On reacting $M n O_{2}$ with $H C l$ ,
1. $M n^{4 +}$ is reduced to
2. $C l^{-}$ is oxidised to

M n^{3 +}, C l^{4 +}

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M n^{2 +}, C l

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M n, C l

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M n

is not reduced nor

C l

is oxidised

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Solution

The correct option is B $M n^{2 +}, C l$
Manganese dioxide on reacting with hydrochloric acid, undergoes redox reaction. $M n O_{2}$ is the oxidising agent while $H C l$ is the reducing agent. $M n^{4 +}$ is thus reduced to $M n^{2 +}$ whereas, $C l^{-}$ is oxidised to $C l$ .

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Similar questions

$M n O_{2} + 4 H C l \to M n C l_{2} + 2 H_{2} O + C l_{2}$

In the above reaction, Mn is reduced and Cl is oxidised. The reactions in which both oxidation and reduction takes place is called __________ reaction.

Q. In alkaline medium,

C l O_{2}

oxidises

H_{2} O_{2}

O_{2}

and is itself reduced to

{C l}^{⊖}

. How many moles of

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Q. In the following reactions:
a.

3 M n O_{2} + 4 A l ⟶ 3 M n + 2 {A l}_{2} O_{3}

2 M n O_{4}^{⊖} + 16 H^{\oplus} + 10 {C l}^{⊖} ⟶ 2 {M n}^{2 +} + 5 {C l}_{2} + 8 H_{2} O

Which species is reduced and which is oxidised?

Q. State which substance is getting oxidised and reduced in the following equation:
MnO₂+ 4HCl -> MnCl₂+ 2H₂O + Cl₂

Q. Which of the following species are oxidised and reduced in the following (unbalanced) reaction?

{C N}^{-} + O {C l}^{-} ⟶ N_{2} + H {C O}_{3}^{-} + {C l}^{-}

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On reacting MnO2 with HCl, 1. Mn4+ is reduced to 2. Cl− is oxidised to

The correct option is B Mn2+,ClManganese dioxide on reacting with hydrochloric acid, undergoes redox reaction. MnO2 is the oxidising agent while HCl is the reducing agent. Mn4+ is thus reduced to Mn2+ whereas, Cl− is oxidised to Cl.

On reacting $M n O_{2}$ with $H C l$ ,
1. $M n^{4 +}$ is reduced to
2. $C l^{-}$ is oxidised to

The correct option is B $M n^{2 +}, C l$
Manganese dioxide on reacting with hydrochloric acid, undergoes redox reaction. $M n O_{2}$ is the oxidising agent while $H C l$ is the reducing agent. $M n^{4 +}$ is thus reduced to $M n^{2 +}$ whereas, $C l^{-}$ is oxidised to $C l$ .