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 ......... $\text{calories}$ $(R = 2 \, \text{cal/mol} \cdot \text{K})$.

If the specific heats of a monoatomic gas and a diatomic gas are the same, which relation is valid?

$105 \, cal$ of heat is required to raise the temperature of $3 \, moles$ of an ideal gas at constant pressure from $30^{\circ} C$ to $35^{\circ} C$. The amount of heat required in calories to raise the temperature of the gas through the range ($60^{\circ} C$ to $65^{\circ} C$) at constant volume is ........ $cal$ $(\gamma = \frac{C_p}{C_v} = 1.4)$.

At constant volume,the specific heat of a gas is $\frac{3R}{2}$. Then the value of $\gamma$ will be ....

What is the correct relationship between molar specific heat at constant pressure $(C_P)$ and constant volume $(C_V)$? ($R$ is the universal gas constant)

The molar specific heat at constant pressure of an ideal gas is $\frac{7}{2} R$. The gas is made up of molecules which are ( $R$ is the universal gas constant)