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