$A$ constant amount of an ideal gas undergoes the cyclic process $ABCA$ in the $p-V$ graph shown below. The path $BC$ is an isothermal process. The work done by the gas during one complete cycle,beginning and ending at $A$,is nearly .......... $kJ$.

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 $R$)

$A$ sample of an ideal gas is taken through the cyclic process $abca$ as shown in the figure. The change in the internal energy of the gas along the path $ca$ is $-180\, J$. The gas absorbs $250\, J$ of heat along the path $ab$ and $60\, J$ along the path $bc$. The work done by the gas along the path $abc$ is ..... $J$.

The given diagram shows an ideal gas taken from state $1$ to $2$ through three different paths $A, B,$ and $C$. Let $Q, W,$ and $\Delta U$ represent the heat supplied to the gas,the work done by the gas,and the change in internal energy of the gas,respectively. Then which of the following conditions is true?

$A$ thermodynamic system is taken through the cyclic process $ABC$ as shown in the figure ($P-V$ graph: $A(2, 100)$, $B(5, 300)$, $C(5, 100)$). The total work done by the system during the cycle $ABC$ is . . . . . . $J$.

In the given figure, $1$ represents isobaric, $2$ represents isothermal, and $3$ represents adiabatic processes of an ideal gas. If $\Delta U_{1}, \Delta U_{2}, \Delta U_{3}$ are the changes in internal energy in these processes respectively, then: