Identify the oxidizing agent in the following balanced reaction.
3 Pb²⁺ (aq) + 2 Cr (s) → 3 Pb (s) + 2 Cr³⁺ (aq)

• A. Pb²⁺
• B. Cr³⁺
• C. Pb
• D. Cr

Answer: (A)

Verified step by step guidance

1. Identify the oxidation states of each element in the reactants and products. In the reactants, Pb is in the +2 oxidation state (Pb²⁺) and Cr is in the 0 oxidation state (Cr). In the products, Pb is in the 0 oxidation state (Pb) and Cr is in the +3 oxidation state (Cr³⁺).
2. Determine which element is oxidized and which is reduced. Oxidation involves an increase in oxidation state, while reduction involves a decrease in oxidation state. Here, Cr goes from 0 to +3, indicating oxidation, and Pb goes from +2 to 0, indicating reduction.
3. Identify the oxidizing agent. The oxidizing agent is the substance that is reduced, meaning it gains electrons. In this reaction, Pb²⁺ is reduced to Pb, so Pb²⁺ is the oxidizing agent.
4. Review the definition of an oxidizing agent: it is a substance that causes another substance to be oxidized and is itself reduced in the process.
5. Confirm the answer by checking the options provided: Pb²⁺, Cr³⁺, Pb, and Cr. Based on the analysis, Pb²⁺ is the correct oxidizing agent.