$A$ gas in a closed container undergoes the cycle $ABCA$ as shown in the figure. The net heat released by the gas after it has undergone $20$ cycles is (in $\,kJ$)

$A$ system goes from $A$ to $B$ via two processes $I$ and $II$ as shown in the figure. If $\Delta U_I$ and $\Delta U_{II}$ are the changes in internal energies in the processes $I$ and $II$ respectively,then:

Three moles of an ideal monatomic gas perform a cyclic process as shown in the figure. The temperatures in different states are $T_1 = 400\,K, T_2 = 800\,K, T_3 = 2400\,K$ and $T_4 = 1200\,K$. Determine the work done by the gas during the cycle in $kJ$. (Given $R = 8.31\, J\, mol^{-1} K^{-1}$)

In the $P-V$ diagram,$I$ is the initial state and $F$ is the final state. The gas goes from $I$ to $F$ by $(i) IAF, (ii) IBF, (iii) ICF$. The heat absorbed by the gas is

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

An ideal gas has undergone a cyclic process as shown in the figure. The work done by the gas in the entire cycle is . . . . . . $\times 10^{-1} \ J$. (Take $\pi = 3.14$)