Chemistry help please?

Question

Under standard conditions what is the maximum electrical work in joules that the cell can accomplish if 67.0 g of Sn is consumed?

A voltaic cell is based on the reaction

Sn(s)+I2(s)—>Sn^2+(aq) + 2I^-(aq)

Answer 1

I₂ + 2e- ==> 2I^- Eº = =0.54 V ... Reduction half reaction

Sn ===> Sn²⁺ + 2e- Eº = -0.14 V ... Oxidation half reaction

____________________________

Sn(s) + I2(s) ==> Sn2+(aq) + 2I-(aq) ... overal reaction Eº = 0.54 + 0.14 = 0.68 V

Maximum work from a galvanic cell = ∆G

∆Gº = -nFEº =

where n = moles electrons transferred = 67.0 g Sn x 1 mol Sn/119 g = 0.563 moles Sn

moles of electrons = 0.563 mol Sn x 2 mol e-/mol Sn = 1.13 mol e-

F = Faraday's constant = 96,485 C/mol e-

E = cell voltage = 0.68 V = 0.68 J/C

∆Gº = -(1.13 mol e-)(96,485 C/mol e-)(0.68 J/C)

∆Gº = 74,139 J = maximum electrical work