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Oxidation Number Method

Balance the f...

Question

Balance the following redox reaction in basic medium:
${M n}^{2 +} + C l O_{3}^{-} ⟶ M n O_{2} + C l O_{2}$

A

{M n}^{2 +} + 2 C l O_{3}^{-} ⟶ M n O_{2} + 2 C l O_{2}

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B

{M n}^{2 +} + 3 C l O_{3}^{-} ⟶ M n O_{2} + 3 C l O_{2}

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C

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

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D

None of these

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Solution

The correct option is A ${M n}^{2 +} + 2 C l O_{3}^{-} ⟶ M n O_{2} + 2 C l O_{2}$
The unbalanced redox equation is as follows:
${M n}^{2 +} + C l O_{3}^{-} ⟶ M n O_{2} + C l O_{2}$
All atoms other than H and O are balanced.
The oxidation number of Mn changes from 2 to 4. The change in the oxidation number is 2.
The oxidation number of Cl changes from 5 to 4. The change in he oxidation number is 1.
To balance the increase in the oxidation number with decrease in the oxidation number multiply $C l O_{3}^{-}$ and $C l O_{2}$ with 2.

${M n}^{2 +} + 2 C l O_{3}^{-} ⟶ M n O_{2} + 2 C l O_{2}$
This is the balanced chemical equation.

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Similar questions

Write balanced redox reactions of the following.

H_{2} O_{2} (a q)

{M n}^{2 +} (a q)

M n O_{2}

in basic medium.

Q. The following two redox reactions are given:
i)

M n O_{4}^{-} + 8 H^{+} + 5 e^{-} \to M n^{2 +} + 4 H_{2} O; E^{o} = X_{1} V

M n O_{2} + 4 H^{+} + 2 e^{-} \to M n^{2 +} + 2 H_{2} O; E^{o} = X_{2} V

E^{o}

for the following reaction.

M n O_{4}^{-} + 4 H^{+} + 3 e^{-} \to M n O_{2} + 2 H_{2} O

Q. Calculate the value of

E_{M n O_{4}^{-} | M n O_{2}}^{\circ}

M n O_{4}^{-} + 8 H^{+} + 5 e^{-} \to M n^{2 +} + 4 H_{2} O

E^{\circ} = 1.51 V

M n O_{2} + 4 H^{+} + 2 e^{-} \to M n^{2 +} + 2 H_{2} O

E^{\circ} = 1.23 V

E^{\circ}

for the half cells :

M n O_{2} + 4 H^{+} + 2 e^{-} \to M n^{2 +} + 2 H_{2} O i s 1.23 V F e^{3 +} + e^{-} \to F e^{2 +} i s 0.77 V

Which of the following statements is true?

Q. Given the standard potential of the following at

25^{\circ} C

M n O_{2} \to M n^{3 +}

E^{⊖} = 0.95 V

M n^{3 +} \to M n^{2 +}

E^{⊖} = 1.51 V

The standard potential of

M n O_{2} \to M n^{2 +}

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