Both mercury and silver button batteries (such as those used in many watches) operate through a redox reaction involving zinc. the balanced equation for the overall reaction in a mercury button battery is given below: (spectator ions have been omitted)
Zn(s)﹢HgO(s) → ZnO(s)﹢Hg(l)

Reduction half-reactions are as follows:
ZnO(s)﹢H₂O(l)﹢2e⁻ ⇆ Zn(s)﹢2OH⁻(aq); E⁰ = - 1.2v
HgO(s)﹢h₂O(l)﹢2e⁻ ⇆ Hg(l)﹢2OH⁻(aq); E⁰ = ﹢0.0997v

Given the reduction half-potentials supplied and knowing that ∆G⁰ = -nFE⁰ₑₗₗ; which of the statements below correctly describe this electrochemical cell? (the faraday constant f = 9.65 x 10⁴ c/mole⁻) choose one or more:

a. E⁰ₑₗₗ = -1.15v,
b. ∆G⁰ = -130kj;
c. E⁰ₑₗₗ = 1.35v,
d. ∆G⁰= 220kj;
e. ∆G⁰ = -261kj