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The reaction I- (aq) + OCl- (aq) → IO- (aq) + Cl- (aq) was studied, and the following data were obrained: [I-]0(mol/L) [OCl-]0(mol/L) Initial Rate (mol/L ·s) 0.12 0.18 7.91x 10-2 0.060 0.18 3.95 x 10-2 0.030 0.090 9.88 x 10-3 0.24 0.090 7.91x 10-2 a. What is the rate law? b. Calculate the value of the rate constant. c. Calculate the initial rate for an experiment where both I- and OCl- are initially present at 0.15 mol/L.

The reaction I- (aq) + OCl- (aq) → IO- (aq) + Cl- (aq) was studied, and the following data were obrained: [I-]0(mol/L) [OCl-]0(mol/L) Initial Rate (mol/L ·s) 0.12 0.18 7.91x 10-2 0.060 0.18 3.95 x 10-2 0.030 0.090 9.88 x 10-3 0.24 0.090 7.91x 10-2 a. What is the rate law? b. Calculate the value of the rate constant. c. Calculate the initial rate for an experiment where both I- and OCl- are initially present at 0.15 mol/L.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 12PS: The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table...
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The reaction

I- (aq) + OCl- (aq) → IO- (aq) + Cl- (aq)

was studied, and the following data were obrained:

[I-]0(mol/L)

[OCl-]0(mol/L)

Initial Rate (mol/L ·s)

0.12

0.18

7.91x 10-2

0.060

0.18

3.95 x 10-2

0.030

0.090

9.88 x 10-3

0.24

0.090

7.91x 10-2

a. What is the rate law?

b. Calculate the value of the rate constant.

c. Calculate the initial rate for an experiment where both I- and OCl- are initially present at 0.15 mol/L.

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