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(A) In reaction $(i)$,the oxidation state of $S$ increases from $0$ to $+6$ in $H_2SO_4$,which is an oxidation process.In reaction $(ii)$,the oxidatio

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$(i)$ Oxidation,$(ii)$ Reduction

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(A) In reaction $(i)$,the oxidation state of $S$ increases from $0$ to $+6$ in $H_2SO_4$,which is an oxidation process.In reaction $(ii)$,the oxidation state of $K$ increases from $0$ to $+1$ (oxidation) and $Br$ decreases from $0$ to $-1$ (reduction). However,considering the overall reaction as a redox process,the formation of $KBr$ involves the oxidation of $K$ and the reduction of $Br_2$. Given the context of identifying the nature of the reaction,$(i)$ is an oxidation of $S$ and $(ii)$ is a redox reaction where $K$ is oxidized and $Br_2$ is reduced.

Identify whether the following reactions act as oxidation or reduction processes:
$(i) \ S + 6HNO_3 \to H_2SO_4 + 6NO_2 + 2H_2O$
$(ii) \ 2K + Br_2 \to 2KBr$

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Identify whether the following reactions act as oxidation or reduction processes:$(i) \ S + 6HNO_3 \to H_2SO_4 + 6NO_2 + 2H_2O$$(ii) \ 2K + Br_2 \to 2KBr$