In Experiment M you studied the reaction: S2Og²- + 2l¯ → 2SO42- + 12 The reaction time was monitored by the "iodine clock reaction": 2S2032- + 12→ 21¯ + S406²- When the above reaction was carried at 22°C (using the same concentrations) with a trace of copper sulfate, the time for the reaction decreased because: The rate constant decreases due to the presence of the copper ions The rate constant decreases due to the presence of the sulfate ions The copper ions provide an alternative path for the reaction of S20g²- + 2I° The copper ions increase AH so more molecules of S2032- could react OThe copper ions provide an alternative path for the reaction of S2O3²- with I2

In Experiment M you studied the reaction: S2Og²- + 2l¯ → 2SO42- + 12 The reaction time was monitored by the "iodine clock reaction": 2S2032- + 12→ 21¯ + S406²- When the above reaction was carried at 22°C (using the same concentrations) with a trace of copper sulfate, the time for the reaction decreased because: The rate constant decreases due to the presence of the copper ions The rate constant decreases due to the presence of the sulfate ions The copper ions provide an alternative path for the reaction of S20g²- + 2I° The copper ions increase AH so more molecules of S2032- could react OThe copper ions provide an alternative path for the reaction of S2O3²- with I2

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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* 97% 7:58 PM Wed Feb 12 х Unanswered •1 attempt left • Due on Feb 13 Rate law of a reaction is experimentally determined as Rate = k [A]^2 [B]^0 [C] The unit of k is sec/M 1/M^3-sec 1/M^2-secc. 1/M^4-sec M^3/sec Submit