Chem 142B Aut 11 - List of Topics to Review for Exam 2*
We have started applying the concepts we learned in Chapters 1-4 to new reactions and
experimental conditions. It is assumed for Exam 2 and future exams that you know ALL of the
material on the Exam 1 topic list, regardless of whether or not it showed up on Exam 1. You
can expect to see comprehensive problems on future exams, so please be sure that you keep
those previous chapters in mind as you study, work through problems, and take the exam.
Types of Chemical Reactions and Solution Stoichiometry (Chapter 4, section 11)
 Balancing oxidation-reduction equations
o Half reaction method and/or oxidation state method (you can use whichever you feel
most comfortable with)
o Balancing reactions in acidic or basic solutions
Gases (Chapter 5, sections 1-8, 10, and 11)
 Definition and common units of pressure
 Instruments for measuring pressure (how do you use the measurements from a manometer to
determine the pressure of a gas or the atmosphere)
 Qualitative and quantitative evaluations of the laws from Boyle, Charles, Avogadro, and
Amontons, as well as the ideal gas law
o Variations of the form of the ideal gas law (if you have, or are looking for, density or
molar mass)
o Calculations involving change of conditions
o Combining the gas laws with reaction stoichiometry – use the gas laws to get the
moles of reactants and/or products and use the mole ratios from balanced reactions to
find the amounts of reactants/products used up or produced
 STP; standard volume only applies if you have 1 mole of substance at STP
 Mole fractions and Dalton’s law of partial pressures
o Also, using partial pressures when considering a reaction for which a gaseous product
is collected over water (you’ll have to be given the vapor pressure of water at a
specified temperature)
 Kinetic Molecular Theory (KMT)
o The four postulates of the KMT theory
o Purpose of the KMT; how does it support the experimentally determined ideal gas law
o Calculate kinetic energy (KEavg of a molecule and KEavg for a mole of gas molecules);
watch your units!
o Calculate the root mean square velocity; watch your units!
o How do velocity and kinetic energy change with mass of the particles, number of
particles, temperature, etc. (understand which variables affect these observed
properties and understand how changes in the variables will translate to changes in the
observed properties (i.e., if temperature doubles, what happens to…)
 Effusion and Diffusion
o Difference between effusion and diffusion
o Relationship between rate of effusion/diffusion and molar mass of a gas
o Calculate the relative rates/velocities of effusion/diffusion of two gases
 Collisions with Container Walls
 Real vs ideal gases – qualitative differentiation; calculations with van der Waals equation
* While this a very full list, it’s always possible that I’ve overlooked something when putting this
together. I suggest that you carefully review the lecture notes, worksheets, and labs, and, of course,
be sure you have read the chapters well. As you study, work through the list of end-of-chapter
problems posted on the course website in addition to any review of topics you decide to do in ALEKS.
Chemical Equilibrium (Chapter 6, sections 1-8)
 Definitions of equilibrium, equilibrium position, and equilibrium constant
 Write an equilibrium expression using activities (with concentrations or pressures)
o Understand why pure liquids and solids are not included
o Know the relationship between Kc and Kp
 Rearrange the equilibrium expression and recalculate the equilibrium constant when the reaction
is reversed, multiplied by a factor, etc.
 Determine the extent of reaction and how to calculate the reaction quotient (Q)
o Compare Q with K to determine in which direction the reaction will proceed
 Equilibrium calculations
o Calculate the equilibrium constant given the chemical reaction and the equilibrium
concentrations or pressures
o Find the equilibrium concentrations (or pressures) of reactants or products given the
value of the equilibrium constant and the initial concentrations
o Find initial concentrations (or pressures) of reactants or products given the value of the
equilibrium constant and additional necessary information
o Know your algebra!...how to work with the quadratic formula, how to solve for x and
then use x to calculate equilibrium or initial concentrations; know how/when to make
assumptions that will simplify these calculations and when they fail (5% rule, etc.).
 LeChâtelier’s Principle – how does a system at equilibrium respond to a change in conditions
o Effect of a change in concentration
o Effect of a change in (partial pressures!)
o Effect of a change in temperature
* While this a very full list, it’s always possible that I’ve overlooked something when putting this
together. I suggest that you carefully review the lecture notes, worksheets, and labs, and, of course,
be sure you have read the chapters well. As you study, work through the list of end-of-chapter
problems posted on the course website in addition to any review of topics you decide to do in ALEKS.