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(C) The reactions describe the chemistry of the thiosulfate ion $(S_2O_3^{2-})$.$1$. Reaction with $dil. H_2SO_4$: $Na_2S_2O_3 + H_2SO_4 	o Na_2SO_4

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Salt $'X'$ contains an anion which has an average oxidation state of $S = +2$.

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(C) The reactions describe the chemistry of the thiosulfate ion $(S_2O_3^{2-})$.$1$. Reaction with $dil. H_2SO_4$: $Na_2S_2O_3 + H_2SO_4 	o Na_2SO_4 + SO_2(g) + S(s) + H_2O(l)$. Here,gas $(B)$ is $SO_2$,neutral oxide $(C)$ is $H_2O$,and $'Y'$ is $S$.$2$. Reaction with $BaCl_2$: $Na_2S_2O_3 + BaCl_2 	o BaS_2O_3(s) + 2NaCl$. $BaS_2O_3$ is a white precipitate $('Z')$.$3$. Reaction of $SO_2$ with $H_2S$: $SO_2 + 2H_2S 	o 3S(s) + 2H_2O(l)$. This matches the given reaction where $(B)$ is $SO_2$,$(C)$ is $H_2O$,and $(Y)$ is $S$.In the thiosulfate ion $(S_2O_3^{2-})$,the average oxidation state of sulfur is calculated as: $2x + 3(-2) = -2 \implies 2x = +4 \implies x = +2$. Thus,option $C$ is correct.

Column-$I$	Column-$II$
$(P) NaBr + \text{conc. } H_2SO_4 \rightarrow$	$(A) \text{Colourless gas}$
$(Q) Na_2S + \text{dil. } HCl \rightarrow$	$(B) \text{Brown colour}$
$(R) NaNO_2 + \text{dil. } HCl \rightarrow$	$(C) \text{Rotten smell}$
$(S) NaNO_3 + \text{conc. } H_2SO_4 \rightarrow$	$(D) \text{Paramagnetic}$

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