Chemical Equilibrium in Chemistry 222: Understanding Principles and Calculations, Study notes of Chemistry

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Kc ' [C] [A]ca^ [D][B]db

Q ' [C] [A]ca^ [D][B]bd

Kp ' p^ Cc p^ Dd p (^) Aa p (^) Bb

x ' &^ b ±^ 2 ab^2 &^ 4 a c

Chemistry 222 Chapter 16 - Principles of Chemical EquilibriumChapter 16 - Principles of Chemical Equilibrium Petrucci/8th Ed. THINGS TO KNOW - THINGS TO DO This is a very important chapter in that it sets down the basic description of chemical equilibrium that will be u and in subsequent chapters. Doing good work here will pay off. We will cover the entire chapter, sections 16.116.

The SUMMARY of Chapter 16 on page 656 covers the important facts. You should know the definition of each w in the KEY TERMS list on page 657. LeChatelier's Principle (section 16.6) is an especially important concept in chapter. You should know how to use the following equations:

For an equation of the form: a A + b B + W c C + d D (W denotes the equilibrium state) The relationship between the four concentrations at equilibrium is: (page 631)

For the system notnot at equilibrium, the reaction quotient, QQ , is: (page 623) Note: For the reaction quotient, the initial concentrations are used (not the eqm^ values)

For gaseous systems in equilibrium express concentration at partial pressure: (page 640)

The relationship between Kc and Kp for a system in equilibrium: (page 635, eqn 16.12) Kp = Kc(RT))n(g)^ R = 0.0821 L-atm/mol-K For many problems the quadratic equation will be useful: for: 4.3x^2 + 1.6x !0.25 = 0 a = 4.3b = 1. c = !0. There are several problems presented through out the chapter, and you should work Review Questions Review Questions on pages 657 & 658. Answers are on page A-56 in the Appendix. Also, do the following: each one of these as well al

25, 29, 33, 37, 39, 45, 49, 67 In addition, several sets of problems will be handed out in class.