Match the reactions (in the given stoichiometry of the reactants) in List-I with one of their products given in List-II and choose the correct option.

	List-I		List-II
(P)	$$${\mathrm{P}}_2{\mathrm{O}}_3+3{\mathrm{H}}_2\mathrm{O}\to$	(1)	$\mathrm{P}\left(\mathrm{O}\right)\left({\mathrm{OCH}}_3\right){\mathrm{Cl}}_2$
(Q)	${\mathrm{P}}_4+3\mathrm{NaOH}+3{\mathrm{H}}_2\mathrm{O}\to$	(2)	${\mathrm{H}}_3{\mathrm{PO}}_3$
(R)	${\mathrm{PCl}}_5+{\mathrm{CH}}_3\mathrm{COOH}\to$	(3)	${\mathrm{PH}}_3$
(S)	${\mathrm{H}}_3{\mathrm{PO}}_2+2{\mathrm{H}}_2\mathrm{O}+4{\mathrm{AgNO}}_3\to$	(4)	${\mathrm{POCl}}_3$
		(5)	${\mathrm{H}}_3{\mathrm{PO}}_4$

 

Phosphorus trioxide reacts with water to form phosphorous acid,

${\mathrm{P}}_2{\mathrm{O}}_3+3{\mathrm{H}}_2\mathrm{O}\to 2{\mathrm{H}}_3{\mathrm{PO}}_3$

When acetic acid is heated with phosphorus pentachloride, acetyl chloride is obtained. In this reaction, $-\mathrm{COOH}$ group is converted to $-\mathrm{COCl}$ group. The side products are phosphorus oxychloride and $\mathrm{HCl}$.

${\mathrm{PCl}}_5+{\mathrm{CH}}_3\mathrm{COOH}\to {\mathrm{CH}}_3\mathrm{COCl}+{\mathrm{POCl}}_3+\mathrm{HCl}$

${\mathrm{P}}_4$ undergo disproportionation reaction with sodium hydroxide.

${\mathrm{P}}_4+3\mathrm{NaOH}+3{\mathrm{H}}_2\mathrm{O} \stackrel{}{\to }{\mathrm{PH}}_3+3{\mathrm{NaH}}_2{\mathrm{PO}}_2$

Due to the presence two $\mathrm{P}-\mathrm{H}$ bonds, ${\mathrm{H}}_3{\mathrm{PO}}_2$ acts as reducing agent. It reduces ${\mathrm{Ag}}^{+}$ to $\mathrm{Ag}$.

${\mathrm{H}}_3{\mathrm{PO}}_2+{\mathrm{H}}_2\mathrm{O}+{\mathrm{AgNO}}_3\to {\mathrm{H}}_3{\mathrm{PO}}_4+{\mathrm{HNO}}_3+\mathrm{Ag}\downarrow$