Problem: Consider the reaction: I2(s) + 2 Br–(aq) → 2 I–(aq) + Br2(l); ΔG˚ = 1.1 x 105 J. The calculation revealed that the reaction is not spontaneous. Based on conceptual reasoning, which of the following best explains why I2 does not oxidize Br–?(a) Br is more electronegative than I; therefore, you do not expect Br– to give up an electron to I2.(b) I is more electronegative than Br; therefore, you do not expect I2 to give up an electron to Br–.(c) Br– is in solution and I2 is a solid. Solids do not gain electrons from substances in solution.

FREE Expert Solution

We’re being asked to choose the best explanation why I2 does not oxidize Br.

Let's analyze each option given.

For Option (a) and (b):

(a) Br is more electronegative than I; therefore, you do not expect Br to give up an electron to I2.

(b) I is more electronegative than Br; therefore, you do not expect I2 to give up an electron to Br.

The electronegativity trend is:

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Problem Details

Consider the reaction: I2(s) + 2 Br(aq) → 2 I(aq) + Br2(l); ΔG˚ = 1.1 x 105 J. The calculation revealed that the reaction is not spontaneous. Based on conceptual reasoning, which of the following best explains why I2 does not oxidize Br?

(a) Br is more electronegative than I; therefore, you do not expect Br to give up an electron to I2.

(b) I is more electronegative than Br; therefore, you do not expect I2 to give up an electron to Br.

(c) Br is in solution and I2 is a solid. Solids do not gain electrons from substances in solution.

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