Book cover for Chemistry

Chemistry

Catherine E. Housecroft, Edwin C. Constable

ISBN #9780273715450

4th Edition

995 Questions

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Homework Questions

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Summary
Learning Objectives
Key Concepts
Example Problems
Explanations
Common Mistakes

Summary

This section on reaction kinetics provides a comprehensive framework for understanding how reaction rates depend on reactant concentrations, temperature, and catalysts. It elucidates methods for determining reaction order, integrating rate laws, and analyzing complex mechanisms including catalytic processes, reversible reactions, and enzyme kinetics. Mastery of these concepts is crucial for interpreting experimental data and designing effective chemical processes in both academic research and industrial applications.

Learning Objectives

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Key Concepts

CONCEPT

DEFINITION

Acyclic and cyclic alkanes

A discussion of both open?chain (acyclic) and ring (cyclic) saturated hydrocarbons, emphasizing their structural features, nomenclature, conformational behavior (including ring strain and conformation), and the processes used in their interconversion and synthesis.

Example Problems

Example 1

(a) The data plotted in Figure $15.4 \mathrm{a}$ refer to a reaction: $A \rightarrow$ products. Determine the rate of this reaction. (b) Figure $15.4 \mathrm{b}$ describes a different reaction: $A \rightarrow$ products, in which the rate changes as a function of time. Determine the rates of reaction at times $t_{1}$ and $t_{2}$ marked on the graph.

Example 2

For a reaction $A \rightarrow$ products which is zero order with respect to A, sketch a graph of (a) rate of reaction against time, and (b) $[\mathrm{A}]$ against time. Repeat the exercise for reactions that are first and second order with respect to A.

Example 3

For a reaction $A \rightarrow$ products which is first order with respect to A, show that the units of the rate constant are $s^{-1}$. Similarly, confirm that the units of the second order rate constant are $\mathrm{dm}^{3} \mathrm{mol}^{-1} \mathrm{s}^{-1}$.

Example 4

What is meant by each of the following terms: (a) rate of reaction; (b) differential and integrated forms of a rate equation; (c) order of a reaction (both the overall order and the order with respect to a given reactant); (d) rate constant, pseudo-nth order rate constant and overall rate constant; (e) activation energy; (f) catalysis and autocatalysis; (g) unimolecular step; (h) bimolecular step?

Example 5

Iron(III) oxidizes iodide according to the following equation: $$2 \mathrm{Fe}^{3+}+2 \mathrm{I}^{-}-2 \mathrm{Fe}^{2+}+\mathrm{I}_{2}$$ Write down a rate equation for this reaction if doubling the iodide concentration increases the rate by a factor of four, and doubling the $\mathrm{Fe}^{3+}$ ion concentration doubles the rate.
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Step-by-Step Explanations

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Common Mistakes

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