Manganese dioxide (MnO₂) for use in dry cells is made by electrolyzing solutions of Mn²⁺, where the following reaction occurs at the anode:
Mn²⁺(aq) + 2H₂O(l) $\to$ MnO₂(s) + 4H⁺(aq) + 2e^-
Using a current of 100. amperes (A), how many hours will it take to produce 5.00 kg of MnO₂, according to the above reaction?

Question

Manganese dioxide (MnO₂) for use in dry cells is made by electrolyzing solutions of Mn²⁺, where the following reaction occurs at the anode:
Mn²⁺(aq) + 2H₂O(l)

\to

MnO₂(s) + 4H⁺(aq) + 2e^-
Using a current of 100. amperes (A), how many hours will it take to produce 5.00 kg of MnO₂, according to the above reaction?

Quizplus · Accepted Answer

The Answer of Manganese dioxide (MnO₂) for use in dry cells is made by electrolyzing solutions of Mn²⁺, where the following reaction occurs at the anode: Mn²⁺(aq) + 2H₂O(l) $\to$ MnO₂(s) + 4H⁺(aq) + 2e^- Using a current of 100. amperes (A), how many hours will it take to produce 5.00 kg of MnO₂, according to the above reaction?

Manganese Dioxide (MnO2) for Use in Dry Cells Is Made →\to→

Manganese Dioxide (MnO₂) for Use in Dry Cells Is Made $\to$