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For the reaction: $X_2O_4(l) \rightarrow 2XO_2(g)$, $\Delta U$ = 2.1 kcal, $\Delta S$ = 20 cal $K^{-1}$ at 300 K. Hence $\Delta G$ is:
A
2.7 kcal
B
−2.7 kcal
C
9.3 kcal
D
−9.3 kcal
Detailed Solution
$X_2O_4(l) \rightarrow 2XO_2(g)$; $\Delta n_g = 2 - 0 = 2$
$\Delta H = \Delta U + \Delta n_gRT = 2.1 + 2\times\frac{2}{1000}\times300 = 3.3$ kcal
$\Delta G = \Delta H - T\Delta S = 3.3 - 300\times\frac{20}{1000} = -2.7$ kcal
$\Delta H = \Delta U + \Delta n_gRT = 2.1 + 2\times\frac{2}{1000}\times300 = 3.3$ kcal
$\Delta G = \Delta H - T\Delta S = 3.3 - 300\times\frac{20}{1000} = -2.7$ kcal