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?
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter18: Chemical Kinetics
Section: Chapter Questions
Problem 37P
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Question
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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