The following reaction was carried out in water :
`Cl_(2) + 2I^(ɵ) rarr I_(2) + 2Cl^(ɵ)`
The initial concentration of `I^(ɵ)` was `0.25 mol L^(-1)` and the concentration after `10 min` was `0.23 mol L^(-1)`. Calculate the rate of disappearance of `I^(ɵ)` and rate of appearance of `I_(2)`.

Explanation

To solve the problem step by step, we will calculate the rate of disappearance of \( I^- \) and the rate of appearance of \( I_2 \) based on the given reaction and the provided concentrations.

### Step 1: Calculate the change in concentration of \( I^- \)

The initial concentration of \( I^- \) is given as \( [I^-]_{initial} = 0.25 \, \text{mol L}^{-1} \) and the concentration after 10 minutes is \( [I^-]_{final} = 0.23 \, \text{mol L}^{-1} \).

The change in concentration (\( \Delta [I^-] \)) can be calculated as:
\[
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