Please help...................?

Question

Consider the galvanic cell based on the following half-reactions.

Au3+ + 3e- Au script e° = 1.50 V

Tl+ + e- Tl script e° = -0.34 V

(a) Determine the overall cell reaction. (Type your answer using the format [H3O]+ for H3O+ and [Mg]2+ for Mg2+. Use the lowest possible coefficients.

(aq) + (s) (s) + (aq)

Calculate E°cell.

(b) Calculate ΔG° and K for the cell reaction at 25°C.

(c) Calculate script ecell at 25°C when [Au3+] = 2.4e-2 M and [Tl+] = 6.8e-4 M.

Answer 1

I am sure you can figure out the reaction on your own.  The more positive E° is, the more tendency is has to reduce.  Go from there.

Then use the relationships

ΔG°(rxn) = -nFΔE, where

n = number of electrons transferred in the balanced reaction

F = 96500 J mol^(-1) = 9.65 kJ mol^(-1)

ΔE° = (RT/nF)lnK

R = 8.314 J K^(-1) mol^(-1)

T = temperature in Kelvins = 298.15

n, F same as above

For part C), use

ΔE = ΔE° - (RT/nF)lnQ, where Q = equilibrium quotient.  Solve for Q using the concentrations and your balanced equation.

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