Can you plz help me w/ this electrochem prob...im stuck

Question

Zn(s) I Zn^2 (aq) II Fe^2 (aq) I Fe(s)

at standard conditions. Calculate the value of change of G for the reaction that occurs when current is drawn from this cell

answer should be in kJ * mol^-1

i know you use this eqn right, change G degrees = -nFE

Answer 1

mind that predator.s(top contri butt or) result is in kJ*mol^-1,but he is not aware.

@predator:what.s u name?

Answer 2

Correct.

ΔG = -nFΔE

Calculate the voltage potential of your cell, assuming standard conditions.  You should find that Δ(total) = +0.31V

n = number of electrons transferred in the balanced equation = 2

F = 96500 coulombs mol^-1

1 J = 1 volt coulombs

ΔG = -(2)(96500)(+0.31) = -59830 J

You want kJ since that's what Gibb's free energy is measured in, so -59.83 kJ is your answer.

[Answer: see above]