The reaction of tert-butyl chloride with methanol (CH3)3C—Cl Tert-butylchloride + CH3—OH methanol —\u003e (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?

Ch.4 - The Study of Chemical Reactions

Wade9th EditionOrganic ChemistryISBN: 9780135213728당신이 사용하는 게 아니라요?교과서 변경

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Wade 9th Edition

Ch.4 - The Study of Chemical Reactions

문제 4

4장, 문제 4

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?

검증된 단계별 안내

Identify the rate equation given in the problem: rate = Kr[(CH3)3C—Cl].

Determine the order of reaction with respect to each reactant.

Notice that the rate equation only includes the concentration of tert-butyl chloride, [(CH3)3C—Cl].

Conclude that the reaction is first order with respect to tert-butyl chloride.

Since methanol does not appear in the rate equation, it is zero order with respect to methanol, making the overall kinetic order of the reaction first order.

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영상 길이:

주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Kinetics

Kinetics is the study of the rates of chemical reactions and the factors that affect these rates. It involves understanding how the concentration of reactants influences the speed of a reaction, which is often expressed through rate equations. In this case, the rate equation indicates that the reaction rate depends solely on the concentration of tert-butyl chloride.

Rate Equation

A rate equation describes the relationship between the rate of a chemical reaction and the concentration of its reactants. The general form includes a rate constant and the concentrations raised to a power, which reflects the order of the reaction with respect to each reactant. For the given reaction, the rate equation shows that the reaction is first-order with respect to tert-butyl chloride.

Kinetic Order

Kinetic order refers to the sum of the powers of the concentration terms in the rate equation, indicating how the rate of reaction changes with varying concentrations of reactants. In this case, since the rate equation is first-order in tert-butyl chloride and has no other reactants affecting the rate, the overall kinetic order of the reaction is one.

관련 실천

교과서 질문

Use the bond-dissociation enthalpies in Table 4-2 (page 167) to calculate the heats of reaction for the two possible first propagation steps in the chlorination of isobutane. Use this information to draw a reaction-energy diagram like Figure 4-8, comparing the activation energies for formation of the two radicals.

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교과서 질문

Deuterium (D) is the hydrogen isotope of mass number 2, with a proton and a neutron in its nucleus. The chemistry of deuterium is nearly identical to the chemistry of hydrogen, except that the C―D bond is slightly stronger than the C―H bond by 5.0 kJ/mol (1.2 kcal/ mol). Reaction rates tend to be slower when a C―D bond (as opposed to a C―H bond) is broken in a rate-limiting step. This effect, called a kinetic isotope effect, is clearly seen in the chlorination of methane. Methane undergoes free-radical chlorination 12 times as fast as tetradeuteriomethane (CD4) Faster: CH4 + Cl⋅ —> CH3Cl + HCl relative rate= 12 Slower: CD4 + Cl⋅ —> CD3Cl + DCl relative rate= 1 c. Consider the thermodynamics of the chlorination of methane and the chlorination of ethane, and use the Hammond postulate to explain why one of these reactions has a much larger isotope effect than the other.

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교과서 질문

Use bond-dissociation enthalpies [TABLE 4-2], p. 167) to calculate values of ΔH° for the following reactions. a. CH3—CH3 + I2 —> CH3CH2I + HI

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교과서 질문

Free-radical chlorination of hexane gives very poor yields of 1-chlorohexane, while cyclohexane can be converted to chlorocyclohexane in good yield.