Assign A, B, C, D from the given type of reac | vedclass

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(D) In the reaction $P_4   10Cl_2 \xrightarrow{\Delta} 4PCl_5$,the oxidation state of $P$ changes from $0$ to $ 5$ and $Cl$ changes from $0$ to $-1$.T

Vedclass · Accepted Answer

Both $(B)$ and $(C)$

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(D) In the reaction $P_4   10Cl_2 \xrightarrow{\Delta} 4PCl_5$,the oxidation state of $P$ changes from $0$ to $ 5$ and $Cl$ changes from $0$ to $-1$.This is a combination reaction where two elements combine to form a single compound,which is a redox reaction.Since heat $(\Delta)$ is involved,it is a thermal combination redox reaction.Additionally,it is an intermolecular redox reaction because the oxidation and reduction occur in different species ($P_4$ and $Cl_2$ respectively).Therefore,the reaction fits both categories described in $(B)$ and $(C)$.

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

Assign $A, B, C, D$ from the given type of reaction.
$P_4 + 10Cl_2 \xrightarrow{\Delta} PCl_5$

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Assign $A, B, C, D$ from the given type of reaction.$P_4 + 10Cl_2 \xrightarrow{\Delta} PCl_5$