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(B) When zinc reacts with very dilute $HNO_3$,it acts as a strong reducing agent and reduces the nitrogen in $HNO_3$ from its $+5$ oxidation state to

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$+5$ to $-3$

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(B) When zinc reacts with very dilute $HNO_3$,it acts as a strong reducing agent and reduces the nitrogen in $HNO_3$ from its $+5$ oxidation state to $-3$ in ammonium nitrate $(NH_4NO_3)$.The balanced chemical equation is:$4Zn_{(s)} + 10HNO_{3(aq)} \rightarrow 4Zn(NO_3)_{2(aq)} + NH_4NO_{3(aq)} + 3H_2O_{(l)}$In $HNO_3$,the oxidation state of $N$ is $+5$.In $NH_4NO_3$,the oxidation state of $N$ in the $NH_4^+$ ion is $-3$.

When zinc reacts with very dilute $HNO_3$,the oxidation state of nitrogen changes from

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