Chapter 17

Chapter 17 - Chapter 17: Chemical Equilibrium Basic...

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

View Full Document Right Arrow Icon
Chapter 17: Chemical Equilibrium Basic Concepts -reversible reactions do not go to completion -they can occur in either direction -symbolically, this is represented as: aA (g) + bB (g) →←cC (g) + dD (g) -mixture is dynamic equilibrium -Chemical equilibrium exists when two opposing reactions occur simultaneously at the same rate -chemical equilibria are dynamic equilibria -molecules are continually reacting, even though the overall composition of the reaction mixture does not change -one example of a dynamic equilibrium can be shown using radioactive 131 I as a tracer in a saturated PbI 2 solution -simple one-step mechanism A (g) + B (g) →← C (g) + D (g) Rate f = k f [A][B] represents the forward rate Rate r = k f [C][D] represents the reverse rate Rate f = rate r The equilibrium constant: k f /k r =K c = [C][D]/[A][B] General reaction aA (g) + bB (g) →←cC (g) + dD (g) K c = [C] c [D] d /[A] a [B] b Products/reactants Less than 1, greater than 0 = fair number of reactants, very few products
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 10/04/2011 for the course CHEM 1212 taught by Professor Suggs during the Spring '08 term at UGA.

Page1 / 2

Chapter 17 - Chapter 17: Chemical Equilibrium Basic...

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