Review2s10 - Dr McCord CH302 REVIEW for EXAM 2 Spring 2010 page 1 Textbook Chapters for Exam 2 All of Chapters 6 and 7 PLUS remember Chapter 10

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Textbook Chapters for Exam 2 All of Chapters 6 and 7 PLUS remember Chapter 10 sections 10 and 11. You’re responsible for any material covered in class whether it was on the homework or not. This review sheet covers most everything we have done. Also remember that no equa- tions are given on the exams. Values for equilibrium constants are given where needed although you should know K w . Chemical Equilibrium • Know how to WRITE the mass action expression — same as equilibrium equation How does this expression change and the value of K when a reaction is "flipped", doubled, halved? When is this expression equal to Q ? When is it equal to K ? • What is thermodynamic K ? How does that relate to K p and K c ? • How does K p relate to K c ? When would they be equal? • What is the relationship between ± G rxn and Q ? (answer: ± G = ± G ° + RT ln Q ) • What is the relationship between ± G 0 rxn and K ? (answer: ± G ° = - RT ln K ) This is the Chapter 10 stuff in sections 10 and 11 — you might even have to back up a bit and reread section 9. • What are the units for an equilibrium constant? There are NO units. Why? Zumdahl refers to “apparent” units in places, I prefer to stick with the “true” no-unit version. • Calculations involving the equilibrium constant, K • Know how to calculate the equilibrium constant if given equi- librium amounts of reactants and products. This is where you are given the entire bottom row “e” (final equilibrium con- centrations) of the equilibrium table (ICE Table) that we use. • Know how to calculate the equilibrium constant if given ini- tial concentrations and ONE f nal concentration at equilib- rium. This is where you are given only ONE of the bottom row concentrations of your equilibrium table. • Know how to calculate f nal (equilibrium) concentrations if given initial concentrations and the value of K c or K p . This is the typical type problem where you must set up and solve the equilibrium expression for x . Your entire bottom row will be lots of concentration formulas containing x . • Know how to predict the direction of a reaction if given con- centrations and a value for K . (hint: compare Q to K ) • Know how to predict how equilibrium shifts (L, R, NC) when a system is stressed. What are stresses? ANYTHING that takes a system OUT of equilibrium. This are typically con-
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 03/24/2011 for the course CHEMISTRY 302 taught by Professor Vanden bout during the Spring '11 term at University of Texas at Austin.

Page1 / 3

Review2s10 - Dr McCord CH302 REVIEW for EXAM 2 Spring 2010 page 1 Textbook Chapters for Exam 2 All of Chapters 6 and 7 PLUS remember Chapter 10

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online