An amount of $700 \,J$ of heat is transferred to a diatomic gas, allowing it to expand with the pressure held constant. The work done by the gas is (in $\,J$)

Half a mole of an ideal monoatomic gas is heated at a constant pressure of $1\, atm$ from $20\,^oC$ to $90\,^oC$. The work done by the gas is close to ..... $J$ (Gas constant $R = 8.31\, J/mol\cdot K$).

For an isochoric process,if $T_1 = 27 \, ^\circ C$ and $T_2 = 127 \, ^\circ C$,then $P_1 / P_2 = \dots$

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

$dQ$ 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:

$A$ graph is drawn between absolute temperature and volume of $3$ moles of helium gas as shown in the figure. If $5 \text{ cal}$ of heat is used in the process, then the work done is (in $\text{ J}$)