$\mathrm{COP}=\frac{\mathrm{T}_{\mathrm{L}}}{\mathrm{T}_{\mathrm{H}}-\mathrm{T}_{\mathrm{L}}}$
Where $\mathrm{T}_{\mathrm{L}} \rightarrow$ lower Temperature
$\mathrm{\&} \quad \mathrm{T}_{\mathrm{H}} \rightarrow$ Higher Temperature
So, $5=\frac{T_{L}}{T_{H}-T_{L}}$
$\Rightarrow \mathrm{T}_{\mathrm{H}}=\frac{6}{5} \mathrm{T}_{\mathrm{L}}=\frac{6}{5}(253)=303.6 \mathrm{K}$
Step $1$ It is first compressed adiabatically from volume $V_{1}$ to $1 \;m ^{3}$.
Step $2$ Then expanded isothermally to volume $10 \;m ^{3}$.
Step $3$ Then expanded adiabatically to volume $V _{3}$.
Step $4$ Then compressed isothermally to volume $V_{1}$. If the efficiency of the above cycle is $3 / 4$, then $V_{1}$ is ............ $m^3$
[ $R$ is the gas constant]
$(1)$ Work done in this thermodynamic cycle $(1 \rightarrow 2 \rightarrow 3 \rightarrow 4 \rightarrow 1)$ is $| W |=\frac{1}{2} RT _0$
$(2)$ The ratio of heat transfer during processes $1 \rightarrow 2$ and $2 \rightarrow 3$ is $\left|\frac{ Q _{1 \rightarrow 2}}{ Q _{2 \rightarrow 3}}\right|=\frac{5}{3}$
$(3)$ The above thermodynamic cycle exhibits only isochoric and adiabatic processes.
$(4)$ The ratio of heat transfer during processes $1 \rightarrow 2$ and $3 \rightarrow 4$ is $\left|\frac{Q_{U \rightarrow 2}}{Q_{3 \rightarrow 4}}\right|=\frac{1}{2}$

Match the quantities mentioned in $List-I$ with their values in $List-II$ and choose the correct option. [ $R$ is the gas constant]
| $List-I$ | $List-II$ |
| ($P$) Work done in the complete cyclic process | ($1$) $R T_0-4 \ R T_0 \ln 2$ |
| ($Q$) Change in the internal energy of the gas in the process $JK$ | ($2$) $0$ |
| ($R$) Heat given to the gas in the process $KL$ | ($3$) $3 \ R T_0$ |
| ($S$) Change in the internal energy of the gas in the process $MJ$ | ($4$) $-2 \ R T_0 \ln 2$ |
| ($5$) $-3 \ R T_0 \ln 2$ |
