The correct relation between $\gamma = \frac{C_p}{C_v}$ and temperature $T$ is:

For a monoatomic gas,work done at constant pressure is $W$. The heat supplied at constant volume for the same rise in temperature of the gas is

On giving an equal amount of heat at constant volume to $1 \, mol$ of a monoatomic and a diatomic gas,the rise in temperature $(\Delta T)$ is more for:

The ratio of the molar specific heat capacities of monatomic and diatomic gases at constant pressure is (in $: 7$)

To increase the temperature of $2$ moles of an ideal gas by $30^{\circ}C$ to $35^{\circ}C$ at constant pressure,$70 \, cal$ of heat is required. How much heat energy in $cal$ is required to increase the temperature by the same amount at constant volume? $(R = 2 \, cal/mol \cdot K)$

Match the following ( $f$ is number of degrees of freedom):

	Gases		$C_P/C_V$ value
$A$	Monoatomic	$I$	$(4+f)/(3+f)$
$B$	Diatomic (rigid)	$II$	$5/3$
$C$	Diatomic (non-rigid)	$III$	$7/5$
$D$	Polyatomic	$IV$	$9/7$