Write the balanced chemical equation for the reaction of $Cl_{2}$ with hot and concentrated $NaOH$. Is this reaction a disproportionation reaction? Justify.
(N/A) The balanced chemical equation is: $3 Cl_{2} + 6 NaOH \rightarrow 5 NaCl + NaClO_{3} + 3 H_{2}O$
Yes,this is a disproportionation reaction because the oxidation state of chlorine changes from $0$ in $Cl_{2}$ to $-1$ in $NaCl$ and $+5$ in $NaClO_{3}$.
Yes,this is a disproportionation reaction because the oxidation state of chlorine changes from $0$ in $Cl_{2}$ to $-1$ in $NaCl$ and $+5$ in $NaClO_{3}$.
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Similar Questions
In the following reaction,assign the oxidation state for the underlined atom in the products of complete hydrolysis at $R.T.$:
$H_2\underline{S}_2O_6 + H_2O \longrightarrow H_2SO_3 + H_2SO_4$
$H_2\underline{S}_2O_6 + H_2O \longrightarrow H_2SO_3 + H_2SO_4$
Difficult
View SolutionAssign $A, B, C, D$ from the given type of reaction.
$Hg_2(NO_3)_2 + 2NH_3(aq) + H_2O \longrightarrow Hg \downarrow + Hg(NH_2)NO_3 \downarrow + NH_4NO_3$
(Note: The reaction represents the disproportionation of mercury$(I)$ nitrate with ammonia.)
$Hg_2(NO_3)_2 + 2NH_3(aq) + H_2O \longrightarrow Hg \downarrow + Hg(NH_2)NO_3 \downarrow + NH_4NO_3$
(Note: The reaction represents the disproportionation of mercury$(I)$ nitrate with ammonia.)
Medium
View SolutionWhich one of the following is an example of a disproportionation reaction?
The compound that cannot act both as an oxidising and reducing agent is:
Auto-oxidation of bleaching powder gives
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