# The relation between two specific heats (in cal/mol) of a gas is: 1.  ${\mathrm{C}}_{\mathrm{P}}-{\mathrm{C}}_{\mathrm{V}}=\frac{\mathrm{R}}{\mathrm{J}}$                                2.  ${\mathrm{C}}_{\mathrm{V}}-{\mathrm{C}}_{\mathrm{P}}=\frac{\mathrm{R}}{\mathrm{J}}$ 3.  ${\mathrm{C}}_{\mathrm{P}}-{\mathrm{C}}_{\mathrm{V}}=\mathrm{J}$                                  4.  ${\mathrm{C}}_{\mathrm{V}}-{\mathrm{C}}_{\mathrm{P}}=\mathrm{J}$

Subtopic:  Specific Heat |
88%
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If the mean free path of atoms is doubled , then the pressure of the gas will become:

1. P/4

2. P/2

3. P/8

4. P

Subtopic:  Mean Free Path |
72%
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What is the velocity of a wave in a monoatomic gas having pressure 1 kilopascal and density  ?

1.

2.

3.  Zero

4.  None of these

Subtopic:  Types of Velocities |
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If the ratio of vapour density for hydrogen and oxygen is $$1 \over 16$$, then under constant pressure, the ratio of their rms velocities will be:

 1 $$4 \over 1$$ 2 $$1 \over 4$$ 3 $$1 \over 16$$ 4 $$16 \over 1$$
Subtopic:  Types of Velocities |
77%
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If $$V_\text{H}$$,$$V_\text{N}$$ and $$V_\text{O}$$ denote the root-mean square velocities of molecules of hydrogen, nitrogen and oxygen respectively at a given temperature, then:
1. $$V_\text{N}>V_\text{O}>V_\text{H}$$
2. $$V_\text{H}>V_\text{N}>V_\text{O}$$
3. $$V_\text{O}>V_\text{N}>V_\text{H}$$
4. $$V_\text{O}>V_\text{H}>V_\text{N}$$

Subtopic:  Types of Velocities |
90%
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Two thermally insulated vessels $$1$$ and $$2$$ are filled with air at temperatures $$\mathrm{T_1},$$ $$\mathrm{T_2},$$ volume $$\mathrm{V_1},$$ $$\mathrm{V_2}$$ and pressure $$\mathrm{P_1},$$ $$\mathrm{P_2}$$ respectively. If the valve joining the two vessels is opened, the temperature inside the vessel at equilibrium will be:

 1 $$T_1+T_2$$ 2 $$\dfrac{T_1+T_2}{2}$$ 3 $$\dfrac{T_1T_2(P_1V_1+P_2V_2)}{P_1V_1T_2+P_2V_2T_1}$$ 4 $$\dfrac{T_1T_2(P_1V_1+P_2V_2)}{P_1V_1T_1+P_2V_2T_2}$$
Subtopic:  Ideal Gas Equation |
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The rms speed of oxygen atoms is v. If the temperature is halved and the oxygen atoms combine to form oxygen molecules, then the rms speed will be:

1. $\frac{v}{\sqrt{2}}$

2. $v\sqrt{2}$

3. 2v

4. $\frac{v}{2}$

Subtopic:  Types of Velocities |
70%
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The pressure in a diatomic gas increases from ${\mathrm{P}}_{0}$ to $3{\mathrm{P}}_{0}$, when its volume is increased from ${\mathrm{V}}_{0}$ $\mathrm{to}$ $2{\mathrm{V}}_{0}$. The increase in internal energy  will be:

1. $6{\mathrm{P}}_{\mathrm{o}}{\mathrm{V}}_{0}$

2. $8.5{\mathrm{P}}_{\mathrm{o}}{\mathrm{V}}_{0}$

3. $12.5{\mathrm{P}}_{\mathrm{o}}{\mathrm{V}}_{0}$

4. $14.5{\mathrm{P}}_{\mathrm{o}}{\mathrm{V}}_{0}$

Subtopic:  Law of Equipartition of Energy |
66%
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How does the pressure of an ideal gas change during the process shown in the diagram?

 1 pressure increases continuously. 2 pressure decreases continuously. 3 pressure first increases and then decreases. 4 pressure first decreases and then increases.

Subtopic:  Ideal Gas Equation |
56%
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In the PV graph shown below for an ideal diatomic gas, the change in the internal energy is:

1. $\frac{3}{2}\mathrm{P}\left({\mathrm{V}}_{2}-{\mathrm{V}}_{1}\right)$

2. $\frac{5}{2}\mathrm{P}\left({\mathrm{V}}_{2}-{\mathrm{V}}_{1}\right)$

3. $\frac{3}{2}\mathrm{P}\left({\mathrm{V}}_{1}-{\mathrm{V}}_{2}\right)$

4. $\frac{7}{2}\mathrm{P}\left({\mathrm{V}}_{1}-{\mathrm{V}}_{2}\right)$

Subtopic:  Law of Equipartition of Energy |
80%
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