A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential
MnO−4(aq) + 2H2O(l) +3e− → MnO2(s) + 4OH−(aq) E0red = +0.59V
Fe+3(aq) +e− → Fe+2(aq) E0red = +0.771V
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?