use the references to access important values if needed for this question.\n(1) identify each of the…

use the references to access important values if needed for this question.\n(1) identify each of the following half - reactions as either an oxidation half - reaction or a reduction half - reaction.\n\n\n(2) write a balanced equation for the overall redox reaction. use smallest possible integer coefficients.\n\n

use the references to access important values if needed for this question.\n(1) identify each of the following half - reactions as either an oxidation half - reaction or a reduction half - reaction.\n\n\n(2) write a balanced equation for the overall redox reaction. use smallest possible integer coefficients.\n\n

Answer

Explanation:

Step1: Identify half-reactions

Reduction gains electrons; oxidation loses electrons.

Step2: Balance electron transfer

Multiply reduction by 2 to match oxidation's 2 electrons.

Step3: Combine half-reactions

Add both half-reactions, cancel electrons.

Answer:

(1) First half-reaction: reduction half-reaction
Second half-reaction: oxidation half-reaction

(2)
$$2\text{Fe}^{3+}(\text{aq}) + 2\text{I}^-(\text{aq}) \rightarrow 2\text{Fe}^{2+}(\text{aq}) + \text{I}_2(\text{s})$$