Multiple Choice
In the following reaction identify the oxidizing agent and the reducing agent:
Cr2O72- + 6 Fe2+ + 14 H+ → 2 Cr3+ + 6 Fe3+ + 7 H2O
20. Electrochemistry
Standard Reduction Potentials
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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
Verified step by step guidance1
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+).
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.
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.
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.
Confirm the answer by checking the options provided: Pb2+, Cr3+, Pb, and Cr. Based on the analysis, Pb2+ is the correct oxidizing agent.
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