The reaction of tert -butyl chloride with methanol is found to follow the rate equation rate = k r [(CH 3 ) 3 C—Cl] a. What is the kinetic order with respect to tert -butyl chloride?

welcome back everyone to chloral to methyl butane reacts with methanol according to the following chemical reaction. Experimental results suggest that the reaction follows the rate equation shown below where the rate of our reaction is equal to the rate constant K. Times the concentration of our first reactant to chloral. Two methyl butane determine the kinetic order with respect to two chloral, two methyl butane. We want to recall that we can find this kinetic order given by the implied exponents for our reactant in the given rate law. And so we would say that the proportion of the rate of the reaction to the concentration of our first reactant to chloral, two metal butane raised to a power of one, determines that the kinetic order of the reaction with respect to to clarity metal butane is first order based on that power of one in the rate law. When it comes to the proportion of the reaction rate to our concentration of methanol. So let's write its formula actually as C three, C H 30. H. We see that it's not technically included, are given rate law in the prompt. And so that tells us that we have a power of zero. Where anything we recall race to power of zero equals a value of one, which tells us that the reaction is going to be zero order. Sorry, zeroth order as the kinetic order of the reaction with respect to methanol. Now, to complete this prompt, our final answer is going to be that the kinetic order with respect to to core two methyl butane is going to be first order corresponding to choice be in the multiple choice as our final answer. I hope that everything I explained was clear. If you have any questions, please leave them down below and I'll see everyone in the next practice video.

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6. Thermodynamics and Kinetics

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Problem 11a

Textbook Question

The reaction of tert-butyl chloride with methanol

is found to follow the rate equation
rate = k_r[(CH₃)₃C—Cl]
a. What is the kinetic order with respect to tert-butyl chloride?

Verified step by step guidance

Step 1: Analyze the given reaction. The reaction involves tert-butyl chloride ((CH3)3C—Cl) reacting with methanol (CH3—OH) to form methyl tert-butyl ether ((CH3)3C—OCH3) and HCl. This is a substitution reaction.

Step 2: Examine the rate equation provided: rate = Kt[(CH3)3C—Cl]. The rate equation indicates that the rate of the reaction depends only on the concentration of tert-butyl chloride.

Step 3: Recall the definition of kinetic order. The kinetic order with respect to a reactant is determined by the exponent of its concentration term in the rate equation. Here, the concentration of tert-butyl chloride is raised to the power of 1.

Step 4: Conclude that the reaction is first-order with respect to tert-butyl chloride because the rate equation shows a direct proportionality to [(CH3)3C—Cl] raised to the power of 1.

Step 5: Note that this reaction likely proceeds via an SN1 mechanism, as the rate depends only on the concentration of tert-butyl chloride and not on methanol. This mechanism involves the formation of a carbocation intermediate.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Kinetics and Rate Laws

Kinetics is the study of the rates of chemical reactions. The rate law expresses the relationship between the rate of a reaction and the concentration of its reactants. In this case, the rate equation indicates that the reaction rate depends only on the concentration of tert-butyl chloride, suggesting it is a first-order reaction with respect to this reactant.

Substitution Reactions

The reaction of tert-butyl chloride with methanol is an example of a nucleophilic substitution reaction, where a nucleophile (methanol) replaces a leaving group (chloride ion). This type of reaction can proceed via different mechanisms, such as SN1 or SN2, with the SN1 mechanism being favored for tertiary alkyl halides like tert-butyl chloride due to steric hindrance.

Energy Diagrams

Energy diagrams visually represent the energy changes during a chemical reaction. They illustrate the transition states and intermediates, showing how the energy of the system changes from reactants to products. In this reaction, the energy diagram would depict the activation energy required for the formation of the carbocation intermediate, which is a key feature of the SN1 mechanism.

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The reaction of tert-butyl chloride with methanol(CH3)3C—Cl Tert-butylchloride + CH3—OH methanol —> (CH3)C—OCH3 methyltert-butylether + HCl is found to follow the rate equation rate= Kt[(CH3)3C—Cl] a. What is the kinetic order with respect to tert-butyl chloride?

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The reaction of tert-butyl chloride with methanol

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rate = k_r[(CH₃)₃C—Cl]

c. What is the kinetic order overall

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The reaction of tert-butyl chloride with methanol(CH3)3C—Cl Tert-butylchloride + CH3—OH methanol —> (CH3)C—OCH3 methyltert-butylether + HCl is found to follow the rate equation rate= Kr[(CH3)3C—Cl] c. What is the kinetic order overall?

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The reaction of tert-butyl chloride with methanol is found to follow the rate equation rate = kr[(CH3)3C—Cl] a. What is the kinetic order with respect to tert-butyl chloride?

Key Concepts

Kinetics and Rate Laws

Substitution Reactions

Energy Diagrams

Watch next

The reaction of tert-butyl chloride with methanol

is found to follow the rate equation
rate = k_r[(CH₃)₃C—Cl]
a. What is the kinetic order with respect to tert-butyl chloride?