In the cyclic process given in the $P-V$ diagram,the work done is

The pressure of an ideal gas varies with volume as $P = \alpha V,$ where $\alpha$ is a constant. One mole of the gas is allowed to undergo expansion such that its volume becomes $m$ times its initial volume. The work done by the gas in the process 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 monoatomic gas is taken round the cycle $12341$ shown in the figure ($p-V$ diagram). The work done in one cycle is (in $P_0V_0$)?

In the following $p-V$ diagram, the equation of state along the curved path is given by $(V-2)^2 = 4aP$, where $a$ is a constant. The total work done in the closed path is:

An ideal gas undergoes a circular cycle centered at $4 \, atm, 4 \, L$ as shown in the diagram. The maximum temperature attained in this process is close to