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Redox Reactions

How much char...

Question

How much charge is required to reduce:
(a) $1 m o l e$ of $A l^{3 +}$ to $A l$ and
(b) $1 m o l e$ of $M n O_{4}^{-}$ to $M n^{2 +}$

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Solution

(a) The reduction reaction is:
$A l^{3 +} 1 m o l e + 3 e^{-} 3 m o l e \to A l$
Thus, $3$ mole of electrons are needed to reduce $1$ mole of $A l^{3 +}$ .
$Q = 3 \times F$
$= 3 \times 96500 = 289500 c o l u o m b$ .
(b) The reduction reaction is:
$M n O_{4}^{-} 1 m o l e + 8 H^{+} + 5 e^{-} 5 m o l e \to M n^{2 +} + 4 H_{2} O$
$Q = 5 \times F$
$= 5 \times 96500 = 482500 c o u l o m b$ .

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1 m o l

A l^{3 +}

A l

1 m o l

C u^{2 +}

C u

1 m o l

{M n O_{4}}^{-}

M n^{2 +}

1 m o l e

M n O_{4}^{-}

M n^{2 +}

How much charge is required for the following reductions :

(i) 1 mole of $A l^{3 +}$ to Al ?

(ii) 1 mole of $C u^{2 +}$ to Cu ?

(iii) 1 mole of $M n O_{4}^{-} t o M n^{2 +}$ ?

1 m o l e

H_{2} O

O_{2}

1 m o l e

F e O

F e_{2} O_{3}

How much charge is required for the following reductions:

(i) 1 mol of Al³⁺ to Al.

(ii) 1 mol of Cu²⁺to Cu.

(iii) 1 mol of to Mn²⁺.

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