Answer
See the detailed answer below.
Work Step by Step
$$\bf (a)$$
We need to find the temperature at point 2 by using the ideal gas law;
$$T_2=\dfrac{P_2V_2}{nR}=\dfrac{(400\times 10^3)(1000\times 10^{-6})}{(0.02)(8.31)}=\color{red}{\bf 2407}\;\rm K$$
From 1 to 2, the gas undergoes an adiabatic process. So,
$$P_1V_1^\gamma=P_2V_2^\gamma$$
Hence,
$$V_1=V_2\left[\dfrac{P_2}{P_1}\right]^\frac{1}{\gamma}$$
Since this is a diatomic gas, so $\gamma=7/5$
$$V_1=1000\left[\dfrac{400}{100}\right]^\frac{5}{7}=\bf 2692\;\rm cm^3$$
Thus,
$$T_1=\dfrac{P_1V_1}{nR}=\dfrac{(100\times 10^3)(2692\times 10^{-6})}{(0.02)(8.31)}=\color{red}{\bf 1620}\;\rm K$$
$$T_3=\dfrac{P_3V_3}{nR}=\dfrac{(400\times 10^3)(2692\times 10^{-6})}{(0.02)(8.31)}=\color{red}{\bf 6479}\;\rm K$$
$$\bf (b)$$
$\textbf{In the first process}$, which is an adiabatic one, the heat exchange is zero.
$$Q_{1\rightarrow 2}= \color{red}{\bf 0}\;\rm J $$
Thus,
$$(\Delta E_{th})_{1\rightarrow 2}=-(W_s)_{1\rightarrow 2}=\frac{5}{2}nR(T_2-T_1)$$
$$(\Delta E_{th})_{1\rightarrow 2}=\frac{5}{2}(0.02)(8.31)(2407-1620)$$
$$(\Delta E_{th})_{1\rightarrow 2}= \color{red}{\bf 327}\;\rm J $$
Anf hence,
$$(W_s)_{1\rightarrow 2}= \color{red}{\bf -327}\;\rm J $$
$\textbf{In the second process}$, which is an isobaric process,
$$(W_s)_{2\rightarrow 3}=P_2(V_3-V_2)$$
$$(W_s)_{2\rightarrow 3}=(400\times 10^3)(2692-1000)\times 10^{-6}$$
$$(W_s)_{2\rightarrow 3}= \color{red}{\bf 677}\;\rm J $$
$$(\Delta E_{th})_{2\rightarrow 3}= \frac{5}{2}nR(T_3-T_2)$$
$$(\Delta E_{th})_{2\rightarrow 3}=\frac{5}{2}(0.02)(8.31)(6479-2407)$$
$$(\Delta E_{th})_{2\rightarrow 3}=\color{red}{\bf 1692 }\;\rm J $$
$$Q_{2\rightarrow 3}= \frac{7}{2}nR(T_3-T_2)$$
$$Q_{2\rightarrow 3}=\frac{7}{2}(0.02)(8.31)(6479-2407)$$
$$Q_{2\rightarrow 3}=\color{red}{\bf 2369}\;\rm J $$
$\textbf{In the third process}$, which is an isochoric process,
$$(W_s)_{3\rightarrow 1}= \color{red}{\bf 0}\;\rm J $$
Hence,
$$(\Delta E_{th})_{3\rightarrow 1}=Q_{3\rightarrow 1}= \frac{5}{2}nR(T_1-T_3)$$
$$(\Delta E_{th})_{3\rightarrow 1}=Q_{3\rightarrow 1}=\frac{5}{2}(0.02)(8.31)(1620-6479)$$
$$(\Delta E_{th})_{3\rightarrow 1}=Q_{3\rightarrow 1}= \color{red}{\bf -2019}\;\rm J $$
See the table below.
\begin{array}{|c|c|c|c|}
\hline
& \Delta E_{th}\;{\rm (J)}& W_s\;{\rm (J)}&Q\;{\rm (J)}\\
\hline
1\rightarrow 2& 327& -327&0 \\
\hline
2\rightarrow 3& 1692 &677 &2369\\
\hline
3\rightarrow1&-2019& 0&-2019\\
\hline
{\rm Sum}& 0 & 350&Q_{in}=2369\\
\hline
\end{array}
$$\bf (c)$$
The engine’s thermal efficiency is given by
$$\eta=\dfrac{(W_s)_{total}}{Q_{in}}=\dfrac{350}{2369}$$
$$\eta=\color{red}{\bf 0.15}$$