Degree of Freedom, Various speeds of Gas Molecules
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Kinetic Theory of Gases

139135 A flask of volume $0.1 \mathrm{~m}^{3}$ contains $\mathrm{He}$ (monatomic) and $\mathrm{O}_{2}$ (diatomic) gases in the ratio 4:1 The flask is maintained at a temperature $27^{\circ} \mathrm{C}$. The ratio of the $\mathrm{rms}$ speeds of the $\mathrm{He}$ - atoms and $\mathrm{O}_{2}$-molecules is
(Atomic mass of $\mathrm{He}=4 \mathrm{amu}$, and oxygen $=16$ amu)

1 $2: 1$
2 $4: 1$
3 $2 \sqrt{2}: 1$
4 $\sqrt{2}: 1$
Shift-I]
Kinetic Theory of Gases

139137 If the volume of a gas is reduced to half then the change in its mean free path is

1 Becomes half
2 Unchanged
3 Doubles
4 Depend on temperature
Shift-I]
Kinetic Theory of Gases

139147 Following statements are given:

1 (1) and (4) only
2 (1), (2) and (4) only
3 (2) and (4) only
4 (1), (2) and (5) only
Shift-I]
Kinetic Theory of Gases

139169 The mean kinetic energy of a vibrating diatomic molecule with two vibrational modes is $(\mathrm{k}=$ Boltzman constant and $T=$ Temperature)

1 $\frac{9}{2} \mathrm{kT}$
2 $\frac{3}{2} \mathrm{kT}$
3 $\frac{5}{2} \mathrm{kT}$
4 $\frac{7}{2} \mathrm{kT}$
So
Kinetic Theory of Gases

139173 Average kinetic energy of $\mathrm{H}_{2}$ molecule at $300 \mathrm{~K}$ is ' $E$ '. At the same temperature, average kinetic energy of $\mathrm{O}_{2}$ molecule will be

1 $\frac{E}{4}$
2 $\frac{E}{2}$
3 $\frac{E}{8}$
4 $\mathrm{E}$
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Kinetic Theory of Gases

139135 A flask of volume $0.1 \mathrm{~m}^{3}$ contains $\mathrm{He}$ (monatomic) and $\mathrm{O}_{2}$ (diatomic) gases in the ratio 4:1 The flask is maintained at a temperature $27^{\circ} \mathrm{C}$. The ratio of the $\mathrm{rms}$ speeds of the $\mathrm{He}$ - atoms and $\mathrm{O}_{2}$-molecules is
(Atomic mass of $\mathrm{He}=4 \mathrm{amu}$, and oxygen $=16$ amu)

1 $2: 1$
2 $4: 1$
3 $2 \sqrt{2}: 1$
4 $\sqrt{2}: 1$
Shift-I]
Kinetic Theory of Gases

139137 If the volume of a gas is reduced to half then the change in its mean free path is

1 Becomes half
2 Unchanged
3 Doubles
4 Depend on temperature
Shift-I]
Kinetic Theory of Gases

139147 Following statements are given:

1 (1) and (4) only
2 (1), (2) and (4) only
3 (2) and (4) only
4 (1), (2) and (5) only
Shift-I]
Kinetic Theory of Gases

139169 The mean kinetic energy of a vibrating diatomic molecule with two vibrational modes is $(\mathrm{k}=$ Boltzman constant and $T=$ Temperature)

1 $\frac{9}{2} \mathrm{kT}$
2 $\frac{3}{2} \mathrm{kT}$
3 $\frac{5}{2} \mathrm{kT}$
4 $\frac{7}{2} \mathrm{kT}$
So
Kinetic Theory of Gases

139173 Average kinetic energy of $\mathrm{H}_{2}$ molecule at $300 \mathrm{~K}$ is ' $E$ '. At the same temperature, average kinetic energy of $\mathrm{O}_{2}$ molecule will be

1 $\frac{E}{4}$
2 $\frac{E}{2}$
3 $\frac{E}{8}$
4 $\mathrm{E}$
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Kinetic Theory of Gases

139135 A flask of volume $0.1 \mathrm{~m}^{3}$ contains $\mathrm{He}$ (monatomic) and $\mathrm{O}_{2}$ (diatomic) gases in the ratio 4:1 The flask is maintained at a temperature $27^{\circ} \mathrm{C}$. The ratio of the $\mathrm{rms}$ speeds of the $\mathrm{He}$ - atoms and $\mathrm{O}_{2}$-molecules is
(Atomic mass of $\mathrm{He}=4 \mathrm{amu}$, and oxygen $=16$ amu)

1 $2: 1$
2 $4: 1$
3 $2 \sqrt{2}: 1$
4 $\sqrt{2}: 1$
Shift-I]
Kinetic Theory of Gases

139137 If the volume of a gas is reduced to half then the change in its mean free path is

1 Becomes half
2 Unchanged
3 Doubles
4 Depend on temperature
Shift-I]
Kinetic Theory of Gases

139147 Following statements are given:

1 (1) and (4) only
2 (1), (2) and (4) only
3 (2) and (4) only
4 (1), (2) and (5) only
Shift-I]
Kinetic Theory of Gases

