Answer
See the detailed answer below.
Work Step by Step
a) We can use the ideal gas law, $PV=nRT$, to find the temperatures.
Thus,
$$T_1=\dfrac{P_1V_1}{nR}=\dfrac{(400\times 10^3)(0.025)}{(2)(8.31)}=\color{red}{\bf 602}\;\rm K$$
$$T_2=\dfrac{P_2V_2}{nR}=\dfrac{(600\times 10^3)(0.050)}{(2)(8.31)}=\color{red}{\bf 1805}\;\rm K$$
$$T_3=\dfrac{P_3V_3}{nR}=\dfrac{(400\times 10^3)(0.050)}{(2)(8.31)}=\color{red}{\bf 1203}\;\rm K$$
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b)
$\textbf{In the first process,}$
We know that the work done by the system in one process is equal to the area under the curve. Hence,
$$(W_s)_{1\rightarrow2}=\text{Area under the $(P-V)$ curve}$$
$$(W_s)_{1\rightarrow2}=\frac{1}{2}(0.05-0.025)(600-400)\times 10^3+(400\times 10^3)(0.05-0.025)$$
$$(W_s)_{1\rightarrow2}=\color{blue}{\bf 12,500}\;\rm J$$
$$(\Delta E_{th})_{1\rightarrow2}=\frac{3}{2}nR(T_2-T_1)$$
$$(\Delta E_{th})_{1\rightarrow2}=\frac{3}{2}(2)(8.31)(1805-602)$$
$$(\Delta E_{th})_{1\rightarrow2}=\color{blue}{\bf 29,990}\;\rm J$$
$$Q_{1\rightarrow2}=(\Delta E_{th})_{1\rightarrow2}+(W_s)_{1\rightarrow2}=29,990+12,500 $$
$$Q_{1\rightarrow2}=\color{blue}{\bf 42,490}\;\rm J$$
$\textbf{In the second process,}$
It is an isochoric process and the volume of the gas is constant.
$$(W_s)_{2\rightarrow3}=\color{blue}{\bf 0}\;\rm J$$
$$(\Delta E_{th})_{2\rightarrow3}=\frac{3}{2}nR(T_3-T_2)$$
$$(\Delta E_{th})_{2\rightarrow3}=\frac{3}{2}(2)(8.31)(1203-1805)$$
$$(\Delta E_{th})_{2\rightarrow3}=\color{blue}{\bf -15,008}\;\rm J$$
$$Q_{2\rightarrow3}=(\Delta E_{th})_{2\rightarrow3}+(W_s)_{2\rightarrow3}=-15,008+0$$
$$Q_{2\rightarrow3}=\color{blue}{\bf -15,008}\;\rm J$$
$\textbf{In the third process,}$
It is an isobaric process:
$$(W_s)_{3\rightarrow1}=P_1\Delta V=P_1(V_1-V_3)$$
$$(W_s)_{3\rightarrow1}=(400\times 10^3) (0.025-0.050)$$
$$(W_s)_{3\rightarrow1}=\color{blue}{\bf -10,000}\;\rm J$$
$$(\Delta E_{th})_{3\rightarrow1}=\frac{3}{2}nR(T_1-T_3)$$
$$(\Delta E_{th})_{3\rightarrow1}=\frac{3}{2}(2)(8.31)(602-1203)$$
$$(\Delta E_{th})_{3\rightarrow1}=\color{blue}{\bf -14,983}\;\rm J$$
$$Q_{3\rightarrow1}=(\Delta E_{th})_{3\rightarrow1}+(W_s)_{3\rightarrow1}= -14,983-10,000$$
$$Q_{2\rightarrow3}=\color{blue}{\bf -24,983}\;\rm J$$
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& 29,990&12,500 &42,490\\
\hline
2\rightarrow 3& -15,008& 0 &-15,008\\
\hline
3\rightarrow1&-14,983& -10,000 &-24,983\\
\hline
{\rm Sum}& 0 & 2,500&Q_{in}=42,490\\
\hline
\end{array}
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c) The engine’s thermal efficiency is given by
$$\eta=\dfrac{W_{net}}{Q_{in}}=\dfrac{2,500}{42,490}$$
$$\eta=\color{red}{\bf 0.06}$$