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

Two moles of an ideal monoatomic gas undergo a cyclic process as shown in the figure. The temperatures in different states are given as $6 T_1 = 3 T_2 = 2 T_4 = T_3 = 2400 \text{ K}$. The work done by the gas during the complete cycle is $(R = \text{Universal gas constant})$ (in $R$)

Three different processes that can occur in an ideal monoatomic gas are shown in the $P$ vs $V$ diagram. The paths are labelled as $A \rightarrow B, A \rightarrow C$ and $A \rightarrow D$. The change in internal energies during these processes are taken as $E_{AB}, E_{AC}$ and $E_{AD}$ and the work done as $W_{AB}, W_{AC}$ and $W_{AD}$. The correct relation between these parameters is:

If a gas is taken from $A$ to $C$ through $B$, the heat absorbed by the gas is $8 \, J$. Calculate the heat absorbed by the gas when it is taken from $A$ to $C$ directly.

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

One mole of a gas obeying the equation of state $P(V-b)=RT$ is made to expand from a state with coordinates $(P_{1}, V_{1})$ to a state with $(P_{2}, V_{2})$ along a process that is depicted by a straight line on a $P-V$ diagram. Then, the work done is given by