139169 The mean kinetic energy of a vibrating diatomic molecule with two vibrational modes is $(\mathrm{k}=$ Boltzman constant and $T=$ Temperature)

1 $\frac{9}{2} \mathrm{kT}$
2 $\frac{3}{2} \mathrm{kT}$
3 $\frac{5}{2} \mathrm{kT}$
4 $\frac{7}{2} \mathrm{kT}$
So
Kinetic Theory of Gases

139173 Average kinetic energy of $\mathrm{H}_{2}$ molecule at $300 \mathrm{~K}$ is ' $E$ '. At the same temperature, average kinetic energy of $\mathrm{O}_{2}$ molecule will be

1 $\frac{E}{4}$
2 $\frac{E}{2}$
3 $\frac{E}{8}$
4 $\mathrm{E}$
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Kinetic Theory of Gases

139135 A flask of volume $0.1 \mathrm{~m}^{3}$ contains $\mathrm{He}$ (monatomic) and $\mathrm{O}_{2}$ (diatomic) gases in the ratio 4:1 The flask is maintained at a temperature $27^{\circ} \mathrm{C}$. The ratio of the $\mathrm{rms}$ speeds of the $\mathrm{He}$ - atoms and $\mathrm{O}_{2}$-molecules is
(Atomic mass of $\mathrm{He}=4 \mathrm{amu}$, and oxygen $=16$ amu)

1 $2: 1$
2 $4: 1$
3 $2 \sqrt{2}: 1$
4 $\sqrt{2}: 1$
Shift-I]
Kinetic Theory of Gases

139137 If the volume of a gas is reduced to half then the change in its mean free path is

1 Becomes half
2 Unchanged
3 Doubles
4 Depend on temperature
Shift-I]
Kinetic Theory of Gases

139147 Following statements are given:

1 (1) and (4) only
2 (1), (2) and (4) only
3 (2) and (4) only
4 (1), (2) and (5) only
Shift-I]
Kinetic Theory of Gases

139169 The mean kinetic energy of a vibrating diatomic molecule with two vibrational modes is $(\mathrm{k}=$ Boltzman constant and $T=$ Temperature)

1 $\frac{9}{2} \mathrm{kT}$
2 $\frac{3}{2} \mathrm{kT}$
3 $\frac{5}{2} \mathrm{kT}$
4 $\frac{7}{2} \mathrm{kT}$
So
Kinetic Theory of Gases

139173 Average kinetic energy of $\mathrm{H}_{2}$ molecule at $300 \mathrm{~K}$ is ' $E$ '. At the same temperature, average kinetic energy of $\mathrm{O}_{2}$ molecule will be

1 $\frac{E}{4}$
2 $\frac{E}{2}$
3 $\frac{E}{8}$
4 $\mathrm{E}$
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Join With Us for More Updates
Kinetic Theory of Gases

139135 A flask of volume $0.1 \mathrm{~m}^{3}$ contains $\mathrm{He}$ (monatomic) and $\mathrm{O}_{2}$ (diatomic) gases in the ratio 4:1 The flask is maintained at a temperature $27^{\circ} \mathrm{C}$. The ratio of the $\mathrm{rms}$ speeds of the $\mathrm{He}$ - atoms and $\mathrm{O}_{2}$-molecules is
(Atomic mass of $\mathrm{He}=4 \mathrm{amu}$, and oxygen $=16$ amu)

1 $2: 1$
2 $4: 1$
3 $2 \sqrt{2}: 1$
4 $\sqrt{2}: 1$
Shift-I]
Kinetic Theory of Gases

139137 If the volume of a gas is reduced to half then the change in its mean free path is

1 Becomes half
2 Unchanged
3 Doubles
4 Depend on temperature
Shift-I]
Kinetic Theory of Gases

139147 Following statements are given:

1 (1) and (4) only
2 (1), (2) and (4) only
3 (2) and (4) only
4 (1), (2) and (5) only
Shift-I]
Kinetic Theory of Gases

139169 The mean kinetic energy of a vibrating diatomic molecule with two vibrational modes is $(\mathrm{k}=$ Boltzman constant and $T=$ Temperature)

1 $\frac{9}{2} \mathrm{kT}$
2 $\frac{3}{2} \mathrm{kT}$
3 $\frac{5}{2} \mathrm{kT}$
4 $\frac{7}{2} \mathrm{kT}$
So
Kinetic Theory of Gases

139173 Average kinetic energy of $\mathrm{H}_{2}$ molecule at $300 \mathrm{~K}$ is ' $E$ '. At the same temperature, average kinetic energy of $\mathrm{O}_{2}$ molecule will be

1 $\frac{E}{4}$
2 $\frac{E}{2}$
3 $\frac{E}{8}$
4 $\mathrm{E}$
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