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When 0.1 mol MnO $_4^{2-}$ is oxidized, the quantity of electricity required to completely convert MnO $_4^{2-}$ to MnO $_4^-$ is

medium

Electrochemistry

2014

chemistry

96,500 C

2 × 96,500 C

9,650 C

96.50 C

Explanation

To solve this problem, we need to determine the quantity of electricity required to oxidize MnO $_4^{2-}$ to MnO $_4^{-}. \\$

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The oxidation reaction can be represented as:

\\

MnO

_4^{2-} \rightarrow

MnO

_4^{-} + e^- \\

This reaction shows that one mole of

MnO

_4^{2-}

releases one mole of electrons.

\\

Given:

\\

• Amount of

MnO

_4^{2-} = 0.1

mol

\\

Since 1 mole of

MnO

_4^{2-}

releases 1 mole of electrons,

\\

0.1 mol of

MnO

_4^{2-}

will release 0.1 mol of electrons.

\\

The charge of 1 mole of electrons (Faraday's constant) is

96,500

C/mol.

\\

Therefore, the total charge required is:

\\

Charge

= 0.1

mol

\times 96,500

C/mol

\\

Charge

= 9,650

C

\\

Thus, the quantity of electricity required is

9,650

C, which corresponds to Option 3.

\\