Book cover for Chemistry and Chemical Reactivity

Chemistry and Chemical Reactivity

John C. Kotz, Paul M. Treichel, John R. Townsend

ISBN #9780840048288

8th Edition

2,165 Questions

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24,952 Students Helped

Homework Questions

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Summary
Learning Objectives
Key Concepts
Example Problems
Explanations
Common Mistakes

Summary

This textbook section reviews the fundamentals of energy, introducing both macroscopic and microscopic perspectives. It connects everyday concepts such as the caloric value of food with chemical thermodynamics principles, including the measurement of energy changes using specific heat, calorimetry, the first law of thermodynamics, and Hess’s law. Additionally, concepts such as state functions and enthalpy provide the framework for understanding energy exchanges in chemical reactions, both in practical laboratory settings and in real-world applications such as fuel combustion and energy production.

Learning Objectives

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Key Concepts

CONCEPT

DEFINITION

Brønsted–Lowry and Lewis definitions

A study of acid–base concepts encompassing both the Brønsted–Lowry and Lewis definitions. This topic explains how to write balanced acid–base reactions, analyze equilibria using ICE tables, and understand molecular influences (such as bond strength and resonance) on acid strength.

Example Problems

Example 1

Define the terms system and surroundings. What does it mean to say that a system and its surroundings are in thermal equilibrium?

Example 2

What determines the directionality of energy transfer as heat?

Example 3

Identify whether the following processes are exothermic or endothermic. (a) combustion of methane (b) melting of ice (c) raising the temperature of water from $25^{\circ} \mathrm{C}$ to $100^{\circ} \mathrm{C}$ (d) heating $\operatorname{CaCO}_{3}(\mathrm{s})$ to form $\mathrm{CaO}(\mathrm{s})$ and $\mathrm{CO}_{2}(\mathrm{g})$

Example 4

Identify whether the following processes are exothermic or endothermic. (a) the reaction of $\mathrm{Na}(\mathrm{s})$ and $\mathrm{Cl}_{2}(\mathrm{g})$ (b) cooling and condensing gaseous $N_{2}$ to form liquid $\mathrm{N}_{2}$ (c) cooling a soft drink from $25^{\circ} \mathrm{C}$ to $0^{\circ} \mathrm{C}$ (d) heating $\mathrm{HgO}(\mathrm{s})$ to form $\mathrm{Hg}(\ell)$ and $\mathrm{O}_{2}(\mathrm{g})$

Example 5

The molar heat capacity of mercury is $28.1 \mathrm{J} / \mathrm{mol} \cdot \mathrm{K}$ What is the specific heat capacity of this metal in $\mathrm{J} / \mathrm{g} \cdot \mathrm{K}$ ?
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Step-by-Step Explanations

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Common Mistakes

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