The equilibrium constant for the reaction sr (s) + mg2 + (aq) ⇌ sr2 + (aq) + mg (s) is 2.69 * 1012 at 25°c. calculate e o for a cell made up of sr / sr2 + and mg / mg2 + half-cells.

Sr (s) + Mg² + (aq) →Sr² + (aq) + Mg (s)

Number of e-'s transfered are, n=2. Equilibrium constant,

K=2.69*10∧12

ΔG=-2.303RT logK

R=gasconstant=8.314J/mol-k

T = temperature in K = 25 oC=25+273=298K

The value we get ΔG = - 70922.3J. But ΔG = - nFE

n = number of e-'s transfered in the reaction = 2

F = farady = 96500C

E=potential of the cell is what?

∴E = ΔG. nF

= - (-70922.3) / 2*96500)

=0.367v.