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?

Question
Asked Mar 17, 2019
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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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Expert Answer

Step 1

The hydrolysis of tert-butyl chloride reaction takes place through SN1 reaction.  This  reaction gives tert-butanol and Hydrochloric acid as products.

Step 2

This reaction is a two...

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