Given the Data:
Ag₂O(s) $\Delta$ H°_f = -31 $\Delta$ H°_f = 0

Given the data:
Ag₂O(s) , $\Delta$ H°_f = -31.1 kJ mol^-1, S° = +121.3 J mol^-1 K^-1
Ag(s) , $\Delta$ H°_f = 0.00 kJ mol^-1, S° = +42.55 J mol^-1 K^-1
O₂(g) , $\Delta$ H°_f = 0.00 kJ mol^-1, S° = +205.0 J mol^-1 K^-1
Calculate the temperature at which $\Delta$ G°_T = 0 for the reaction, Ag₂O(s) $\rarr$ 2 Ag(s) + ½ O₂(g) . Assume that, since the physical states do not change, $\Delta$ H° and $\Delta$ S° are independent of temperature between -50.0 °C and 950.0 °C.

A) +196 °C
B) +246 °C
C) +423 °C
D) +610 °C
E) +818 °C