Balancing Oxidation-Reduction Reactions
This worksheet focuses on balancing oxidation-reduction (redox) reactions using the half-reaction method in acidic and basic solutions.
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Balancing Oxidation-Reduction Reactions
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Read each question carefully and balance the given oxidation-reduction reactions. Show all your work for full credit.
1. Balance the following redox reaction in acidic solution:
Cr₂O₇²⁻(aq) + SO₃²⁻(aq) → Cr³⁺(aq) + SO₄²⁻(aq)
2. Balance the following redox reaction in basic solution:
MnO₄⁻(aq) + C₂O₄²⁻(aq) → MnO₂(s) + CO₃²⁻(aq)
3. In the reaction: Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)
The element that is oxidized is and the element that is reduced is .
The reducing agent is and the oxidizing agent is .
4. Which of the following statements is true regarding oxidation-reduction reactions?
Oxidation involves a gain of electrons.
Reduction involves a loss of electrons.
The oxidizing agent is reduced.
The reducing agent gains electrons.
5. In a redox reaction, the total number of electrons lost must equal the total number of electrons gained.
True
False
6. Balance the following disproportionation reaction in acidic solution:
P₄(s) → PH₃(g) + H₂PO₂⁻(aq)
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