The $P-V$ diagram of $2\,g$ of helium gas for a certain process $A \to B$ is shown in the figure. What is the heat given to the gas during the process $A \to B$ (in $,P_0V_0$)?

In the cyclic process shown on the $P-V$ diagram,the magnitude of the work done is

One mole of an ideal gas in initial state $A$ undergoes a cyclic process $ABCA$,as shown in the figure. Its pressure at $A$ is $P_0$. Choose the correct option$(s)$ from the following:
$(A)$ Internal energies at $A$ and $B$ are the same
$(B)$ Work done by the gas in process $AB$ is $P_0 V_0 \ln 4$
$(C)$ Pressure at $C$ is $\frac{P_0}{4}$
$(D)$ Temperature at $C$ is $\frac{T_0}{4}$

$A$ thermodynamic process is shown in the figure. The pressure and volume at the points shown in the figure are as follows:
$P_A = 3 \times 10^{4} \text{ Pa}, V_A = 2 \times 10^{-3} \text{ m}^3, P_B = 8 \times 10^{4} \text{ Pa}, V_D = 5 \times 10^{-3} \text{ m}^3.$
In process $AB$, $600 \text{ J}$ of heat is added to the system, and in process $BC$, $200 \text{ J}$ of heat is added. The change in internal energy during the process $AC$ is: (in $\text{ J}$)

The net work done by an ideal gas going through the cycle as shown in the $P-V$ diagram below is

An ideal gas is made to undergo the cyclic process shown in the figure below. Let $\Delta W$ depict the work done,$\Delta U$ be the change in internal energy of the gas,and $Q$ be the heat added to the gas. The signs of each of these three quantities for the whole cycle will be ($0$ refers to no change):