ELECTROCHEMISTRY Designing a galvanic cell from two half-reactions A chem signs

Question

ELECTROCHEMISTRY Designing a galvanic cell from two half-reactions A chem signs a galvanic cell that uses these two half-reactions: half-reaction N2(g)+4H2O()+4e-N2H4(aq)+40H-(aq)| Br2(l)+2e- 2Br-(aq) standard reduction potential E ed=-1.16V Ered = + 1.065 V Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written

Explanation / Answer

1) The half reaction at cathode is

Br2 + 2e -------------> 2Br- [reduction]

2) the half reaction at anode is

N2H4 + 4 OH- ------------> N2 + 4H2O + 4e [oxidation]

3) the overall cell reaction is

N2H4 + 4Oh- + 2Br2 ------------> N2 + 4H2O + 4Br-

4) Yes

5) E0 cell = SRP of cathode - SRP of anode

= +1.065V - (-1.16)V

= + 2.225 V

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