A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential
Cl2(g) + 2e- → 2Cl- E0red = +1.359 V
MnO2(s) + 4H+ (aq) + 2e- → Mn2+(aq) + 2H2O(I) E0red = +1.23 V
a. Write a balanced equation for the half-reaction that happens at the cathode.
b. Write a balanced equation for the half-reaction that happens at the anode.
c. Write a balanced equation for the overall reaction that powers the cell.
Do you have enough information to calculate the cell voltage under standard conditions?