Thermodynamics question. Please show work:
ΔfHo(HCl) = -100 kJ mol^-1
ΔfSo(HCl) = 200 J mol^-1 K^-1
ΔfSo(Cl2) = 200 J mol^-1 K^-1
ΔfSo(H2) = 100 J mol^-1 K^-1
Given the above standard molar enthalpies and entropies of formation at 300K and 1 bar, what is the standard molar Gibbs free energy of reaction for the below process with all species as gases at 300 K and 1 bar?
(1/2) Cl2 + (1/2) H2 --> HCl
(a) -138 kJ mol^-1
(b) -126 kJ mol^-1
(c) -115 kJ mol^-1
(d) 0 kJ mol^-1
(e) 64 kJ mol^-1
(f) 104 kJ mol^-1