $T$ represents the absolute temperature of the gas.

Question 46

According to the kinetic theory of gases, which of the following statements is true about the relationship between temperature and the average kinetic energy of gas molecules?

Accepted Answer

Correct Option: C. Solution: The kinetic theory of gases states that the average kinetic energy of gas molecules is directly proportional to the absolute temperature, as given by $$E = \frac{3}{2} k_B T$$.

Question 47

If the temperature of a gas is increased, how does it affect the root mean square speed of its molecules?

Accepted Answer

Correct Option: C. Solution: The root mean square speed $v_{rms}$ is proportional to the square root of the temperature $T$. Therefore, as the temperature increases, $v_{rms}$ also increases.

Question 48

In the context of the law of equipartition of energy, which of the following statements is true for a vibrational mode?

Accepted Answer

Correct Option: C. Solution: A vibrational mode contributes $2 	imes \frac{1}{2} k_B T = k_B T$ to the energy, accounting for both kinetic and potential energy components.

Question 49

What is the specific heat capacity at constant volume ($C_v$) for a monatomic gas according to the law of equipartition of energy?

Accepted Answer

Correct Option: A. Solution: For a monatomic gas, the specific heat capacity at constant volume $C_v$ is $(3/2)R$ as it has three translational degrees of freedom.

Question 50

A gas cylinder contains a mixture of two non-reactive gases: helium and argon. If the partial pressures of helium and argon are in the ratio 2:3, what is the ratio of the number of moles of helium to argon in the cylinder?

Accepted Answer

Correct Option: B. Solution: According to Dalton's law of partial pressures, the partial pressure of a gas in a mixture is proportional to the number of moles of the gas. Therefore, the ratio of the number of moles of helium to argon is the inverse of their partial pressure ratio, which is 3:2.

Question 51

In the kinetic theory of gases, the pressure exerted by an ideal gas is due to:

Accepted Answer

Correct Option: B. Solution: The pressure of an ideal gas is due to the elastic collisions of gas molecules with the walls of the container. This is a fundamental aspect of the kinetic theory of gases.

Question 52

A sample of gas is compressed at constant temperature from a volume of 10 L to 5 L. According to Boyle's Law, what happens to the pressure of the gas?

Accepted Answer

Correct Option: A. Solution: Boyle's Law states that for a given mass of gas at constant temperature, the pressure is inversely proportional to the volume. Therefore, halving the volume doubles the pressure.

Question 53

Which of the following correctly describes the law of equipartition of energy?

Accepted Answer

Correct Option: B. Solution: The law of equipartition of energy states that each translational and rotational degree of freedom contributes $\frac{1}{2} k_B T$ to the total energy. Vibrational modes contribute $k_B T$ as they have both kinetic and potential energy components.

Question 54

Which of the following equations correctly represents the relationship between pressure, volume, and temperature for an ideal gas?

Accepted Answer

Correct Option: A. Solution: The ideal gas law is given by $PV = nRT$, where $n$ is the number of moles, $R$ is the universal gas constant, and $T$ is the temperature in Kelvin.

Question 55

What does the kinetic interpretation of temperature imply about the relationship between temperature and the average kinetic energy of gas molecules?

Accepted Answer

Correct Option: A. Solution: The kinetic interpretation of temperature states that temperature is a measure of the average kinetic energy of gas molecules, implying a direct proportionality.

Question 56

If the mean squared speed of gas molecules is doubled, what happens to the pressure of the gas, assuming all other factors remain constant?

Accepted Answer

Correct Option: C. Solution: According to the formula $P = \frac{1}{3}nmv^2$, if $v^2$ is doubled, the pressure $P$ is also doubled.

Question 57

For a monatomic ideal gas, what is the ratio of specific heats $\gamma = \frac{C_p}{C_v}$?

Accepted Answer

Correct Option: A. Solution: For a monatomic ideal gas, $C_v = \frac{3}{2}R$ and $C_p = \frac{5}{2}R$, thus $\gamma = \frac{C_p}{C_v} = \frac{5}{3}$.

Question 58

For a diatomic gas, which of the following statements about its degrees of freedom and specific heat capacities is correct?

Accepted Answer

Correct Option: C. Solution: For a diatomic gas treated as a rigid rotator, it has 5 degrees of freedom (3 translational and 2 rotational). Its molar specific heat at constant pressure $C_P$ is $\frac{7}{2} R$.

Question 59

Which of the following statements about real gases is true at high pressures and low temperatures?

Accepted Answer

Correct Option: B. Solution: At high pressures and low temperatures, real gases deviate significantly from ideal behavior due to increased intermolecular forces and finite molecular volume.

Question 60

If a gas behaves ideally, what is the relationship between pressure, volume, and temperature?

Accepted Answer

Correct Option: A. Solution: For an ideal gas, the relationship is given by the ideal gas equation $PV = nRT$, where $P$ is pressure, $V$ is volume, $n$ is the number of moles, $R$ is the universal gas constant, and $T$ is temperature.

Question 61

For a diatomic gas treated as a rigid rotator, how many degrees of freedom does it have, and what is its molar specific heat at constant volume $C_V$?

Accepted Answer

Correct Option: A. Solution: A diatomic molecule treated as a rigid rotator has 3 translational and 2 rotational degrees of freedom, totaling 5. The molar specific heat at constant volume is $C_V = \frac{5}{2} R$.

Question 62

A vessel contains a mixture of helium ($He$) and argon ($Ar$) at the same temperature. Which gas will have a higher average kinetic energy per molecule?

