# To find out the degree of freedom, the correct expression is: 1. $f=\frac{2}{\gamma -1}$ 2. $f=\frac{\gamma +1}{2}$ 3. $f=\frac{2}{\gamma +1}$ 4. $f=\frac{1}{\gamma +1}$

Subtopic:  Law of Equipartition of Energy |
82%
From NCERT
AIPMT - 2000
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The equation of state for 5g of oxygen at a pressure P and temperature T, when occupying a volume V, will be: (where R is the gas constant)
1. PV = 5 RT
2. PV = (5/2) RT
3. PV = (5/16) RT
4. PV = (5/32) RT

Subtopic:  Ideal Gas Equation |
83%
From NCERT
AIPMT - 2004
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Uranium has two isotopes of masses $$235$$ and $$238$$ units. If both are present in Uranium hexafluoride gas, which would have the larger average speed?
1. $$^{235} \mathrm{U} \mathrm{F}_{6}$$
2. $${}^{238} \mathrm{U} \mathrm{F}_{6}$$
3. Both will have the same average speed.
4. Data insufficient

Subtopic:  Types of Velocities |
74%
From NCERT
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A cylinder of fixed capacity $$44.8$$ litres contains helium gas at standard temperature and pressure. What is the amount of heat needed to raise the temperature of the gas in the cylinder by $$15.0^\circ~\mathrm{C}?$$ ($$R=8.31$$ J mol–1 K–1)

 1 $$379$$ J 2 $$357$$ J 3 $$457$$ J 4 $$374$$ J

Subtopic:  Specific Heat |
51%
From NCERT
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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:  Kinetic Energy of an Ideal Gas |
91%
From NCERT
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If $$C_p$$ and $$C_v$$ denote the specific heats (per unit mass) of an ideal gas of molecular weight $$M$$ (where $$R$$ is the molar gas constant), the correct relation is:
1. $$C_p-C_v=R$$
2. $$C_p-C_v=\frac{R}{M}$$
3. $$C_p-C_v=MR$$
4. $$C_p-C_v=\frac{R}{M^2}$$

Subtopic:  Specific Heat |
64%
From NCERT
AIPMT - 2010
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The mean free path $$l$$ for a gas molecule depends upon the diameter, $$d$$ of the molecule as:

 1 $$l\propto \dfrac{1}{d^2}$$ 2 $$l\propto d$$ 3 $$l\propto d^2$$ 4 $$l\propto \dfrac{1}{d}$$
Subtopic:  Mean Free Path |
84%
From NCERT
NEET - 2020
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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, $$PV = \dfrac{2}{3}E$$$,$ $$E$$ 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:  Kinetic Energy of an Ideal Gas |
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$$1$$ mole of an ideal gas is contained in a cubical volume V, ABCDEFGH at $$300$$ K (figure). One face of the cube (EFGH) is made up of a material which totally absorbs any gas molecule incident on it. At any given time:

 1 the pressure on EFGH would be zero. 2 the pressure on all the faces will be equal. 3 the pressure on EFGH would be double the pressure on ABCD. 4 the pressure on EFGH would be half that on ABCD.
Subtopic:  Kinetic Energy of an Ideal Gas |
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When an ideal gas is compressed adiabatically, its temperature rises: the molecules on an average have more kinetic energy than before. The kinetic energy increases:

 1 because of collisions with moving parts of the wall only. 2 because of collisions with the entire wall. 3 because the molecules get accelerated in their motion inside the volume. 4 because of the redistribution of energy amongst the molecules.
Subtopic:  Kinetic Energy of an Ideal Gas |
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