One mole of an ideal monatomic gas undergoes a cyclic process as shown in the $P-V$ diagram. The total heat supplied to the gas is: (in $\text{ J}$)
[Note: The $P-V$ diagram is a rectangle with vertices at $(V, P)$ coordinates $(2, 100)$, $(5, 100)$, $(5, 300)$, and $(2, 300)$ where $V$ is in $\text{m}^3$ and $P$ is in $\text{N/m}^2$.]

$A$ cyclic process for $1 \, \text{mol}$ of an ideal gas is shown in the $V-T$ diagram. Find the work done in processes $AB$,$BC$,and $CA$ respectively.

The $P-V$ diagram shown below indicates two paths along which a sample of gas can be taken from state $A$ to state $B$. The energy equal to $5PV$ in the form of heat is required to be transferred if Path-$1$ is chosen. How much energy in the form of heat should be transferred if Path-$2$ is chosen?

The $p-V$ diagram for a fixed mass of an ideal gas undergoing a cyclic process is as shown in the figure. $AB$ represents an isothermal process, $BC$ represents an isobaric process, and $CA$ represents an adiabatic process. Which one of the following graphs represents the $p-T$ diagram of this cyclic process?

The pressure versus temperature $(P-T)$ graph of an ideal gas is shown in the figure.

The figure given below shows the variation in the internal energy $U$ with volume $V$ of $2.0 \text{ mole}$ of an ideal gas in a cyclic process $abcda$. The temperatures of the gas during the processes $ab$ and $cd$ are $500 \text{ K}$ and $300 \text{ K}$ respectively. The heat absorbed by the gas during the complete process is .... $J$. (Take $R = 8.3 \text{ J/mol-K}$ and $\ln 2 = 0.69$)