A Working Method Approach For Introductory Physical Chemistry Calculations (Rsc Paperbacks),Used

Excerpt. Reprinted by permission. All rights reserved.A Working Method Approach for Introductory Physical Chemistry CalculationsNumerical and Graphical Problem SolvingBy Brian Murphy, Clair Murphy, Brian Hathaway The Royal Society of ChemistryCopyright 1997 The Royal Society of ChemistryAll rights reserved.ISBN: 9780854045532ContentsChapter 1 Introduction to Physical Chemistry: Acids and Bases The Gas Laws, Numerical and Graphical Problem Solving, 1,Chapter 2 Thermodynamics I: Internal Energy, Enthalpy, First Law of Thermodynamics, State Functions, and Hess's Law, 17,Chapter 3 Thermodynamics 11: Enthalpy, Heat Capacity, Entropy, the Second and Third Laws of Thermodynamics and Gibbs Free Energy, 24,Chapter 4 Equilibrium I: Introduction to Equilibrium and Le Chtelier's Principle, 36,Chapter 5 Equilibrium 11: Aqueous Solution Equilibria, 47,Chapter 6 Electrochemistry I: Galvanic Cells., 63,Chapter 7 Electrochemistry 11: Electrolytic Cells, 89,Chapter 8 Chemical Kinetics I: Basic Kinetic Laws, 113,Chapter 9 Chemical Kinetics II: The Arrhenius Equation and Graphical Problems, 128,Answers to Problem, 145,Further Reading, 147,Periodic Table of the Elements, 148,Subject Index, 149,CHAPTER 1Introduction to Physical Chemistry: Acids and Bases, The Gas Laws and Numerical and Graphical Problem SolvingINTRODUCTIONThis chapter is a brief introduction to many of the assumptions made in the remainder of this text and the basis of physical chemistry type problems. The spider diagram of Figure 1.1 illustrates the various sections.STATES OF MATTERMutter is the chemical term for materials. There are three states of matter: the solid phase (s), the liquid phase (1) and the gaseous phase (g). In the solid phase, all the atoms or molecules are arranged in a highly ordered manner [Figure 1,2(a)], whereas in the liquid phase [Figure 1.2(b)], this ordered structure is not as evident. In the gaseous phase [Figure 1.2(c)), all the particles are moving at high velocity, in random motion. The disorder or entropy, S, is at its maximum in the gaseous phase [Figure 1.2(c)].If a species is dissolved in water, it is said to be in the aqueous phase (aq), and the symbol can be represented as a subscript, e.g. HCl(aq).ACIDS AND BASESAn acid is a proton (H+) donor and a base is a proton acceptor, e.g. (OH). Examples of acids include HCl, H2SO4, HNO3, HCN and CH3CO2H. A monoprotic acid is an acid with one replaceable proton, e.g. HCl (eA = 1); a diprotic acid is an acid with two replaceable protons e.g. H2SO4 (eA = 2) etc., where eA is the number of reactive species. A dilute acid is an acid which contains a small amount of acid dissolved in a large quantity of water, whereas a concentrated acid is an acid which contains a large amount of acid dissolved in a small quantity of water.Examples of bases include NaOH (eB = 1), KOH (eB = 1), Ba(OH)2 (eB = 2), Ca(OH)2 (eB. An acid combines with a base to form a salt and water:i.e. ACID + BASE [right arrow] SALT + WATERe.g. HNO3 + NaOH [right arrow] NaNO3 + H2OIn general, an acid can be represented as HA, where HA [right arrow] H+ + A or, more precisely, HA + H2O [right arrow] A + H3O+, since all aqueous protons are solvated by water. Likewise, a base containing hydroxide anions, OH, can be represented as MOH, where MOH [right arrow] M+ + OH.When an acid donates a proton, H+, it is said to form the conjugate base of the acid, i.e. HA (acid) [??] H+ + A (conjugate base). The conjugate base is a base since it can accept a proton to reform HA, the acid. Similarly, when a base accepts a proton, H+, the conjugate acid of the base is said to be formed, i.e. B (base) + H+ [??] HB+ (conjugate acid). The conjugate acid is an acid since it can donate a proton, H+, and reform the base, e.g. NH4+ (conjugate acid) [??] NH3 (base) + H+.Ions, Cations, Anions, Oxyanions and OxyacidsIons are charged species, e.g. Na+, Cl, NH4+etc. Cations are positively charged ions, e.g. Na+, NH