A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential

N2(g)+4H2O(l)+4e−→ N2H4(aq)+4OH−(aq) E0red = −1.16V
Zn+2(aq)+2e−→ Zn(s) E0red = −0.763V

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.