When KM nO 4 solution is added to oxalic acid solution- the decolourisation is slow in the beginning but becomes instantaneous after some time because-A- CO 2 is formed as the productB- MnO 4-catalyses the reactionC- M n 2- acts as an autocatalystD- The reaction is exothermic

Reduction Half: [MnO_4^ + 8H^+ + 5e^ ⟶ Mn^2+ + 4H_2O ] nbsp; ×2 Oxidation Half: [C_2O_4^2 ⟶ 2CO_2 + 2e^ ] ×5 Overall Reaction : 2MnO_4^ + 16H^+ + 5C_2O_4^ ...

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Byju's Answer

Standard XII

Chemistry

Potassium Permanganate

When KM nO 4 ...

Question

When $K M n O_{4}$ solution is added to oxalic acid solution, the decolourisation is slow in the beginning but becomes instantaneous after some time because:

C O_{2}

is formed as the product

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The reaction is exothermic

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M n O_{4}^{-}

catalyses the reaction

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M n^{2 +}

acts as an autocatalyst

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Solution

The correct option is D $M n^{2 +}$ acts as an autocatalyst
Reduction Half:
$[{M n O_{4}}^{-} + 8 H^{+} + 5 e^{-} ⟶ M n^{2 +} + 4 H_{2} O] \times 2$
Oxidation Half:
$[C_{2} O_{4}^{2 -} ⟶ 2 C O_{2} + 2 e^{-}] \times 5$
Overall Reaction :
${2 M n O_{4}}^{-} + 16 H^{+} + 5 C_{2} O_{4}^{2 -} ⟶ 2 M n^{2 +} + 10 C O_{2} + 8 H_{2} O$

End Point: Colourless to light pink.

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Similar questions

Q. When

K M n O_{4}

solution is added to oxalic acid solution, the decolourisation is slow in the beginning but becomes instantaneous after some time because:

Q. The colour of

K M n O_{4}

disappears when oxalic acid is added to its solution in an acidic medium. This can be explained as :

Q. In the titration between oxalic acid and acidified potassium permanganate, the manganous salt formed during the reaction and catalyses the reaction. The manganous salt acts as:

What is the normality of a $K M n O_{4}$ solution in which $15.8 g$ of $K M n O_{4}$ is present in $250 m L$ solution and the solution is used as an oxidant, where ${M n O_{4}}^{-}$ is reduced to ${M n}^{2 +}$ ? (Given: molar mass of $K M n O_{4} = 158 g m o l^{- 1}$ )

Q. When

K M n O_{4}

acts as an oxidising agent and ultimately forms

[M n O_{4}]^{2 -}

M n O_{2}

M n_{2} O_{3}

M n^{2 +}

, then the number of electrons transferred in each case respectively is:

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When KMnO4 solution is added to oxalic acid solution, the decolourisation is slow in the beginning but becomes instantaneous after some time because:

The correct option is D Mn2+ acts as an autocatalystReduction Half: [MnO4−+8H++5e−⟶Mn2++4H2O]×2 Oxidation Half: [C2O2−4⟶2CO2+2e−]×5 Overall Reaction : 2MnO4−+16H++5C2O2−4⟶2Mn2++10CO2+8H2O End Point: Colourless to light pink.

When $K M n O_{4}$ solution is added to oxalic acid solution, the decolourisation is slow in the beginning but becomes instantaneous after some time because: