The following reaction was carried out in $H_{2} O$
${Cl}_{2} + 2 I^{-} \to I_{2} + 2 {Cl}^{-}$
The initial concentration of $I^{-}$ was $0.25 mol L^{-}$ and concentration after $10$ min. is $0.23 mol L^{-}$ .Calculate rate of disappearance of $I^{-}$ and appearance of $I_{2} .$

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Detailed Solution

$∆ [I^{-}] = {[I^{-}]}_{final} - {[I^{-}]}_{initial} = (0.23 - 0.25) mol L^{- 1} = - 0.02 mol L^{- 1}$

$∆ t = T_{final} - T_{initial} = 10 \min - 0 \min = 10 \min$

Rate of disappearance of $I^{-}$ is:

$- \frac{1}{2} \frac{Δ [I^{-}]}{Δt} = - \frac{1}{2} \frac{- 0.02 mol L^{- 1}}{10 \min} = 0.001 mol L^{- 1} \min^{- 1}$

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