$1 \mathrm{mole}$ of an ideal gas, $\left[\mathrm{\gamma }=\text{1.5}\right]$, are taken through a series of processes.

Information-I The temperature at state '$\mathrm{A}$' is $300 \mathrm{K}$.

Information-II The reversible isothermal expansion from $\mathrm{B} \mathrm{to} \mathrm{C}$ doubles the volume.

Information-III The entropy change of the system from $\mathrm{C} \mathrm{to} \mathrm{D}$ is $4\ln 16 \mathrm{cal} {\mathrm{K}}^{-1}$.

Select the correct option(s) using the above information.

The combination of plots which does not represent isothermal expansion of an ideal gas is

$\left(\mathrm{A}\right)$

$\left(\mathrm{B}\right)$

$\left(\mathrm{C}\right)$

$\left(\mathrm{D}\right)$

One mole of an ideal monoatomic gas is subjected to changes as shown in the graph. The magnitude of the work done (by the system or on the system) is _______ J (nearest integer)

Given : log 2 = 0.3, ln 10 = 2.3

A certain mass of a gas was brought from state $\mathrm{A}$ to $\mathrm{B}$ by following three different paths, namely $1,2$ and $3$, respectively. Which of the following relations is correct for the work done?

($\mathrm{p}$: pressure, $\mathrm{V}$: volume, $\mathrm{T}$: temperature, $\mathrm{H}$: enthalpy, $\mathrm{S}$: entropy)

$$\begin{gathered} \mathrm{State} 1 \leftrightarrows \mathrm{State} 2 \leftrightarrows \mathrm{State} 3 \\ \left(\begin{array}{c}\mathrm{T}=300\mathrm{K}\\ \mathrm{P}=15\mathrm{bar}\\ 1\mathrm{mole} \end{array}\right)\left(\begin{array}{c}\mathrm{T}=300\mathrm{K}\\ \mathrm{P}=10\mathrm{bar}\\ 1\mathrm{mole} \end{array}\right) \left(\begin{array}{c}\mathrm{T}=300\mathrm{K}\\ \mathrm{P}=5\mathrm{bar}\\ 1 \mathrm{mole} \end{array}\right) \end{gathered}$$

Above shows a cyclic process. Calculate the total work done during one complete cycle.
(Assume a single step to reach the next state).