For a gas molecule with $6$ degrees of freedom,which one of the following relations between gas constant '$R$' and molar specific heat '$C_{V}$' is correct?

$5$ moles of oxygen is heated at constant volume from $10^{\circ}C$ to $20^{\circ}C$. The change in the internal energy of the gas is (given $C_p = 8 \text{ cal/mole } ^{\circ}C$ and $R = 2 \text{ cal/mole } ^{\circ}C$ approximately).

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

Can we use the degree of freedom to obtain the specific heat capacity of a gas? Explain.

If a gas has $n$ degrees of freedom,the ratio of specific heats of the gas is:

$C_{v}$ and $C_{p}$ denote the molar specific heat capacities of a gas at constant volume and constant pressure,respectively. Then
$(A)$ $C_{p}-C_{v}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas
$(B)$ $C_{p}+C_{v}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas
$(C)$ $C_{p} / C_{v}$ is larger for a diatomic ideal gas than for a monoatomic ideal gas
$(D)$ $C_{p} \cdot C_v$ is larger for a diatomic ideal gas than for a monoatomic ideal gas