Consider the following reaction:Cl_{2(g)} + H | vedclass

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(D) The reaction is: $Cl_{2(g)} + H_2O \xrightarrow{R.T.} \underbrace{HCl}_{(P)} + \underbrace{HClO}_{(Q)}$.Molecular weight of $HCl$ $(P)$ is $36.5 \

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$P$ reacts with $H_2S$ gas while $Q$ does not

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(D) The reaction is: $Cl_{2(g)} + H_2O \xrightarrow{R.T.} \underbrace{HCl}_{(P)} + \underbrace{HClO}_{(Q)}$.Molecular weight of $HCl$ $(P)$ is $36.5 \ g/mol$ and $HClO$ $(Q)$ is $52.5 \ g/mol$. Since $36.5 $(A)$ $HCl$ reacts with $CrO_3$ to form chromyl chloride $(CrO_2Cl_2)$,which gives deep red vapours. This statement is correct.$(B)$ $HClO$ is an oxidizing agent and exhibits bleaching properties due to the release of nascent oxygen. This statement is correct.$(C)$ $MnO_2$ oxidizes $HCl$ to $Cl_2$ gas upon heating: $MnO_2 + 4HCl 	o MnCl_2 + Cl_2 + 2H_2O$. This statement is correct.$(D)$ $HCl$ does not react with $H_2S$,whereas $HClO$ (being an oxidizing agent) reacts with $H_2S$ to form sulfur. Thus,the statement that $P$ reacts with $H_2S$ while $Q$ does not is incorrect.

Consider the following reaction:
$Cl_{2(g)} + H_2O \xrightarrow{R.T.} P + Q$
If the molecular weight of $P$ is less than $Q$,then the incorrect statement is:

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Consider the following reaction:$Cl_{2(g)} + H_2O \xrightarrow{R.T.} P + Q$If the molecular weight of $P$ is less than $Q$,then the incorrect statement is: