If $C_p$ and $C_v$ are molar specific heats of an ideal gas at constant pressure and volume respectively,if $\gamma$ is the ratio of the two specific heats and $R$ is the universal gas constant,then $C_p$ is equal to

$105 \, cal$ 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 ........ $cal$ $(\gamma = \frac{C_p}{C_v} = 1.4)$.

Obtain the equation for $\gamma = \frac{C_P}{C_V}$ in terms of the degree of freedom $f$.

For an ideal gas of diatomic molecules,which of the following relations is correct?

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

For a gas,$R/C_V = 0.67$. What kind of molecules is this gas made of?