(C) In the reaction $4 KClO_3 \longrightarrow 3 KClO_4 + KCl$,the oxidation state of chlorine in $KClO_3$ is $+5$. In $KClO_4$,the oxidation state of

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$4 KClO_3 \longrightarrow 3 KClO_4 + KCl$

(C) In the reaction $4 KClO_3 \longrightarrow 3 KClO_4 + KCl$,the oxidation state of chlorine in $KClO_3$ is $+5$. In $KClO_4$,the oxidation state of chlorine is $+7$ (oxidation). In $KCl$,the oxidation state of chlorine is $-1$ (reduction). Since the same element (chlorine) is simultaneously oxidized and reduced,this is a disproportionation reaction. Hence,the correct option is $(C)$.

Class 11 Chemistry Redox Reactions Auto oxidation and Disproportionation

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Which of the following represents the disproportionation of potassium chlorate?

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A
$2 KClO_3 \longrightarrow 2 KCl + 3 O_2$
B
$3 KClO_3 \longrightarrow 2 KClO_2 + KClO_4$
C
$4 KClO_3 \longrightarrow 3 KClO_4 + KCl$
D
None of the above

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Redox Reactions

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Auto oxidation and Disproportionation

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Total number of species from the following which can undergo disproportionation reaction . . . . . . .
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Which of the following represents the disproportionation of potassium chlorate?

Similar Questions

Which of the following ionic or molecular species does not disproportionate in water at room temperature?

The reaction that takes place when $Cl_2$ gas is passed through concentrated $NaOH$ solution is:

Assign $A$,$B$,$C$,$D$ from the given type of reaction.$Ca(OH)_2 + Cl_2 \longrightarrow CaOCl_2 + H_2O$

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Total number of species from the following which can undergo disproportionation reaction . . . . . . .$H_2O_2$,$ClO_3^{-}$,$P_4$,$Cl_2$,$Ag$,$Cu^{+}$,$F_2$,$NO_2$,$K^{+}$

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Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$Ca(OH)_2 + Cl_2 \longrightarrow CaOCl_2 + H_2O$

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$H_2O_2 \xrightarrow{R.T} H_2O + \frac{1}{2} O_2$

Total number of species from the following which can undergo disproportionation reaction . . . . . . .
$H_2O_2$,$ClO_3^{-}$,$P_4$,$Cl_2$,$Ag$,$Cu^{+}$,$F_2$,$NO_2$,$K^{+}$