Multiple Choice
Which of the following is the correctly balanced redox reaction for Cr2O7^2-(aq) + I^-(aq) → Cr^3+(aq) + IO3^-(aq) in acidic solution?
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6. Chemical Quantities & Aqueous Reactions
Balancing Redox Reactions: Acidic Solutions
Multiple Choice
Which of the following is the balanced redox reaction for IO3⁻(aq) + H2SO3(aq) → I2(aq) + SO4²⁻(aq) in an acidic solution?
A
2 IO3⁻(aq) + 5 H2SO3(aq) + 2 H⁺(aq) → I2(aq) + 5 SO4²⁻(aq) + 4 H2O(l)
B
2 IO3⁻(aq) + 3 H2SO3(aq) + 6 H⁺(aq) → I2(aq) + 3 SO4²⁻(aq) + 6 H2O(l)
C
IO3⁻(aq) + H2SO3(aq) + H⁺(aq) → I2(aq) + SO4²⁻(aq) + H2O(l)
D
IO3⁻(aq) + 3 H2SO3(aq) → I2(aq) + 3 SO4²⁻(aq) + 3 H⁺(aq)
Verified step by step guidance1
Identify the oxidation and reduction half-reactions. IO3⁻ is reduced to I2, and H2SO3 is oxidized to SO4²⁻.
Write the reduction half-reaction: IO3⁻ → I2. Balance iodine atoms first, then add electrons to balance the charge.
Write the oxidation half-reaction: H2SO3 → SO4²⁻. Balance sulfur atoms first, then add electrons to balance the charge.
Balance oxygen atoms by adding H2O molecules to the side that needs oxygen. Then balance hydrogen atoms by adding H⁺ ions.
Combine the balanced half-reactions, ensuring that the number of electrons lost in oxidation equals the number gained in reduction. Adjust coefficients to achieve this balance.
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