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) $P_2{O}_3+3H_{2}O\to$	(1) $P\left(OC{H}_3\right){\mathrm{Cl}}_2$
(Q) $P_4+3\mathrm{NaOH}+3H_{2}O\to$	(2) $H_3{P}_{\mathrm{O}}{O}_3$
(R) $P_{\mathrm{Cl}}5+C{H}_3\mathrm{COOH}\to$	(3) $P_{\mathrm{H}}3$
(S) $H_3{P}_{\mathrm{O}}2+2H_{2}O+4\mathrm{AgNO}3\to$	(4) $\mathrm{POCl}3$
	(5) $H_3{P}_{\mathrm{O}}{O}_4$

The correct option is P → 2; Q → 3; R → 4; S → 5.

Let us analyze each reaction in List-I step-by-step to identify the corresponding product in List-II:

Reaction (P):

Phosphorus trioxide ($P_2{O}_3$) dissolves in cold water to form phosphorous acid ($H_3{\mathrm{PO}}_3$):

$P_2{O}_3+3H_{2}O\to 2H_3{\mathrm{PO}}_3$

Thus, (P) matches with (2).

Reaction (Q):

White phosphorus ($P_4$) reacts with sodium hydroxide solution in an inert atmosphere to produce phosphine gas (${\mathrm{PH}}_3$) and sodium hypophosphite (${\mathrm{NaH}}_2{\mathrm{PO}}_2$):

$P_4+3\mathrm{NaOH}+3H_{2}O\to {\mathrm{PH}}_3+3{\mathrm{NaH}}_2{\mathrm{PO}}_2$

Thus, (Q) matches with (3).

Reaction (R):

Phosphorus pentachloride (${\mathrm{PCl}}_5$) reacts with acetic acid (${\mathrm{CH}}_3\mathrm{COOH}$) to form acetyl chloride, phosphorus oxychloride (${\mathrm{POCl}}_3$), and hydrogen chloride gas:

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

Thus, (R) matches with (4).

Reaction (S):

Hypophosphorous acid ($H_3{\mathrm{PO}}_2$) acts as a strong reducing agent and reduces silver nitrate (${\mathrm{AgNO}}_3$) to metallic silver, while itself getting oxidized to phosphoric acid ($H_3{\mathrm{PO}}_4$):

$H_3{\mathrm{PO}}_2+2H_{2}O+4{\mathrm{AgNO}}_3\to 4\mathrm{Ag}+4{\mathrm{HNO}}_3+H_3{\mathrm{PO}}_4$

Thus, (S) matches with (5).

Combining all the correct pairs gives:
P → 2; Q → 3; R → 4; S → 5