Which of the following reactions is/are disproportionation reaction(s)?

{C l}_{2} + 2 ⊖ O H ⟶ {C l}^{⊖} + C l O^{⊖} + H_{2} O

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

2 H C u {C l}_{2} ⟶ C u + {C u}^{2 +} + 4 {C l}^{⊖} + 2 H^{\oplus}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

H C H O + ⊖ O H ⟶ C H_{3} O H + H C O O^{⊖}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

M g C O_{3} ⟶ M g O + C O_{2}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct options are
A ${C l}_{2} + 2 ⊖ O H ⟶ {C l}^{⊖} + C l O^{⊖} + H_{2} O$
B $2 H C u {C l}_{2} ⟶ C u + {C u}^{2 +} + 4 {C l}^{⊖} + 2 H^{\oplus}$
C $H C H O + ⊖ O H ⟶ C H_{3} O H + H C O O^{⊖}$
a. $2 e^{-} + {C l}_{2} ⟶ 2 {C l}^{⊖}$ (Reduction)
$2 C l O^{⊖} + 2 e^{-}$ (Oxidation)
Hence, it is a disproportionation reaction.
b. It is also a disproportionation reaction.
$[+ 1 H + 1 C u_{2}]$
$e^{-} + {C u}^{1 +} ⟶ C u$ (Reduction)
${C u}^{1 +} ⟶ {C u}^{2 +} + e^{-}$ (Oxidation)
c. It is also a disproportionation reaction.
$H C H O$ is oxidised to $H C O O^{⊖}$ and reduced to $C H_{3} O H$ .
d. It is not, sinc,e the oxidation state of $M g$ is +2 in both reactant and product. Similarly, the oxidation states of $C$ and $O$ are +4 and -2 in both reactant and product.

Suggest Corrections

Similar questions

C l_{2} + O H^{-} \to C l^{-} + C l O_{4}^{-} + H_{2} O

C r (O H)_{3} + C l O^{-} + O H^{-} \to C r O_{4}^{2 -} + C l^{-} + H_{2} O

C l_{2} + O H^{-} \to C l^{-} + C l O_{4}^{-} + H_{2} O

C l_{2} + O H^{-} \to C l^{-} + C l O^{-}_{3} + H_{2} O

C l_{2} + O H^{-} \to C l^{-} + C l O_{3}^{-} + H_{2} O

Join BYJU'S Learning Program