Name:
1. Neither PbCl2 nor PbF2 is appreciably soluble in water. If solid PbCl2 and solid PbF2 are placed in equal amounts of water in separate beakers, in which beaker is the concentration of Pb+2 ions greater?
Equilibrium constants are: Keq for PbCl2 is 1.7 x 10-5 and Keq for PbF2 is 3.7 x 10-8
2. The decomposition of calcium carbonate CaCO3 <--> CaS + CO2 is an endothermic process. Using LeChatelier's Principle, explain:
(a) how increasing the temperature would affect the equilibrium.
(b) If more CaCO3 is added to the flask in which the equilibrium exits.
(c) Additional CO2 is added tot he flask.
3. Do question number 8 (page 683) on paper.
4. K = 5.6 x 10-12 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) <--> 2I(g). A mixture has [I2] = 0.020 mol/L and [I] = 2.0 x 10-8 mol/L. Is the reaction at equilibrium? Select One Yes No If no, in which direction must the reaction shift in order to regain equilibrium? has [I2] = 0.020 mol/L and [I] = 2.0 x 10-8 mol/L. Is the reaction at equilibrium? Select One To the left producing more reactants To the right producing more products
5. The reaction PCl5(g) <--> PCl3(g) + Cl2(g) was examined at 250 oC. At equilibrium [PCl5] = 4.2 x 10-5 mol/L, [PCl3] = 1.3 x10-2 mol/L, and [Cl2] = 3.9 x 10-3 mol/L. Calculate K for this reaction.
6. A mixture of CO and Cl2 is placed into a reaction flask: [CO] = 0.0102 mol/L and [Cl2] = 0.00609 mol/L. When the reaction CO(g) + Cl2 <-> COCl2(g) has come to equilibrium at 600 K, [Cl2] = 0.0030 mol/L. (a) Calculate the concentrations of CO and COCl2 at equilibrium. (b) Calculate K
7. Do number 20 in the textbook.
8. Do number 26 in the textbook.
9. Do number 30 in the textbook.
10. Do number 32 in the textbook.
