Question

In the redox reaction Cr₂O²⁻₇(aq)+I⁻(aq)→Cr³⁺(aq)+I₂(s), what is the balanced oxidation reaction (before the half reactions are added together)?

a) Cr₂O²⁻₇→Cr³⁺
b) I⁻→I₂
c) Cr₂O²⁻₇→Cr³⁺+3e⁻
d) I⁻→I₂+2e⁻

Answer 1

The balanced oxidation reaction for the redox reaction is d) I⁻→I₂+2e⁻. In the half-reaction, the iodide ion (I⁻) is oxidized to form molecular iodine (I₂) and release two electrons. This is consistent with the overall redox reaction where Cr₂O²⁻₇ is reduced to Cr³⁺.

Step-by-step explanation:

The balanced oxidation reaction for the given redox reaction is d) I⁻→I₂+2e⁻. In the half-reaction, the iodide ion (I⁻) is oxidized to form molecular iodine (I₂) and release two electrons. This is consistent with the overall redox reaction where Cr₂O²⁻₇ is reduced to Cr³⁺.

balanced oxidation reaction for the redox reaction is d) I⁻→I₂+2e⁻. In the half-reaction, the iodide ion (I⁻) is oxidized to form molecular iodine (I₂) and release two electrons. This is consistent with the overall redox reaction where Cr₂O²⁻₇ is reduced to Cr³⁺.