The values of $C_P$ and $C_V$ for a gas were measured by three different students. The unit is $\text{cal/g mol-K}$. Which set is the most reliable?

The specific heat relation for an ideal gas is:

The molar specific heat of an ideal gas at constant pressure and constant volume is $C_p$ and $C_v$ respectively. If $R$ is the universal gas constant and the ratio of $C_p$ to $C_v$ is $\gamma$,then $C_v$ is equal to:

$A$ polyatomic gas with $6$ degrees of freedom does $25 \ J$ of work when it is expanded at constant pressure. The heat given to the gas is ..... $J$.

Specific heats of an ideal gas at constant pressure and volume are denoted by $C_p$ and $C_v$ respectively. If $\gamma = \frac{C_p}{C_v}$ and $R$ is the universal gas constant,then $C_v$ is equal to:

When $300 \ J$ of heat is given to an ideal gas with $C_{p} = \frac{7}{2} R$, its temperature rises from $20^{\circ}C$ to $50^{\circ}C$ while keeping its volume constant. The mass of the gas is (approximately) . . . . . . g. (Assume the molar mass of the gas is $28 \ g/mol$ and $R = 8.314 \ J/mol \cdot K$).