question_answer

Consider the following reaction in an aqueous solution                 \[{{I}^{-}}(aq)+C{{l}^{-}}\to I{{O}^{-}}(aq)+C{{l}^{-}}(aq)\] and the following initial concentration and initial rate data for this reaction.

Exp. No	\[[{{l}^{-}}]M\]	\[[O{{C}^{-}}]M\]	Initial rate\[M{{s}^{-1}}\]
1. 2. 3. 4.	0.1000 0.2000 0.3000 0.3000	0.0500 0.0500 0.0100 0.0200	\[3.05\times {{10}^{-4}}\] \[6.10\times {{10}^{-4}}\] \[1.83\times {{10}^{-4}}\] \[3.66\times {{10}^{-4}}\]

Which of the following is the correct rate law for this reaction?

A)  Rate\[=k{{[{{l}^{-}}]}^{2}}[OC{{l}^{-}}]\]

B) Rate\[=k[OC{{l}^{-}}]\]

C) Rate\[=k{{[{{l}^{-}}]}^{2}}\]

D) Rate\[=k[{{l}^{-}}][OC{{l}^{-}}]\]