Consider the following reaction in an aqueous solution {\I}^{-}(\aq)+ {\Cl}^{-} \to{\IO}^{-}(\aq)+ {\Cl}^{-}(\aq) and the following initial concentration and initial rate data for this reaction. Exp. No [\I^{-} ] {\M} [\OCl^{-} ] {\M} Initial rate \Ms^{-1} 1. 0.1000 0.0500 3.05\times 10^{-4} 2. 0.2000 0.0500 6.10\times 10^{-4} 3. 0.3000 0.0100 1.83\times 10^{-4} 4. 0.3000 0.0200 3.66\times 10^{-4} Which of the following is the correct rate lawfor this reaction?

Correct Answer is : Rate =k[I−][OCl−]

Rate = \k [\I^{-} ]^ 2[\OCl^{-} ]

Manipal Entrance Test 2013 Chemistry Paper

Question : 55 of 60

Marks: +1, -0

Consider the following reaction in an aqueous solution
I−(aq)+Cl−→IO−(aq)+Cl−(aq)
and the following initial concentration and initial rate data for this reaction.

Exp. No	[I−]M	[OCl−]M	Initial rate Ms−1
1.	0.1000	0.0500	3.05×10−4
2.	0.2000	0.0500	6.10×10−4
3.	0.3000	0.0100	1.83×10−4
4.	0.3000	0.0200	3.66×10−4

Which of the following is the correct rate lawfor this reaction?

Rate =k[I−]2[OCl−]
Rate =k[OCl−]
Rate =k[I−]2
Rate =k[I−][OCl−]

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