Two cylinders contain the same amount of an ideal monatomic gas. The same amount of heat is given to both cylinders. If the temperature rise in cylinder $A$ is $T_0$,then the temperature rise in cylinder $B$ will be:

$A$ diatomic ideal gas undergoes a thermodynamic change according to the $P-V$ diagram shown in the figure. The heat given to the gas in process $AB$ is: (in $, P_0 V_0$)

In an isobaric process of an ideal gas, the ratio of work done by the system $(W)$ during the expansion and the heat exchanged $(Q)$ is $(\gamma = \frac{C_p}{C_v})$

The ratio of specific heats of a gas is $\gamma$. The change in internal energy of one mole of the gas, when the volume changes from $V$ to $2V$ at constant pressure $p$, is:

One mole of an ideal gas is contained within a cylinder by a frictionless piston and is initially at temperature $T$. The pressure of the gas is kept constant while it is heated and its volume doubles. If $R$ is the molar gas constant,the work done by the gas in increasing its volume is

Which of the following relations is correct for an isochoric process?