Multiple Choice
Which of the following reactions is a redox reaction?
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6. Chemical Quantities & Aqueous Reactions
Redox Reactions
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In the disproportionation reaction Cl2(g) → Cl−(aq) + ClO−(aq), which element undergoes both oxidation and reduction?
A
Sodium
B
Hydrogen
C
Oxygen
D
Chlorine
Verified step by step guidance1
Identify the species involved in the reaction: Cl2(g) is converted into Cl⁻(aq) and ClO⁻(aq).
Determine the oxidation states of chlorine in each species: In Cl2, chlorine has an oxidation state of 0; in Cl⁻, chlorine has an oxidation state of -1; in ClO⁻, chlorine has an oxidation state of +1.
Recognize that in a disproportionation reaction, the same element is both oxidized and reduced simultaneously.
Observe that chlorine goes from 0 in Cl2 to -1 in Cl⁻ (reduction) and from 0 in Cl2 to +1 in ClO⁻ (oxidation).
Conclude that chlorine is the element undergoing both oxidation and reduction in this reaction.
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