1. Chapter 15: Chemical Equilibria

7. Manipulating Equilibrium Expressions : N 2 (g) + 3 H 2 (g)  2 NH 3 (g) K = =5.5 x 10 5 Reversing Reactions Multiplying by a Factor

10. Given these initial concentrations, what will the final concentrations be when equilibrium is reached?

11. Given these initial concentrations, what will the final concentrations be when equilibrium is reached?

12. K in terms of pressure: K p vs. K c K p = K c (RT)  n  n = change in numbers of moles of gas 2 NH 3 (g) ==== N 2 (g) + 3 H 2 (g) K c = 5.8 x 10 5 K p = ------------- =

17. LeChatelier’s Principle: Doing the math 1-Liter flask contains 0.50 mol butane and 1.25 mol isobutane (at equilibrium). 0.50 mol butane are added. What happens, and what is the result?