The work done to double the volume of $0.1 \ mol$ of a gas at constant pressure and a temperature of $27 \ ^\circ C$ is equal to ..... $cal$.

$A$ sample of a gas expands from volume $V_1$ to $V_2$. The amount of work done by the gas is maximum when the expansion 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:

The $P-V$ diagram for an ideal gas in a piston-cylinder assembly undergoing a thermodynamic process is shown in the figure. The process 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 $7.03 \, cal/mol-K$).

$0.08 \text{ kg}$ of air is heated at constant volume through $5^{\circ} \text{C}$. The specific heat of air at constant volume is $0.17 \text{ kcal/kg}^{\circ} \text{C}$ and $J = 4.18 \text{ J/cal}$. The change in its internal energy is approximately: (in $\text{ J}$)