**Review Sheet for Physical Chemistry I 330****,
Exam One, Lycoming College, Fall 2006, Dr. Mahler**

**Chapter One** (all sections) States of gases, equation of state; p, V, T, n
– units and how to measure these; diathermic, adiabatic, isobar, isochore,
isotherm; Ideal Gas law and constant, and laws in it (Boyle's, Charles',
Avogadro's); SATP and STP; Molecular motion in gases, Kinetic Theory of Gases,
root mean square speed; Zeroth Law of Thermodynamics; Real gases - repulsive and
attractive forces, compression factor Z and molar volume; other equations of
state (van der Waals, virial); critical point and constants (p, V, T); principle
of corresponding states.

**Chapter 1**:

Exercises 1.1 (Ideal and van der Waals Gas Laws), 2 (Boyle’s Law), 3 (Ideal Gas Law), 8 (Density of gases, IGL), 10 (Dalton’s Law of Partial Pressures, mole fractions, IGL), 13 (van der Waals, IGL), 16 (Z, vdW), 18 (Dalton’s, IGL), 21 (Principle of Corresponding States).

**Chapter Twenty One** (section 1) Molecular motion in gases, Kinetic Theory
of Gases; Maxwell distribution and types of molecular speed; collision-diameter
and, collision-cross section, collision-frequency, and mean-free path.

**Chapter 21**:

Exercises 21.1 (mean speed), 2 (mean speed, mean free path, collision frequency), 4 (mean free path),

5 (collision frequency), 6 (mean free path).**Chapter Two** (all sections) Definitions basic to Thermodynamics (system,
surroundings, open, closed, isolated, energy, work, heat, diathermic, adiabatic,
exothermic, endothermic, etc.); First Law of Thermodynamics and internal energy
(U); State functions; Expansion work, types (free, (isothermal) reversible,
against constant pressure); Reversible vs. irreversible processes and
equilibrium; Calorimetry and thermochemistry; Enthalpy (heat at constant
pressure), relation to U and temperature dependence; Heat capacities at constant
pressure and volume; adiabatic changes, work, P,V, T; standard enthalpy changes
and Hess' law, thermochemical equations; Standard enthalpies of formation;
stoichiometric numbers; Kirchoff's law and enthalpy temperature dependence; )
State functions and exact differentials; partial derivatives and their
properties; partial derivative properties for all systems and for ideal gases,
and their relations (heat capacities C_{P} and C_{V}, internal
pressure ˙_{T},
expansion coefficient ˙,
isothermal compressibility ˙_{T},
(isothermal) Joule-Thomson coefficient ˙
and ˙_{T},
and inversion temperature); temperature dependence of enthalpy.

**Chapter 2**: Exercises 2.2 (pV work), 3 (work and q,
˙U,
˙H), 4 (isochoric heat),
7 (pV work of a reaction), 10 (adiabatic rev. work), 14 (adiabatic w, q,
˙U,
˙H,
˙T), 17, 18, 21, (Hess’
Law, ˙H of
formation), 28 (Born-Haber cycle –
more thermochemical equations).

**Chapter Three** (sections 1, 2a) Entropy –
spontaneity, Second Law of Thermodynamics, dispersal of energy, time’s arrow,
definition of S.

**Chapter Seven** (sections 5, 6, 7, 8) Electrochemistry ; redox chemistry,
half reactions, anode, cathode, cell reaction, Nernst equation, standard
potentials (voltages). Ions and Electrochemistry; Properties of Ions in solution
(mean ionic activity coefficient); Debye-Hückel limiting law; Electrochemical
cells & their conventions and definitions; Half cells and half reactions;
Electrochemical relations (Nernst equation, standard potentials).

**Chapter 7**: Exercises 7.14 (electrode & cell rxns), 15, (devise cells to
get rxns), 16 (Nernst, ˙G).