Multiple Choice
What is the balanced equation for the redox reaction occurring in acidic solution: Au3+(aq) + Cr3+(aq) → Au(s) + Cr2O7^2-(aq)?
6. Chemical Quantities & Aqueous Reactions
Balancing Redox Reactions: Acidic Solutions
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In a galvanic cell operating in an acidic solution, which of the following represents the correct half-reaction occurring at the anode?
A
2H⁺ + 2e⁻ → H₂
B
Cu²⁺ + 2e⁻ → Cu
C
Zn → Zn²⁺ + 2e⁻
D
O₂ + 4H⁺ + 4e⁻ → 2H₂O
Verified step by step guidance1
Identify the role of the anode in a galvanic cell. The anode is where oxidation occurs, meaning it loses electrons.
Examine each given half-reaction to determine which one involves oxidation. Oxidation is characterized by the loss of electrons.
Analyze the half-reaction '2H⁺ + 2e⁻ → H₂'. This reaction involves the gain of electrons (reduction), so it cannot occur at the anode.
Consider the half-reaction 'Cu²⁺ + 2e⁻ → Cu'. This also involves the gain of electrons (reduction), so it is not the anode reaction.
Evaluate the half-reaction 'Zn → Zn²⁺ + 2e⁻'. This reaction involves the loss of electrons, indicating oxidation, which is consistent with the process occurring at the anode in a galvanic cell.
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