Please help me with this chemistry question

1 (f) (i)
The most powerful reducing agent is the species that is most easily oxidized, which corresponds to the half-reaction with the lowest (most negative) standard reduction potential ($E^\circ$).
Comparing the $E^\circ$ values from the table:

• A: $\text{Fe}^{2+} + 2e^- \to \text{Fe}$ ($E^\circ = +0.27$ V) - Reducing agent: $\text{Fe}$
• B: $\text{NO}_3^- + 3\text{H}^+ + 2e^- \to \text{HNO}_2 + \text{H}_2\text{O}$ ($E^\circ = +0.94$ V) - Reducing agent: $\text{HNO}_2$
• C: $\text{Cl}_2 + 2e^- \to 2\text{Cl}^-$ ($E^\circ = +1.36$ V) - Reducing agent: $\text{Cl}^-$
• D: $\text{Cr}_2\text{O}_7^{2-} + 14\text{H}^+ + 6e^- \to 2\text{Cr}^{3+} + 7\text{H}_2\text{O}$ ($E^\circ = +1.33$ V) - Reducing agent: $\text{Cr}^{3+}$
• E: $\text{S}_2\text{O}_8^{2-} + 2e^- \to 2\text{SO}_4^{2-}$ ($E^\circ = +2.01$ V) - Reducing agent: $\text{SO}_4^{2-}$

The lowest $E^\circ$ value is $+0.27$ V, which corresponds to the $\text{Fe}^{2+}/\text{Fe}$ couple. Therefore, $\text{Fe}$ is the most powerful reducing agent.

The most powerful reducing agent is $\boxed