For the t-butyl chloride hydrolysis reaction, which was the kinetics demonstration from lecture, we saw one reaction go much faster (in other words, it turned from green to red faster) than the other reaction, even though they were both at the same temperature. Why was it that one reaction went faster than the other? Answer: One solution was more concentrated in the reactant and the reaction was governed by 1st order kinetics, so an increase in [reactant] caused an increase in the rate. Can you explain how this relates to first order kinetics?
For the t-butyl chloride hydrolysis reaction, which was the kinetics demonstration from lecture, we saw one reaction go much faster (in other words, it turned from green to red faster) than the other reaction, even though they were both at the same temperature. Why was it that one reaction went faster than the other? Answer: One solution was more concentrated in the reactant and the reaction was governed by 1st order kinetics, so an increase in [reactant] caused an increase in the rate. Can you explain how this relates to first order kinetics?
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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For the t-butyl chloride hydrolysis reaction, which was the kinetics demonstration from lecture, we saw one reaction go much faster (in other words, it turned from green to red faster) than the other reaction, even though they were both at the same temperature. Why was it that one reaction went faster than the other?
Answer:
One solution was more concentrated in the reactant and the reaction was governed by 1st order kinetics, so an increase in [reactant] caused an increase in the rate.
Can you explain how this relates to first order kinetics?
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