$306 \ J$ 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 $J$)

The amount of heat energy required to raise the temperature of $1\, g$ of Helium at $NTP$ from $T_1\, K$ to $T_2\, K$ is:

If $\gamma$ is the ratio of specific heats and $R$ is the universal gas constant,then the molar specific heat at constant volume $C_{V}$ is given by

The adiabatic Bulk modulus of a diatomic gas at atmospheric pressure is

Which of the following statements is correct regarding the molar specific heat of $1$ mole of an ideal gas at constant pressure $(C_P)$ and constant volume $(C_V)$?

$5 \ \text{moles}$ of an unknown gas is heated at constant volume from $10^\circ \text{C}$ to $20^\circ \text{C}$. The molar specific heat of this gas at constant pressure is $c_p = 8 \ \text{cal/mol} \cdot ^\circ \text{C}$ and the gas constant is $R = 8.36 \ \text{J/mol} \cdot ^\circ \text{C}$. The change in the internal energy of the gas is . . . . . . calorie.