Problem: The MnO2 used in alkaline batteries can be produced by an electrochemical process of which one half-reaction isMn2+(aq) + 2H2O(l) ⟶ MnO2(s) + 4H+(aq) + 2e−If a current of 25.0 A is used, how many hours are needed to produce 1.00 kg of MnO  2? At which electrode is the MnO2 formed?

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The MnO2 used in alkaline batteries can be produced by an electrochemical process of which one half-reaction is

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

If a current of 25.0 A is used, how many hours are needed to produce 1.00 kg of MnO  2? At which electrode is the MnO2 formed?

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Our data indicates that this problem or a close variation was asked in Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition. You can also practice Chemistry: The Molecular Nature of Matter and Change - Silberberg 8th Edition practice problems.