The specific heat relation for an ideal gas is:

Obtain the relation between specific heat capacity at constant pressure $(C_P)$ and specific heat capacity at constant volume $(C_V)$ for an ideal gas.

$A$ gas has $n$ degrees of freedom. The ratio of specific heat of gas at constant volume $(C_v)$ to the specific heat of gas at constant pressure $(C_p)$ will be.

The figure shows the graph of logarithmic reading of pressure and volume for two ideal gases $A$ and $B$ undergoing an adiabatic process. From the figure, it can be concluded that:

The relation between two specific heats of a gas is

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