The reactionI (aq) + OCI (aq) → IO (aq) + Cl¯¯ (aq)was studied, and the following data were obtained:[I] (mol/L) [OCI]o (mol/L) Initial Rate (mol/Ls)8.30 × 10-24.20 × 10-²1.00 x 10-28.30 × 10-20.160.0800.040k =0.32Rate =0.200.200.10What is the rate law?(Use k for the rate constant.)0.10Calculate the value of the rate constant.L/mol sCalculate the initial rate for an experiment where bothI andOCI are initially present at 0.16 mol/L.Rate = |mol/L s

Recall the given reactionWhere K is rate constant

The reaction I (aq) + OCI (aq) → IO¯(aq) + CI¯ (aq) was studied, and the following data were obtained: [I] (mol/L) [OCI ]o (mol/L) Initial Rate (mol/Ls) 8.30 × 10-² 4.20 × 10-² 0.16 0.080 0.20 0.20 10-2

The reaction I (aq) + OCI (aq) → IO¯(aq) + CI¯ (aq) was studied, and the following data were obtained: [I] (mol/L) [OCI ]o (mol/L) Initial Rate (mol/Ls) 8.30 × 10-² 4.20 × 10-² 0.16 0.080 0.20 0.20 10-2

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 84AE: The reaction H2SeO3(aq) + 6I-(aq) + 4H+(aq) Se(s) + 2I-3(aq) + 3H2O(l) was studied at 0C, and the...

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Question

The reaction
I (aq) + OCI (aq) → IO (aq) + Cl¯¯ (aq)
was studied, and the following data were obtained:
[I] (mol/L) [OCI]o (mol/L) Initial Rate (mol/Ls)
8.30 × 10-2
4.20 × 10-²
1.00 x 10-2
8.30 × 10-2
0.16
0.080
0.040
k =
0.32
Rate =
0.20
0.20
0.10
What is the rate law?
(Use k for the rate constant.)
0.10
Calculate the value of the rate constant.
L/mol s
Calculate the initial rate for an experiment where both
I and
OCI are initially present at 0.16 mol/L.
Rate = |
mol/L s

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