Question

In the redox reaction 6 Fe²⁺ + Cr₂O₇²⁻ + 14 H⁺ → 2 Cr³⁺ + 6 Fe³⁺ + 7 H₂O, what is the reducing agent? A) Fe²⁺ B) Cr₂O₇²⁻ C) H⁺ D) Cr³⁺ E) Fe³⁺

Answer 1

In the given redox reaction, the reducing agent is the species that gets oxidized, meaning it loses electrons. To determine the reducing agent, we need to identify the species that undergoes an increase in oxidation state.

Let's examine the oxidation states of each element involved in the reaction:

Fe²⁺ → Fe³⁺ (oxidation state increases from +2 to +3) Cr₂O₇²⁻ → 2 Cr³⁺ (oxidation state increases from +6 to +3)

H⁺ and H₂O do not undergo any change in oxidation state, and Cr³⁺ does not change its oxidation state.

Therefore, the species that is being oxidized, and thus acting as the reducing agent, is Fe²⁺ (choice A).

So, the answer is A) Fe²⁺.