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

If $c_p$ and $c_v$ denote the specific heats (per unit mass) of an ideal gas of molecular weight $M$,then which of the following relations holds true,where $R$ is the molar gas constant?

For a gas,the value of $\frac{R}{C_v} = 0.4$. What is the nature of the gas? ($R$ is the universal gas constant)

The energy required to raise the temperature of $5 \, \text{moles}$ of $H_2$ gas from $30^{\circ}C$ to $60^{\circ}C$ at constant pressure is ......... $\text{calories}$ $(R = 2 \, \text{cal/mol} \cdot \text{K})$.

The molar specific heats of an ideal gas at constant pressure and constant volume are denoted by $C_P$ and $C_V$ respectively. If $\gamma = C_P/C_V$ and $R$ is the universal gas constant,then $C_V = $ ........

Write the value of $\frac{C_P}{C_V}$ for a monoatomic gas.