# Problem: Calculate Eº cell for each of the following balanced redox reactions.Determine whether the reaction is spontaneous as written.a. 2Cu(s) +Mn2+(aq) → 2Cu+(aq) + Mn(s)b. MnO2(s) + 4H+(aq) + Zn(s) → Mn2+(aq) + 2H2O(l) + Zn2+(aq)c. Cl2(g) + 2F−(aq) → F2(g) + 2Cl−(aq)

###### FREE Expert Solution

$\overline{){\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cathode}}}{\mathbf{-}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{anode}}}}$

Recall:

Lose               Gain
Electron         Electrons
Oxidation       Reduction

cathode → reduction → oxidation number decreases

anode → oxidation → oxidation number increases

For ions: charge of the ion = oxidation number
For neutral atoms/compound: oxidation number = 0

Also recall:

E°cell > 0 spontaneous in the forward direction
E°cell < 0 nonspontaneous in the forward direction

91% (479 ratings) ###### Problem Details

Calculate Eº cell for each of the following balanced redox reactions.

Determine whether the reaction is spontaneous as written.

a. 2Cu(s) +Mn2+(aq) → 2Cu+(aq) + Mn(s)
b. MnO2(s) + 4H+(aq) + Zn(s) → Mn2+(aq) + 2H2O(l) + Zn2+(aq)
c. Cl2(g) + 2F(aq) → F2(g) + 2Cl(aq)