Question

I-(aq) + OCl-(aq) IO-(aq) + Cl-(aq)
The above reaction was studied (at a particular temperature) andthe following data were obtained:

[I-]0 [OCl-]0 Initial Rate
(mol/L) (mol/L) (mol L-1 s-1)
0.120 0.160 6.30×10-2
0.030 0.080 7.87×10-3
0.240 0.080 6.30×10-2
0.060 0.160 3.15×10-2

Which of the following expressions for the rate law are completelyconsistent with the above experimental data.

d[Cl-]/dt = k[OCl-]
k[OCl-][I-] = -d[I-]/dt
-d[I-]/dt = k[I-]2[OCl-]
-d[OCl-]/dt = k[I-][OCl-]2
k[OCl-][I-] = d[Cl-]/dt

(Answer with yes/no)

----------------

I have calculated the following values
K = 3.28 L mol^-1 s^-1
k[I^-]^m[OCl^-]^n where m = 1 and n = 1

Not too sure where to go from here. Any help is much appreciated.Thanks! :)