Which of the following reactions is not a red | vedclass

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(C) redox reaction is one in which both oxidation and reduction occur simultaneously,involving a change in the oxidation states of the elements involv

Vedclass · Accepted Answer

$Na_2O + H_2SO_4 \longrightarrow Na_2SO_4 + H_2O$

Vedclass · Answer

(C) redox reaction is one in which both oxidation and reduction occur simultaneously,involving a change in the oxidation states of the elements involved.In option $A$,$S$ in $SO_2$ is $+4$ and in $H_2S$ is $-2$,changing to $0$ in $S$. This is a redox reaction.In option $B$,$Cl$ in $KClO_3$ is $+5$,changing to $+7$ in $KClO_4$ and $-1$ in $KCl$. This is a disproportionation redox reaction.In option $C$,$Na_2O + H_2SO_4 \longrightarrow Na_2SO_4 + H_2O$,the oxidation states are: $Na(+1)$,$O(-2)$,$H(+1)$,$S(+6)$. These remain unchanged in the products. This is a neutralization reaction,not a redox reaction.In option $D$,$Na$ changes from $0$ to $+1$ and $O$ changes from $0$ to $-1$. This is a redox reaction.

Column $I$	Column $II$
$A$. $O_2^{-} \rightarrow O_2 + O_2^{2-}$	$p$. redox reaction
$B$. $CrO_4^{2-} + H^{+} \rightarrow$	$q$. one of the products has trigonal planar structure
$C$. $MnO_4^{-} + NO_2^{-} + H^{+} \rightarrow$	$r$. dimeric bridged tetrahedral metal ion
$D$. $NO_3^{-} + H_2SO_4 + Fe^{2+} \rightarrow$	$s$. disproportionation

Which of the following reactions is not a redox reaction?

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