Assuming That, Since the Physical States Do Not Change, the Values

Assuming that, since the physical states do not change, the values of $\Delta$ H and $\Delta$ S do not change as we raise the temperature, and using,
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 a value for the free energy change, $\Delta$ G°_T for the reaction below, at 500 °C N₂(g) + 3 H₂(g) $\rarr$ 2 NH₃(g)

A) +7.2 kJ mol^-1
B) +245.3 kJ mol^-1
C) +99.1 kJ mol^-1
D) +61.3 kJ mol^-1
E) +153.2 kJ mol^-1