The bromination of methane proceeds through the following steps: 1. Br2 + 2 Br• ΔH° (per mole)/+190 kJ (45 kcal) Ea (per mole)/ 190 kJ (45 kcal) 2. CH4 + Br• —\u003e CH3+ HBr +73 kJ (17 kcal) 79 kJ (19 kcal) 3. • CH3 + Br2 —\u003e CH3Br + Br -112 kJ (-27 kcal) 4 kJ (1 kcal) a. Draw a complete reaction-energy diagram for this reaction. b. Label the rate-limiting step.

Ch.4 - The Study of Chemical Reactions

Wade9th EditionOrganic ChemistryISBN: 9780135213728Not the one you use?Change textbook

All textbooks

Wade 9th Edition

Ch.4 - The Study of Chemical Reactions

Problem 4

Chapter 4, Problem 4

The bromination of methane proceeds through the following steps:1. Br2 + 2 Br• ΔH° (per mole)/+190 kJ (45 kcal)Ea (per mole)/ 190 kJ (45 kcal)2. CH4 + Br• —> CH3+ HBr +73 kJ (17 kcal) 79 kJ (19 kcal) 3. • CH3 + Br2 —> CH3Br + Br -112 kJ (-27 kcal) 4 kJ (1 kcal) a. Draw a complete reaction-energy diagram for this reaction. b. Label the rate-limiting step.

Verified step by step guidance

Identify the steps involved in the bromination of methane: initiation, propagation, and termination.

For the reaction-energy diagram, plot the energy on the y-axis and the reaction progress on the x-axis.

Start with the energy level of the reactants (Br2 and CH4) and show the energy change for each step.

Indicate the energy barrier (activation energy, Ea) for each step, especially focusing on the highest energy transition state.

Label the rate-limiting step as the one with the highest activation energy, which is typically the slowest step in the reaction.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

13m

Was this helpful?

Key Concepts

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

Reaction Energy Diagram

A reaction energy diagram visually represents the energy changes during a chemical reaction. It typically plots the energy of the reactants, products, and the transition states against the reaction coordinate. Key features include the activation energy (Ea) for each step and the overall change in enthalpy (ΔH°). Understanding this diagram is crucial for identifying the energy barriers and the stability of intermediates in the reaction.

Activation Energy (Ea)

Activation energy is the minimum energy required for a chemical reaction to occur. It represents the energy barrier that reactants must overcome to form products. In the context of the bromination of methane, each step has a specific Ea, which influences the rate of the reaction. The step with the highest Ea is the rate-limiting step, determining the overall speed of the reaction.

Rate-Limiting Step

The rate-limiting step is the slowest step in a multi-step reaction mechanism, which dictates the overall reaction rate. It has the highest activation energy compared to other steps, meaning it takes the longest time to occur. Identifying this step is essential for understanding the kinetics of the reaction and for predicting how changes in conditions might affect the reaction rate.

Recommended video:

Guided course

10:14

Limitations

Related Practice

Textbook Question

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.

1047

views

Textbook Question

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= 12Slower: CD4 + Cl⋅ —> CD3Cl + DClrelative 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.

1786

views

Textbook Question

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

1425

views

Textbook Question

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