Ch.14 - Chemical Kinetics

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

McMurry 8th Edition

Ch.14 - Chemical Kinetics

Problem 48b

Chapter 14, Problem 48b

Consider a reaction that occurs by the following mechanism:
A + BC → AC + B
AC + D → A + CD
The potential energy profile for this reaction is as follows:
(b) Write structural formulas for all species present at reaction stages 1–5. Identify each species as a reactant, product, catalyst, intermediate, or transition state.

Verified step by step guidance

Step 1: Identify the species involved in each elementary step of the reaction mechanism.

Step 2: For the first step, A + BC → AC + B, identify A and BC as reactants, AC and B as products.

Step 3: For the second step, AC + D → A + CD, identify AC and D as reactants, A and CD as products.

Step 4: Determine the role of each species: A is a catalyst as it is regenerated, AC is an intermediate as it is formed and consumed, BC and D are reactants, B and CD are products.

Step 5: Consider the potential energy profile to identify transition states, which are high-energy states between reactants and products in each step.

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Key Concepts

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

Reaction Mechanism

A reaction mechanism is a step-by-step description of the pathway taken by reactants to form products. It outlines the sequence of elementary reactions, including the formation of intermediates and transition states. Understanding the mechanism helps in predicting the rate and outcome of the reaction, as well as identifying the roles of different species involved.

Structural Formulas

Structural formulas represent the arrangement of atoms within a molecule, showing how atoms are bonded together. They provide insight into the molecular geometry and functional groups present in each species. Writing structural formulas is essential for identifying the chemical nature of reactants, products, intermediates, and catalysts in a reaction.

Catalysts and Intermediates

Catalysts are substances that increase the rate of a reaction without being consumed, while intermediates are transient species formed during the reaction that are not present in the final products. Recognizing these roles is crucial for understanding the overall reaction dynamics and energy changes, as intermediates often have distinct structural features that can be identified in the reaction mechanism.

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Catalyzed vs. Uncatalyzed Reactions

Related Practice

Textbook Question

The relative rates of the reaction A + B S AB in vessels(1)–(3) are 4:4:1. Red spheres represent A molecules, andblue spheres represent B molecules.(1)-(3)

(a) What is the order of the reaction in A and B?

Textbook Question

What is the molecularity of each of the following elementary reactions?(a)

(b)

(c)

Textbook Question

Draw a plausible transition state for the bimolecular reaction of nitric oxide with ozone. Use dashed lines to indicate the atoms that are weakly linked together in the transition state. NO(g) + O3(g) NO2(g) + O2(g)

Textbook Question

Consider a reaction that occurs by the following mechanism:

A + BC → AC + B

AC + D → A + CD

The potential energy profile for this reaction is as follows:

(d) Is the reaction endothermic or exothermic? Add labels to the diagram that show the values of the energy of reaction ΔE and the activation energy Ea for the overall reaction.

Textbook Question

The following pictures represent the progress of a reaction in which two A molecules combine to give a more complex molecule A2, 2 AS A2.

(b) What is the rate law?

Textbook Question

Consider a reaction that occurs by the following mechanism:

A + BC → AC + B

AC + D → A + CD

The potential energy profile for this reaction is as follows: