Consider the following reaction.

\[{\text{Sn(s)}} + {\text{4HN}}{{\text{O}}_3}{\text{(aq)}} \to {\text{Sn}}{{\text{O}}_2}{\text{(s)}} + {\text{4N}}{{\text{O}}_2}{\text{(g)}} + {\text{2}}{{\text{H}}_2}{\text{O(g)}}\]

Which statement is correct?

A.     \({\text{HN}}{{\text{O}}_{\text{3}}}\) is the oxidizing agent because it undergoes oxidation.

B.     \({\text{HN}}{{\text{O}}_{\text{3}}}\) is the reducing agent because the oxidation number of nitrogen changes from \( + 5\) to \( + 4\).

C.     Sn is the oxidizing agent because it undergoes reduction.

D.     Sn is the reducing agent because the oxidation number of tin changes from 0 to \( + 4\).

D