Accepted Answer

Correct Option: C. Solution: The average kinetic energy per molecule of a gas depends only on the temperature and is given by $\frac{3}{2} k_B T$. Since both gases are at the same temperature, their average kinetic energies per molecule are the same.

Question 63

According to the law of equipartition of energy, what is the average energy per degree of freedom for a molecule in thermal equilibrium at temperature $T$?

Accepted Answer

Correct Option: B. Solution: The law of equipartition of energy states that each degree of freedom contributes an average energy of $\frac{1}{2} k_B T$ in thermal equilibrium.

Question 64

If two gases at the same temperature have different molecular masses, how does their average speed compare?

Accepted Answer

Correct Option: A. Solution: At the same temperature, the gas with lighter molecules will have a higher average speed because the average kinetic energy is the same for both gases, but kinetic energy depends on both mass and speed.

Kinetic Theory

Learning Objectives

Learning Objectives

Revision Notes & Summary

Chapter Notes

Kinetic Theory of Gases

Ideal Gas Law

Law of Equipartition of Energy

Mean Free Path

Specific Heat Capacities of Gases

Kinetic Interpretation of Temperature

Pressure of an Ideal Gas

Gas Laws and Real Gas Behaviour

Avogadro Hypothesis and Dalton’s Law of Partial Pressures

RMS Speed and Molecular Speed Calculations

Degrees of Freedom of Molecules

Exam Tips & Common Mistakes

Common Mistakes & Exam Tips

Kinetic Theory of Gases

Ideal Gas Law

Law of Equipartition of Energy

Mean Free Path

Specific Heat Capacities of Gases

Kinetic Interpretation of Temperature

Pressure of an Ideal Gas

Gas Laws and Real Gas Behaviour

Avogadro Hypothesis and Dalton’s Law of Partial Pressures

RMS Speed and Molecular Speed Calculations

Degrees of Freedom of Molecules

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Multiple Choice Questions

Q1.At what temperature is the root mean square speed of an argon atom equal to that of a helium atom at −20∘C-20^\circ C−20∘C?

Correct Answer: C

Q2.Consider a diatomic gas such as O2O_2O2​. According to the kinetic theory of gases, what is the total internal energy of one mole of this gas at temperature TTT, assuming it behaves as a rigid rotator?

Correct Answer: B

Q3.Which of the following equations represents the Ideal Gas Law?

Correct Answer: A

Q4.If a diatomic gas molecule has a vibrational mode in addition to translational and rotational modes, how does this affect its specific heat capacity?

Correct Answer: A

Correct Answer: B

Q6.In a mixture of gases, how is the total pressure related to the partial pressures of the individual gases?

Correct Answer: B

Q7.For a diatomic gas, which of the following correctly represents the specific heat capacity at constant volume, CvC_vCv​, according to the law of equipartition of energy?

Correct Answer: B

Q8.Which of the following statements is true about the specific heat capacities of monatomic and diatomic gases?

Correct Answer: C

Q9.What is the primary reason that gases at low pressures and high temperatures behave like ideal gases?

Correct Answer: B

Q10.If the pressure of an ideal gas is P=13nmv2P = \frac{1}{3}nmv^2P=31​nmv2, and the gas is compressed to half its original volume at constant temperature, what happens to the mean squared speed v2v^2v2?

Correct Answer: B

Q11.A gas is contained in a vessel at standard temperature and pressure (STP). If the mean free path of the molecules is 2.9×10−7 m2.9 \times 10^{-7} \text{ m}2.9×10−7 m, what is the approximate diameter of the gas molecules?

Correct Answer: B

Q12.Consider a gas where the mean free path lll is given by the equation l=12πnd2l = \frac{1}{\sqrt{2\pi nd^2}}l=2πnd2​1​. If the number density nnn of the gas is doubled, what happens to the mean free path lll?

Correct Answer: B

Q13.If the RMS speed of a nitrogen molecule (N2N_2N2​) at 300 K is 500 m/s, what will be its RMS speed at 600 K?

Correct Answer: B

Q14.A mixture of ideal gases is contained in a vessel. If the partial pressures of two gases are 3 atm and 2 atm respectively, what is the total pressure inside the vessel according to Dalton's Law of Partial Pressures?

Correct Answer: C

Q15.Which of the following statements about the kinetic theory of gases is correct?

Correct Answer: B

Q16.If the number of moles of gas in a container is doubled while keeping the temperature and volume constant, what happens to the pressure of the gas according to the ideal gas law?

Correct Answer: B

Q17.Given a diatomic gas with vibrational modes activated at high temperatures, what would be the expected specific heat capacity at constant volume, CvC_vCv​?

Correct Answer: C

Q18.According to Avogadro's hypothesis, which of the following statements is true for equal volumes of different gases at the same temperature and pressure?

Correct Answer: A

Q19.According to the kinetic theory of gases, which of the following statements is true about the mean free path of molecules in a gas at standard temperature and pressure (STP)?

Correct Answer: C

Q20.For a diatomic gas like O2O_2O2​, how many degrees of freedom are associated with translational and rotational motion?

Correct Answer: A

Q21.If the root mean square speed of gas molecules is given by vrms=3kBTmv_{rms} = \sqrt{\frac{3k_B T}{m}}vrms​=m3kB​T​​, what happens to vrmsv_{rms}vrms​ if the temperature is quadrupled?

Correct Answer: A

Q22.Which of the following statements correctly describes the law of equipartition of energy for a diatomic molecule?

Correct Answer: A