The amount of heat required to raise the temperature of $2$ moles of helium gas from $0^{\circ}C$ to $100^{\circ}C$ at constant volume and constant pressure,respectively,is:

$306 \ J$ of heat is required to raise the temperature of $2 \ moles$ of an ideal gas at constant pressure from $25^{\circ} C$ to $35^{\circ} C$. The amount of heat required to raise the temperature of the same gas through the same range at constant volume is (in $J$)

For a gas,$\frac{R}{C_{V}} = 0.4$,where $R$ is the universal gas constant and $C_{V}$ is the molar specific heat at constant volume. The gas is made up of molecules which are

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

Match the List-$I$ with List-$II$:

List-$I$	List-$II$
$A$. Triatomic rigid gas	$I$. $\frac{C_P}{C_V} = \frac{5}{3}$
$B$. Diatomic non-rigid gas	$II$. $\frac{C_P}{C_V} = \frac{7}{5}$
$C$. Monoatomic gas	$III$. $\frac{C_P}{C_V} = \frac{4}{3}$
$D$. Diatomic rigid gas	$IV$. $\frac{C_P}{C_V} = \frac{9}{7}$

Choose the correct answer from the options given below:

The ratio of two specific heats $\frac{C_P}{C_V}$ of $CO$ is