Problem: A galvanic cell is powered by the following redox reaction: Cl2(g) + Mn2+(aq) + 2 H2O(l) → 2 Cl-(aq) + MnO2(s) + 4 H+(aq). Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode Write a balanced equation for the half-reaction that takes place at the anode.Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places.

FREE Expert Solution

Cl2(g) → 2 Cl-(aq)     

Cl2 (g): O.S. = 0

Cl- (aq): O.S. = -1

change O.S. = 0 to -1

decrease/gain electrons            

reduction → cathode  

           

 Mn2+(aq) + 2 H2O(l) →  MnO2(s) + 4 H+(aq)

Mn2+ (aq): O.S. = +2

MnO2(s): O.S. = +4

change O.S. = +2 to +4

increase/lose electrons

oxidation → anode


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Problem Details

A galvanic cell is powered by the following redox reaction: Cl2(g) + Mn2+(aq) + 2 H2O(l) → 2 Cl-(aq) + MnO2(s) + 4 H+(aq). Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. 


Write a balanced equation for the half-reaction that takes place at the cathode 

Write a balanced equation for the half-reaction that takes place at the anode.


Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places.

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