The heat energy supplied to a diatomic gas at constant pressure is $210 \,J$. Then, the work done by the gas is: (in $\,J$)

$A$ 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 $7.03 \, cal/mol-K$).

If $R$ is the universal gas constant,the amount of heat needed to raise the temperature of $2$ moles of an ideal monoatomic gas from $273 \ K$ to $373 \ K$ when no work is done is: (in $R$)

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:

$dQ$ is the heat energy supplied to an ideal gas under isochoric conditions. If $dU$ and $dW$ denote the change in internal energy and the work done respectively,then:

$A$ sample of an ideal gas $(\gamma = 5/3)$ is heated at constant pressure. If $100 \ J$ of heat is supplied to the gas,the work done by the gas is: (in $J$)