The MnO2 used in alkaline batteries can be produced by an

Chapter 22, Problem 85P

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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?

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.

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