Calculate the cell potential, Ecell, of a cell operating with the following reaction at 25⁰C, in which [MnO4-] = 0.010M, [Br-] = 0.010M, [Mn2+] = 0.15 M, and [H+] = 1.0 M.

2MnO4- (aq) + 10Br- (aq) + 16H+ (aq) -->  2Mn2+ (aq) + 5Br2 (l) + 8H2O (l)

use Nernst equation
E= E0cell - RT/nF ln ([ Mn2+]^2/[MnO4-]^2[Br-]^10[H+]^16
E0Cell= E0cathode + E0anode
cathode -
2MnO4- (aq)  -->  2Mn2+ (aq)

anode
10Br- (aq) ---> 5Br2 (l)