17. (14 pts) Consider the following reaction:
2SO$_2$ (g) + O$_2$ (g) = 2SO$_3$ (g)
a) Calculate ?G°$_{rxn}$ in kJ/mol.
298.15K
K = 7.50 x 10$^{24}$ at 25°C
should be neg
$-?G°$
K = e$^{\frac{-?G°}{RT}}$ = 7.5 x 10$^{24}$
b) Predict the sign of ?H°$_{rxn}$:
(i) Positive (ii) Negative (iii) cannot be determined
c) Calculate ?G$_{rxn}$ in kJ/mol with the following conditions:
P$_{SO2}$ = 0.30 atm, P$_{O2}$ = 0.30 atm, and P$_{SO3}$ = 99 atm at 25°C.
$= \sum_p Y_p \cdot G_m(p)^i - \sum_r Y_r \cdot G_m(r)^i$
(2 mol)(99 atm) - (1 mol)(0.30 atm) - (1 mol)(0.30 atm) = 197.1 atm
d) At the conditions in part c, which direction will the reaction progress to reach equilibrium?
(i) Forward. (ii) Backward. (iii) No change. (iv) Can not be determined
