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.  ${\mathrm{C}}_{\mathrm{V}}-{\mathrm{C}}_{\mathrm{P}}=\mathrm{J}$

The ratio of the specific heats $\frac{{\mathrm{C}}_{\mathrm{P}}}{{\mathrm{C}}_{\mathrm{V}}}=\gamma$ in terms of degrees of freedom (\(n\)) is given by:
1. \(1+1/n\)
2. \(1+n/3\)
3. \(1+2/n\)
4. \(1+n/2\)

The figure shows a process for a gas in which pressure (P) and volume (V) of the gas change. If $C_1$ and $C_2$ are the molar heat capacities of the gas during the processes AB and BC respectively, then:

1. $C_1=C_2$

2. $C_1>C_2$

3. $C_1<C_2$

4. $C_1\le C_2$

The specific heat of an ideal gas is:

1.  proportional to $\mathrm{T.}$                     

2.  proportional to T².

3.  proportional to T³.                  

4.  independent of $\mathrm{T.}$

For hydrogen gas \(C_P-C_V=a\) and for oxygen gas \(C_P-C_V=b\) where molar specific heats are given. So the relation between \(a\) and \(b\) is given by: (where \(C_p\) and \(C_V\) in J mol^-1 K^-1)
1. \(a=16b\)
2. \(b=16a\)
3. \(a=4b\)
4. \(a=b\)