$A$ gas expands under constant pressure $P$ from volume $V_1$ to $V_2$. The work done by the gas is

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:

$A$ container having $1$ mole of a gas at a temperature $27^{\circ}C$ has a movable piston which maintains a constant pressure in the container of $1 \, atm$. The gas is compressed until the temperature becomes $127^{\circ}C$. The work done is ........ $J$ ($C_P$ for the gas is $7.03 \, cal/mol-K$).

Which one of the following $p-V$ diagrams is correct for an isochoric process?

An ideal monoatomic gas expands at constant pressure. The work done by the gas on its environment is $200 \,J$, then the heat absorbed by the gas during the process is (in $\,J$)

$A$ 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 $, P_0 V_0$)