The complete balanced equation is- MnO2 - H2O2 -MnO-4 - H2O Basic medium

The correct option is A 3H_2O_2 + 2MnO_2 + 2OH^ → 2MnO^ _4 + 4H_2O The unbalanced redox equation is as follows: MnO_2 + H_2O_2 →MnO^ _4 + H_2O All ato ...

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Standard XII

Chemistry

S Block Elements

The complete ...

Question

The complete balanced equation is:
$M n O_{2} + H_{2} O_{2} \to {M n O}_{4}^{-} + H_{2} O$ (Basic medium)

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

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3 H_{2} O_{2} + M n O_{2} + 3 O H^{-} \to 2 {M n O}_{4}^{-} + 5 H_{2} O

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

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none of these

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Solution

The correct option is A $3 H_{2} O_{2} + 2 M n O_{2} + 2 O H^{-} \to 2 {M n O}_{4}^{-} + 4 H_{2} O$
The unbalanced redox equation is as follows:
$M n O_{2} + H_{2} O_{2} \to {M n O}_{4}^{-} + H_{2} O$
All atoms other than H and O are balanced.
The oxidation number of Mn changes from 4 to 7. The change in the oxidation number of Mn is 3.
The oxidation number of O changes from -1 to -2. The change in the oxidation number of one atom of O is 1. For 2 O atoms, the total change is 2.
The increase in the oxidation number is balanced with decrease in the oxidation number by multiplying $M n O_{2}$ and $M n O_{4}^{-}$ with 2
and $H_{2} O_{2}$ with $H_{2} O$ with 2.
$2 M n O_{2} + 3 H_{2} O_{2} \to 2 {M n O}_{4}^{-} + 3 H_{2} O$
O atoms are balanced by adding 1 water molecule on LHS.
$2 M n O_{2} + 3 H_{2} O_{2} + H_{2} O \to 2 {M n O}_{4}^{-} + 3 H_{2} O$
$2 M n O_{2} + 3 H_{2} O_{2} \to 2 {M n O}_{4}^{-} + 2 H_{2} O$
H atoms are balanced by adding $2 H^{+}$ on RHS.
$2 M n O_{2} + 3 H_{2} O_{2} \to 2 {M n O}_{4}^{-} + 2 H_{2} O + 2 H^{+}$
Since the reaction occurs in basic medium, add 2 hydroxide ions on both sides of the equation.
$2 M n O_{2} + 3 H_{2} O_{2} + 2 O H^{-} \to 2 {M n O}_{4}^{-} + 2 H_{2} O + 2 H^{+} + 2 O H^{-}$
On RHS, 2 $H^{+}$ ions combine with 2 $O H^{-}$ ions to form 2 water molecules.
$2 M n O_{2} + 3 H_{2} O_{2} + 2 O H^{-} \to 2 {M n O}_{4}^{-} + 4 H_{2} O$
This is the balanced chemical equation.

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Similar questions

Q. The equation

M n O_{4}^{-} (a q) + B r^{-} (a q) \to M n O_{2} (s) + B r O_{3}^{-} (a q)

when balanced in a basic medium by oxidation number method will be :

Q. Balance the following chemical equation in basic medium:

M n O_{4}^{-} (a q) + B r^{-} (a q) \to M n O_{2} (s) + B r O_{3}^{-} (a q)

Q. Balanced reaction : 2MnO

_{4}^{-}

+ I

^{-}

+ H

_{2}

\to

2MnO

_{2}

+ 2OH

^{-}

+ IO

_{3}^{- 1}

.
If true enter 1 else 0.

Q. Assertion :Bromide ion acts as a reducing agent in the recation,

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

. Reason: Oxidation number of bromine increases from

- 1

Q. Which of the following reactions are disproportionation reactions?
(I)

C u^{+} \to C u^{2 +} + C u

(II)

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

(III)

2 K M n O_{4} \to K_{2} M n O_{4} + M n O_{2} + O_{2}

(IV)

2 M n O_{4}^{-} + 3 M n^{2 +} + 2 H_{2} O \to 5 M n O_{2} + 4 H^{+}

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The complete balanced equation is:MnO2+H2O2→MnO−4+H2O (Basic medium)

The complete balanced equation is:
$M n O_{2} + H_{2} O_{2} \to {M n O}_{4}^{-} + H_{2} O$ (Basic medium)