Identify the type of the following redox reac | vedclass

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(A) Step $1$: Assign oxidation states to the chlorine atoms in the reaction.In $Cl_2$, the oxidation state of $Cl$ is $0$.In $NaCl$, the oxidation sta

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Disproportionation reaction

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(A) Step $1$: Assign oxidation states to the chlorine atoms in the reaction.In $Cl_2$, the oxidation state of $Cl$ is $0$.In $NaCl$, the oxidation state of $Cl$ is $-1$.In $NaOCl$, the oxidation state of $Cl$ is $+1$.Step $2$: Observe the change in oxidation states.The oxidation state of $Cl$ decreases from $0$ to $-1$ (reduction) and increases from $0$ to $+1$ (oxidation).Step $3$: Conclusion.Since the same element $(Cl)$ is simultaneously oxidized and reduced, this is a disproportionation reaction.Therefore, the correct option is $A$.

Identify the type of the following redox reaction:
$Cl_2 + 2NaOH \longrightarrow NaCl + NaOCl + H_2O$

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Identify the type of the following redox reaction:$Cl_2 + 2NaOH \longrightarrow NaCl + NaOCl + H_2O$

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Identify the type of the following redox reaction:
$Cl_2 + 2NaOH \longrightarrow NaCl + NaOCl + H_2O$