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%
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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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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. \({ }_{235} \mathrm{UF}_6\)
2. \({ }_{238} \mathrm{UF}_6\)
3. Both will have the same average speed.
4. Data insufficient

Subtopic:  Types of Velocities |
 74%
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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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To find out the degree of freedom, the correct expression is:

1. f=2γ-1

2. f=γ+12

3. f=2γ+1

4. f=1γ+1

Subtopic:  Law of Equipartition of Energy |
 82%
From NCERT
AIPMT - 2000
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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 |
From NCERT
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