1. Chemical Equilibrium: Keq 2H 2 S(g)  2H 2 (g) + S 2 (g) At 1130 o C the following equilibrium concentrations are as follows: H 2 S = 0.15 M; H 2 = 0.01 M; S 2 = 0.051 M. Calculate K eq.

2. Chemical Equilibrium: Keq H 2 (g) + I 2 (g)  2HI(g) What is the equilibrium concentration of HI for the above reaction given the following information: H 2 (g) equilibrium conc. = 2.0M; I 2 (g) equilibrium conc. = 3.0M; K eq =51

3. Chemical Equilibrium: Keq At 900 K, a 4.00 L reaction vessel originally contained 0.55 mols SO 3 (g). Once equilibrium was reached, 0.12 mols of O 2 (g) was made. Calculate the K eq given the following equation: 2SO 3 (g)  2SO 2 (g) + O 2 (g)

4. Chemical Equilibrium: Keq A 1.00 M sample of HI is heated in a sealed container to 510 o C. At equilibrium, a 0.14 M concentration of each of the products (H 2 & I 2 ) is present. Calculate the K eq.

5. Chemical Equilibrium: Keq At 500 K, a 1.00 L reaction vessel originally contained 0.045 mols NO 2 (g). Once equilibrium was reached, 0.0020 mols of O 2 (g) was made. Calculate the K eq given the following equation: 2NO 2 (g)  2NO(g) + O 2 (g)

6. Shifts: Le Chatelier The following system is in equilibrium: Heat + 2NH 3 (g)  N 2 (g) + 3H 2 (g) 1. If more N 2 (g) were added, what effect on the equilibrium would there be? 2. If H 2 (g) could be selectively removed from the system, what effect would there be on the equilibrium ?

7. Le Chatelier For the system 2 SO 2 (g) + O 2 (g)  2 SO 3 (g), Predict the effect of each of the following changes on the value of the equilibrium constant and on the number of moles of SO 3 present in the mixture at equilibrium. (a)Decreasing the volume of the system. (b)Adding oxygen to the equilibrium mixture. (c)Raising the temperature of the system.

8. Le Chatelier C(s) + H 2 O(g)  CO(g) + H 2 (g)  H o = +131 kJ 1.Additional H 2 (g) is added. 2.The temperature of the system is increased. 3.The volume of the container is decreased. 4. The graphite pellets are pulverized

9. Solubility Product: Ksp At 25 o C, a saturated solution of calcium hydroxide has a concentration of 0.0126 M. Calculate the K sp.

10. Solubility Product: Ksp The solubility of calcium sulfate is found to be 0.67 grams per liter of solution. Calculate the K sp.

11. Solubility Product: Ksp The K sp for silver carbonate is 8.1 x 10 -12 at 25 o C. Calculate the molar solubility of this substance at this temperature.

12. Solubility Product: Ksp Solid calcium nitrate is added to a 100.0 ml solution of 0.10 M KF until the reaction stops. How many grams of solid CaF 2 is produced and what is the molar solubility of the of CaF 2 (Ksp = 3.9 x 10 -11 )

13. Solubility Product: Ksp At 25 o C, the K sp of silver carbonate, Ag 2 CO 3 is 8.1 x 10 -12. Calculate the molar concentrations of silver and carbonate ions at this temperature.

14. Solubility Product: Ksp a) At 25 degrees the Ksp of magnesium carbonate (MgCO 3 ) is 3.60 X 10 -8. Calculate the molar concentration of Magnesium ions present in a saturated solution at this temperature. b) If you were asked to prepare a solution of this substance at this temp. by dissolving 0.240 grams MgCO 3 into 10.0 L, would all the solute dissolve? If not, how much (in grams) would be left undissolved?

15. Solubility Product: Ksp If 0.01 L of a 0.00825 M solution of Na 2 SO 4 is added to 0.29 L of a 0.00125 M solution of CaCl 2, will a CaSO 4 precipiate form, and if so how much? The K sp for CaSO 4 = 1.7 x 10 -8