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A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential N2(g)+4H2O(l)+4e−→...

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
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.  
Do you have enough information to calculate the cell voltage under standard conditions?   Yes or No
If you said it was possible to calculate the cell voltage, do so and enter your answer here. Round your answer to 2 significant digits.



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Homework Answers

Answer #2

Reaction at cathode : reduction

Zn2+ (aq) + 2 e- Zn(s) E° = - 0.763V

Reaction at Anode : Oxidation

N2H4(aq)  + 4 OH-(aq)    N2(g)  + 4 H2O (l) + 4e- . E°oxidation = 1.16V

Net cell reaction :

N2H4(aq)  + 4 OH-(aq) + 2 Zn2+(aq)   N2(g)  + 4 H2O (l) + 2 Zn(s)

Yes , we can calculate cell voltage under standard conditions .

Ecell = 1.16V - 0.763V = 0.397 V

= 0.40 V

answered by: anonymous
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