Which of the following chemical reactions depicts the oxidizing behaviour of ${\text{H}}_2{\text{SO}}_4$?

In an oxidizing reaction, the oxidation state of the element in the oxidizing agent decreases.In ${\text{H}}_2{\text{SO}}_4$, the oxidation state of Sulphur is $+6$.In Option A: $2\text{HI}+{\text{H}}_2{\text{SO}}_4\to {\text{I}}_2+{\text{SO}}_2+2{\text{H}}_2\text{O}$ Sulphur goes from $+6$ in ${\text{H}}_2{\text{SO}}_4$ to $+4$ in ${\text{SO}}_2$ (Reduction).Iodine goes from $-1$ in $\text{HI}$ to $0$ in ${\text{I}}_2$ (Oxidation).Here, ${\text{H}}_2{\text{SO}}_4$ acts as an oxidizing agent.In B and C, it acts as an acid. In D, it is a chlorination/displacement type reaction.