Solution Found!
The MnO2 used in alkaline batteries can be produced by an
Chapter 22, Problem 85P(choose chapter or problem)
Problem 85P
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 MnO2? At which electrode is the MnO2 formed?
Questions & Answers
QUESTION:
Problem 85P
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 MnO2? At which electrode is the MnO2 formed?
ANSWER:
Step 1 of 3
The formula to be used is shown below.
Where,
m is the mass in grams.
Q is the electric charge.
M is the molar mass. It is measured in grams per mole.
z is the valency number of ions.
F is the Faraday constant.