How much charge is required for the following reaction?
(i) 1mol of `Al^(3+)` to Al. (ii) 1 mol of `Cu^(2+)` to Cu. (iii) 10 mole of `MnO_(4)^(-)` to `Mn^(2+)`

Explanation

To determine the amount of charge required for the given reactions, we will use Faraday's law of electrolysis, which states that the amount of charge (Q) required to transfer a certain number of moles of electrons (n) is given by the formula:

\[ Q = n \times F \]

where \( F \) is Faraday's constant, approximately \( 96500 \, C/mol \).

Now, let's solve each part of the question step by step.

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