(Solved): Consider the reversible Carnot cycle shown in the figure below with 1.90mol of an ideal gas with ...

Consider the reversible Carnot cycle shown in the figure below with $1.90\mathrm{mol}$ of an ideal gas with $C_{\mathrm{V}}=5R/2$ as the working substance. The initial isothermal expansion occurs at the hot reservoif temperature of $T_{\text{hot }}=715\mathrm{K}$ from an initial volume of $4.55\mathrm{L}\left(V_4\right)$ to a volume of $10.5\mathrm{L}\left(V_b\right)$. The system then undergoes an adiabatic expansion until the temperature falls to $T_{\mathrm{cold}}=298\mathrm{K}$. The system then undergoes an isothermal compression and a subsequent adiabatic compression unti the initial state described by $T_{\mathrm{a}}=715\mathrm{K}$ and $V_{\mathrm{a}}=4.55\mathrm{L}$ is reached, $w$ for each step in the cycle are the following: $w_{\mathrm{a}}\to \mathrm{b}=-9450\mathrm{J}$, $w_{\mathrm{b}\to \mathrm{c}}=-1.65\times 10^4\mathrm{J},w_{\mathrm{c}\to \mathrm{d}}=3940\mathrm{J}$, and $w_{\mathrm{d}\to \mathrm{a}}=1.65\times 10^4\mathrm{J}$ Part C Calculate $q,\Delta U$, and $\Delta H$ tor the step $\mathrm{c}\to \mathrm{d}$ in the cycle. Express your answers in joules to three significant figures separated by commas. Part D Calculate $q,\Delta U$, and $\Delta H$ for the step $\mathrm{d}\to \mathrm{a}$ in the cycle. Express your answers in joules to three significant figures separated by commas.