Question

The standard reduction potentials at 298K for the following half reactions are given: \[ \text{Zn}^{2+}(aq) + 2e^- \rightarrow \text{Zn}(s) \quad E_0 = -0.762 \, \text{V} \] \[ \text{Cr}^{3+}(aq) + 3e^- \rightarrow \text{Cr}(s) \quad E_0 = -0.740 \, \text{V} \] \[ 2H^+(aq) + 2e^- \rightarrow H_2(g) \quad E_0 = 0.00 \, \text{V} \] \[ \text{Fe}^{3+}(aq) + e^- \rightarrow \text{Fe}^{2+}(aq) \quad E_0 = +0.762 \, \text{V} \] The strongest reducing agent is

• A. Zn
• B. Cr
• C. H₂
• D. Fe²⁺

Hint:

The strongest reducing agent corresponds to the most negative reduction potential.

Answer 1

The Correct Option is A

Step 1: Understanding reduction potentials.
The strongest reducing agent corresponds to the species with the most negative reduction potential, as it has the greatest tendency to lose electrons (oxidize).

Step 2: Conclusion.
Thus, the strongest reducing agent is \( \text{Zn} \), as it has the most negative reduction potential.

Final Answer: \[ \boxed{\text{(A) Zn}} \]