The standard cell potential (E° cell) of the reaction below is +1.34 V. The value of ΔG° for the reaction is kJ/mol. 3Cu(s)+2MnO−4(aq)+8H+(aq)→3Cu2+ (aq)+2MnO2(s)+4H2O(l)

The standard cell potential (E cell) of the reaction below is +1.34 V. The value of G° for the reaction is kJ/mol.

3Cu(s)+2MnO−4(aq)+8H+(aq)→3Cu2+ (aq)+2MnO2(s)+4H2O(l)

a. -776
b. +259
c. -24.3
d. +776
e. -259

-776 KJ/mol

Explanation:

We must look towards the balanced reaction equation in order to obtain the number of electrons transferred in the redox reaction.

3Cu(s) + 2MnO4^-(aq) + 8H^+(aq)>3Cu2+(aq) + 2MnO2(s) + 4H2O(l)

We can easily see that copper lost six electrons while Manganese gained six electrons hence n=6

ΔG =-nFEcell

Where;

n= 6

F = 96500 C

Ecell=+1.34

ΔG = -(6 * 96500 * 1.34)

ΔG = -776 KJ/mol

it is the most commonly accepted one