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A study was made of the effect of the hydroxide concentration on the rate of the reaction: I- (aq) + OCI (aq) → IO (aq) + Cl(aq) The following data were obtained: [1], (mol/L) 0.0013 0.0026 0.0013 0.0013 0.0013 0.0013 0.0013 [OCI ]o (mol/L) 0.012 0.012 0.0060 0.018 0.012 0.012 0.018 Determine the rate law. [OH-], (mol/L) 0.10 0.10 0.10 0.10 0.050 0.20 0.20 Initial Rate (mol/L-s) 9.4 x 10-3 18.7 x 10-3 4.7 x 10-3 14.0 x 10-3 18.7 x 10-3 4.7 x 10-3 7.0 × 10-³

A study was made of the effect of the hydroxide concentration on the rate of the reaction: I- (aq) + OCI (aq) → IO (aq) + Cl(aq) The following data were obtained: [1], (mol/L) 0.0013 0.0026 0.0013 0.0013 0.0013 0.0013 0.0013 [OCI ]o (mol/L) 0.012 0.012 0.0060 0.018 0.012 0.012 0.018 Determine the rate law. [OH-], (mol/L) 0.10 0.10 0.10 0.10 0.050 0.20 0.20 Initial Rate (mol/L-s) 9.4 x 10-3 18.7 x 10-3 4.7 x 10-3 14.0 x 10-3 18.7 x 10-3 4.7 x 10-3 7.0 × 10-³

Chemistry
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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A study was made of the effect of the hydroxide concentration on the rate of the reaction: I- (aq) + OC (aq) IO (aq) + Cl(aq) The following data were obtained: [1] (mol/L) 0.0013 0.0026 0.0013 0.0013 0.0013 0.0013 0.0013 [OCI-], (mol/L) 0.012 0.012 0.0060 0.018 0.012 0.012 0.018 Determine the rate law. O A. k[OH-][OCI][I]¹ O B. k[OH ][OCI][I] O C. k[OH-][OC]0.5[1] O D. K [OCI-]²[1] O E. K[OH] [I] [OH-] (mol/L) 0.10 0.10 0.10 0.10 0.050 0.20 0.20 Initial Rate (mol/Ls) 9.4 x 10-3 18.7 x 10-3 4.7 x 10-3 14.0 × 10-3 18.7 x 10-3 4.7 x 10-3 7.0 × 10-³
Transcribed Image Text:A study was made of the effect of the hydroxide concentration on the rate of the reaction: I- (aq) + OC (aq) IO (aq) + Cl(aq) The following data were obtained: [1] (mol/L) 0.0013 0.0026 0.0013 0.0013 0.0013 0.0013 0.0013 [OCI-], (mol/L) 0.012 0.012 0.0060 0.018 0.012 0.012 0.018 Determine the rate law. O A. k[OH-][OCI][I]¹ O B. k[OH ][OCI][I] O C. k[OH-][OC]0.5[1] O D. K [OCI-]²[1] O E. K[OH] [I] [OH-] (mol/L) 0.10 0.10 0.10 0.10 0.050 0.20 0.20 Initial Rate (mol/Ls) 9.4 x 10-3 18.7 x 10-3 4.7 x 10-3 14.0 × 10-3 18.7 x 10-3 4.7 x 10-3 7.0 × 10-³
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