Using Chemical ExergyThe accompanying table shows an

Chapter 13, Problem 92P

(choose chapter or problem)

The accompanying table shows an environment consisting of a gas phase and a condensed water phase. The gas phase forms an ideal gas mixture.

(a) Show that the chemical exergy of the hydrocarbon \(\mathrm{C}_{a} \mathrm{H}_{b}\) can be determined as

\(\begin{aligned} \overline{\mathrm{e}}^{\mathrm{ch}}= & {\left[\bar{g}_{\mathrm{F}}+\left(\mathrm{a}+\frac{\mathrm{b}}{4}\right) \bar{g}_{\mathrm{O}_{2}}-\mathrm{a}_{\mathrm{CO}_{2}}\right.} \\ & \left.-\frac{\mathrm{b}}{2} \bar{g}_{\mathrm{H}_{2} \mathrm{O}(\mathrm{1})}\right]+\bar{R} T_{0} \ln \left[\frac{\left(y_{\mathrm{O}_{2}}^{\mathrm{e}}\right)^{\mathrm{a}+\mathrm{b} / 4}}{\left(y_{\mathrm{CO}_{2}}^{\mathrm{e}}\right)^{\mathrm{a}}}\right] \end{aligned}\)

(b) Using the result of part (a), repeat parts (a) through (c) of Problem 13.91.