Cl2(g) → 2 Cl-(aq)
Cl2 (g): O.S. = 0
Cl- (aq): O.S. = -1
change O.S. = 0 to -1
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
oxidation → anode
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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