JEE MAIN - Chemistry (2024 - 5th April Morning Shift - No. 18)
The reaction at cathode in the cells commonly used in clocks involves.
oxidation of $$\mathrm{Mn}$$ from +2 to +7
reduction of $$\mathrm{Mn}$$ from +4 to +3
oxidation of $$\mathrm{Mn}$$ from +3 to +4
reduction of $$\mathrm{Mn}$$ from +7 to +2
Explanation
In the cells commonly used in clocks, specifically alkaline batteries, the reaction at the cathode involves the reduction of manganese dioxide (MnO2). The manganese in MnO2 is initially in the +4 oxidation state, and it gets reduced to the +3 oxidation state. Thus, the correct reaction occurring at the cathode can be represented as follows:
The correct answer is:
Option B
reduction of $$\mathrm{Mn}$$ from +4 to +3
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