Chlorine undergoes disproportionation in alka | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The given reaction is a disproportionation reaction of chlorine in an alkaline medium:$Cl_2 + 2OH^- \rightarrow Cl^- + ClO^- + H_2O$Step $1$: Assi

Vedclass · Accepted Answer

$1, 2, 1$ and $1$

Vedclass · Answer

(A) The given reaction is a disproportionation reaction of chlorine in an alkaline medium:$Cl_2 + 2OH^- \rightarrow Cl^- + ClO^- + H_2O$Step $1$: Assign oxidation states.$Cl_2$ $(0)$ $\rightarrow Cl^-$ $(-1)$ and $ClO^-$ $(+1)$.Step $2$: Write half-reactions.Reduction: $Cl_2 + 2e^- \rightarrow 2Cl^-$Oxidation: $Cl_2 + 4OH^- \rightarrow 2ClO^- + 2H_2O + 2e^-$Step $3$: Add the half-reactions.$2Cl_2 + 4OH^- \rightarrow 2Cl^- + 2ClO^- + 2H_2O$Step $4$: Simplify by dividing by $2$.$Cl_2 + 2OH^- \rightarrow Cl^- + ClO^- + H_2O$Comparing with $a Cl_2 + b OH^- \rightarrow c ClO^- + d Cl^- + e H_2O$,we get $a=1, b=2, c=1, d=1$.

Chlorine undergoes disproportionation in alkaline medium as shown below:
$a Cl_{2(g)} + b OH^{-}_{(aq)} \rightarrow c ClO^{-}_{(aq)} + d Cl^{-}_{(aq)} + e H_2O_{(l)}$
The values of $a, b, c$ and $d$ in a balanced redox reaction are respectively:

Similar Questions

In alkaline medium,what will be the equivalent weight of $I_2$ on its conversion to iodate ion $(IO_3^-)$?

In acidic medium,potassium dichromate acts as an oxidant according to the equation,$Cr_2O_7^{2-} + 14H^{+} + 6e^- \to 2Cr^{3+} + 7H_2O$. What is the equivalent weight of $K_2Cr_2O_7$? (Molecular weight $= M$)

When sulphur dioxide is passed in an acidified $K_{2}Cr_{2}O_{7}$ solution,the oxidation state of sulphur is changed from

Which of the following is a redox reaction?
$(i) \, CdCl_2 + 2 KOH \longrightarrow Cd(OH)_2 + 2 KCl$
$(ii) \, BaCl_2 + K_2SO_4 \longrightarrow BaSO_4 + 2 KCl$
$(iii) \, CaCO_3 \longrightarrow CaO + CO_2$
$(iv) \, 2 Ca + O_2 \longrightarrow 2 CaO$

In acidic medium,$K_2Cr_2O_7$ shows oxidising action as represented in the half reaction:
$Cr_2O_7^{2-} + XH^+ + Ye^- \rightarrow 2A + ZH_2O$
$X, Y, Z$ and $A$ are respectively:

Vedclass Test Series

Exam Paper Generator

Online Exam Module

Chlorine undergoes disproportionation in alkaline medium as shown below:$a Cl_{2(g)} + b OH^{-}_{(aq)} \rightarrow c ClO^{-}_{(aq)} + d Cl^{-}_{(aq)} + e H_2O_{(l)}$The values of $a, b, c$ and $d$ in a balanced redox reaction are respectively: