Equilibrium constant from standard electrode potentials?

Calculate the equilibrium constant K for the following reaction at 25°C from standard electrode potentials. .





Sn^4+(aq) + 2Hg(l) Sn^2+(aq) + Hg2^2+(aq)

Equilibrium constant from standard electrode potentials?
Sn^4+(aq) + 2Hg(l) --%26gt; Sn^2+(aq) + Hg2^2+(aq)





Like the question states, find the ΔE of your reaction.





Then use the equation of


ΔE = (RT/nF)lnK, and solve for K, where


constant R = 8.314


T = temperature (in Kelvins)


n = number of electrons being transferred in the cell


F = 96500


ΔE = value you solved before





[Answer: see above]