An ideal gas follows the path shown in the figure. The net work done in the whole cycle is

Work done by a gas in the process shown in the figure will be

The $P-V$ diagram shown below indicates two paths along which a sample of gas can be taken from state $A$ to state $B$. The energy equal to $5PV$ in the form of heat is required to be transferred if Path-$1$ is chosen. How much energy in the form of heat should be transferred if Path-$2$ is chosen?

In a thermodynamic process,the pressures and volumes corresponding to some points in the figure are $P_A = 3 \times 10^4 \, Pa$,$V_A = 2 \times 10^{-3} \, m^3$,$P_B = 8 \times 10^4 \, Pa$,and $V_D = 5 \times 10^{-3} \, m^3$. In process $AB$,$600 \, J$ of heat is added,and in process $BC$,$200 \, J$ of heat is added to the system. The change in the internal energy in process $AC$ would be .... $J$.

One mole of an ideal monoatomic gas is taken along the path $ABCA$ as shown in the $PV$ diagram. The maximum temperature attained by the gas along the path $BC$ is given by

The heat energy absorbed by a system in going through the cyclic process shown in the figure is: