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Chapter 6: Problem 6.20 (page 233)

Draw an energy diagram for a two-step reaction, A鈫�B鈫�C, where the relative energy of these compounds is C<A<B, and the conversion of B鈫�Cis rate-determining.

Short Answer

Expert verified

Answer

The energy diagram is as follows:

Step by step solution

01

Step-by-Step SolutionStep 1: Energy diagram

An energy diagram (energy vs. reaction coordinate) is used to describe the change in energy of a system during the conversion of the reactants to the products.

02

Rate determining step

The step (in a chemical reaction) that takes the maximum time in the conversion of the reactants to products is termed the rate-determining step.

The rate-determining step has the maximum activation energy barrier.

03

Energy diagram of the given reaction

The reaction involves the transformation of the reactant A to product C through an intermediate B.

Species C has the lowest energy, and B has the highest energy.

Since it is given that the conversion of B to C is the rate-determining step, the activation energy barrier between B and C will be the maximum.

Energy diagram of a two-step reaction

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Most popular questions from this chapter

The conversion of acetyl chloride to methyl acetate occurs via the following two-step mechanism:

a. Add curved arrows to show the movement of the electrons in each step.

b. Write the rate equation for this reaction, assuming the first step is rate-determining.

c. If the concentration of were increased 10 times, what would happen to the rate of the reaction?

d. If the concentrations of both and were increased 10 times, what would happen to the rate of the reaction?

e. Classify the conversion of acetyl chloride to methyl acetate as an addition, elimination, or substitution.

Use the values in Table 6.2 to calculatefor each reaction. Classify each reaction as endothermic or exothermic.

a.

b.

As we learned in Chapter 4, propane (CH3CH2CH3)has both 1掳and 2掳hydrogens.

  1. Draw the carbon radical formed by homolysis of each type of C-H bond.
  2. Use the values in Table 6.2 to determine which C-H bond is stronger.
  3. Explain how this information can be used to determine the relative stability of the two radicals formed. Which radical formed from propane is more stable?

Write a rate equation for each reaction, given the indicated mechanism.

a.

b.

The following is a concerted, bimolecular reaction:CH3+NaCN鈫�CH3CN+NaBr.

a. What is the rate equation for this reaction?

b. What happens to the rate of the reaction if[CH3Br] is doubled?

c. What happens to the rate of the reaction if [NaCN] is halved?

d. What happens to the rate of the reaction if [CH3Br] and [NaCN] are both increased by a factor of five?
See all solutions

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