Iodide ion is oxidized to hypoiodite ion, IO-, by hypochlorite ion, ClO-, in basic solution. The equation is I-(aq) + ClO-(aq) +OH-(aq) → IO-(aq) + Cl-(aq)The following intitial rate experiments were run and, for each, the initial rate of formation of IO- was determined. Initial Rate(mol/(L•s))Exp. 10.010 M0.020 M 0.010 M12.2x10-2Exp. 20.020 M0.010 M 0.010 M12.2x10-2Exp. 30.010 M0.010 M 0.010 M6.1x10-2Exp. 40.010 M0.010 M0.020 M3.0x10-2What is the rate law for the reaction?Input the answer in the form rate = k[A]2[B]

The given reaction : I-(aq)+ClO-(aq)+OH-(aq)→IO-(aq)+Cl-(aq)

Answered: Iodide ion is oxidized to hypoiodite…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Iodide ion is oxidized to hypoiodite ion, IO^-, by hypochlorite ion, ClO^-, in basic solution. The equation is

I^-(aq) + ClO^-(aq) +OH^-(aq) → IO^-(aq) + Cl^-(aq)

The following intitial rate experiments were run and, for each, the initial rate of formation of IO- was determined.

				Initial Rate (mol/(L•s))
Exp. 1	0.010 M	0.020 M	0.010 M	12.2x10^-2
Exp. 2	0.020 M	0.010 M	0.010 M	12.2x10^-2
Exp. 3	0.010 M	0.010 M	0.010 M	6.1x10^-2
Exp. 4	0.010 M	0.010 M	0.020 M	3.0x10^-2

What is the rate law for the reaction?

Input the answer in the form rate = k[A]2[B]

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