Given the Data:
N₂(g) $\Delta$ H°_f = 0 $\Delta$ H°_f = 0 $\Delta$

Given the data:
N₂(g) , $\Delta$ H°_f = 0.00 kJ mol^-1, S° = +191.5 J mol^-1 K^-1
H₂(g) , $\Delta$ H°_f = 0.00 kJ mol^-1, S° = +130.6 J mol^-1 K^-1
NH₃(g) , $\Delta$ H°_f = -46.0 kJ mol^-1, S° = +192.5 J mol^-1 K^-1
Calculate the standard free energy change, $\Delta$ G° for the reaction:N₂(g) + 3 H₂(g) $\rarr$ 2 NH₃(g)

A) -7.4 kJ mol^-1
B) -32.9 kJ mol^-1
C) -84.6 kJ mol^-1
D) +112.3 kJ mol^-1
E) +32.9 kJ mol^-1