Manganese ions Mn 2- can be oxidised by persulphate ions S 2O 82- according to the following half - equations -S 2O 82- - 2e - -2SO 42- Mn 2- - 4 H 2O -MnO 4- - 8 H - - 5e -How many moles of S 2O 82- are required to oxidise 1 mole of Mn 2-

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Electrochemical Series

Manganese ion...

Question

Manganese ions (Mn $^{2 +}$ can be oxidised by persulphate ions S $_{2}$ O $_{8}^{2 -}$ according to the following half - equations ,
S $_{2}$ O $_{8} 2 -$ + 2e $^{-}$ $\to$ 2SO $_{4}^{2 -}$
Mn $^{2 +}$ + 4 H $_{2}$ O $\to$ MnO $_{4}^{-}$ + 8 H $^{+}$ + 5e $^{-}$
How many moles of S $_{2}$ O $_{8}^{2 -}$ are required to oxidise 1 mole of Mn $^{2 +}$ ?

2.5

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0.4

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Solution

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V O_{3}^{2 -} + M n O_{4}^{-} ⟶ {M n}^{2 +} + V O_{4}^{3 -}

M n O_{4}

1

V O_{3}^{2 -}

M n (O H)_{2} (s) + M n O_{4}^{-} (a q) \to M n O_{2} (s)

M n (O H)_{2} (s) + M n O_{4}^{-} (a q) \to M n O_{2} (s)

H_{2} O_{2}

M n O_{2}

M n O_{4}^{-}

H_{2} O_{2}

M n O_{2}

$2 M n O_{4}^{-} + 5 H_{2} O_{2} + 6 H^{+} ⟶ 2 Z + 5 O_{2} + 8 H_{2} O$
In this reaction Z is

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