An increase in the temperature of a gas-filled in a container would lead to:

 1 decrease in the intermolecular distance. 2 increase in its mass. 3 increase in its kinetic energy. 4 decrease in its pressure.

Subtopic: Â Kinetic Energy of an Ideal Gas |
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If the pressure of a gas is doubled, then the average kinetic energy per unit volume of the gas will be:

 1 half of its initial value. 2 double its initial value. 3 one-fourth of its initial value. 4 four times its initial value.
Subtopic: Â Kinetic Energy of an Ideal Gas |
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The ratio of the average translatory kinetic energy of He gas molecules to ${\mathrm{O}}_{2}$ gas molecules is:

1. $\frac{25}{21}$

2. $\frac{21}{25}$

3. $\frac{3}{2}$

4. 1

Subtopic: Â Kinetic Energy of an Ideal Gas |
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A gas at pressure ${\mathrm{P}}_{0}$ is contained in a vessel. If the masses of all the molecules are halved and their speeds doubled, the resulting pressure would be:

1. $4{\mathrm{P}}_{0}$

2. $2{\mathrm{P}}_{0}$

3. ${\mathrm{P}}_{0}$

4. $\frac{{\mathrm{P}}_{0}}{2}$

Subtopic: Â Kinetic Energy of an Ideal Gas |
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The translational kinetic energy of moles of a diatomic gas at absolute temperature is given by:
1. $\frac{5}{2}nRT$
2. $\frac{3}{2}nRT$
3. $\mathit{5}nRT$
4. $\frac{7}{2}nRT$

Subtopic: Â Kinetic Energy of an Ideal Gas |
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If at a pressure of $$10^6$$ dyne/cm2, one gram of nitrogen occupies $$2\times10^4$$ c.c. volume, then the average energy of a nitrogen molecule in erg is:

 1 $$14\times10^{-13}$$ 2 $$10\times10^{-12}$$ 3 $$10^{6}$$ 4 $$2\times10^{6}$$
Subtopic: Â Kinetic Energy of an Ideal Gas |
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The translatory kinetic energy of a gas per $$\text{g}$$ is:

 1 $${3 \over 2}{RT \over N}$$ 2 $${3 \over 2}{RT \over M}$$ 3 $${3 \over 2}RT$$ 4 $${3 \over 2}NKT$$
Subtopic: Â Kinetic Energy of an Ideal Gas |
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Without change in temperature, a gas is forced in a smaller volume. Its pressure increases because its molecules:

 1 strike the unit area of the container wall more often. 2 strike the unit area of the container wall at a higher speed. 3 strike the unit area of the container wall with greater force. 4 have more energy.

Subtopic: Â Kinetic Energy of an Ideal Gas |
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Diatomic molecules like hydrogen have energies due to both translational as well as rotational motion. From the equation in kinetic theory, $$PV = \frac{2}{3}E$$$,$ $$E$$ is:

 1 the total energy per unit volume. 2 only the translational part of energy because rotational energy is very small compared to translational energy. 3 only the translational part of the energy because during collisions with the wall, pressure relates to change in linear momentum. 4 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.

Subtopic: Â Kinetic Energy of an Ideal Gas |
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Heat is  associated with:

 1 kinetic energy of random motion of molecules. 2 kinetic energy of orderly motion of molecules. 3 total kinetic energy of random and orderly motion of molecules. 4 kinetic energy of random motion in some cases and kinetic energy of orderly motion in other cases.

Subtopic: Â Kinetic Energy of an Ideal Gas |
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