Multiple Choice
Which of the following reactions is a redox reaction?
6. Chemical Quantities & Aqueous Reactions
Redox Reactions
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In the redox reaction Sn²⁺(aq) + 2 Fe³⁺(aq) → Sn⁴⁺(aq) + 2 Fe²⁺(aq), which substance is undergoing oxidation and which is undergoing reduction?
A
Sn²⁺ is oxidized and Fe³⁺ is reduced.
B
Sn²⁺ is reduced and Fe³⁺ is oxidized.
C
Sn⁴⁺ is oxidized and Fe²⁺ is reduced.
D
Sn⁴⁺ is reduced and Fe²⁺ is oxidized.
Verified step by step guidance1
Identify the oxidation states of each element in the reactants and products. Sn²⁺ has an oxidation state of +2, Fe³⁺ has an oxidation state of +3, Sn⁴⁺ has an oxidation state of +4, and Fe²⁺ has an oxidation state of +2.
Determine the change in oxidation states for each element. Sn²⁺ changes from +2 to +4, indicating an increase in oxidation state, while Fe³⁺ changes from +3 to +2, indicating a decrease in oxidation state.
Recall that oxidation involves an increase in oxidation state, while reduction involves a decrease in oxidation state.
Apply the definitions: Sn²⁺ is oxidized because its oxidation state increases from +2 to +4. Fe³⁺ is reduced because its oxidation state decreases from +3 to +2.
Conclude that in the given redox reaction, Sn²⁺ is the substance undergoing oxidation, and Fe³⁺ is the substance undergoing reduction.
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