1. Equilibrium Station Review

2. 1 How do you know if a reaction is reactant- or product-favored?
What is Le Chateleir’s Princlple?
How does flipping an equation change the value of K?
How do coefficients get used in equilibrium expressions?

3. 2
Ag2SO4 is considered slightly soluble and forms the following equilibrium when placed in water:
Ag2SO4(s)  2Ag+(aq) + SO42-(aq)
Ksp is known to be 1.5E-5 at 25 C. If some solid silver sulfate is added to a solution that is 0.15 M Ag+, what will the final concentration of sulfate ion be?
What is the solubility of silver sulfate (in grams per liter)?

4. 3
2CO(g)  CO2(g) + C(s)
Two grams of all substances are placed in an evacuated 2.0 L flask at 19 C.
Kc at 19 C is known to be 7.88E14. Which direction will the reaction proceed to reach equilibrium? Justify your answer.
What is Kc at 19 C for this reaction?
3CO2(g) + 3C(s)  6CO(g)

5. 4

6. 5
Write equilibrium expressions for the following: Ti(s) + 2Cl2(g)  TiCl4(l) 2C2H4(g) + 2H2O(g)  2C2H6(g) + O2(g) FeO(s) + H2(g)  Fe(s) + H2O(g) 4HCl(g) + O2(g)  2H2O(l) + 2Cl2(g)

7. 6 Use the following reaction: 2A(g) + B(l)  C(aq)
Write the equilibrium expression for Kp.
If A, at a pressure of 2.5 atm, and some B are placed in an evacuated chamber and the pressure of A at equilibrium is determined to be 1.5 atm, calculate Kp.

8. 7 When is K<O? When is K>1? When is K<1?
If a reaction is endothermic, how does increasing the temperature affect K? Will it increase, decrease, or stay the same? Explain.
You have initial values for all substances in a RICE table. How do you know which way a reaction will shift?

9. 8
For the system 2 SO2(g) + O2(g)  2 SO3(g) , H is negative for the production of SO3. Assume that one has an equilibrium mixture of these substances. Predict the effect of each of the following changes on the value of the equilibrium constant and on the number of moles of SO3 present in the mixture at equilibrium. Briefly account for each of your predictions. (Assume that in each case all other factors remain constant.) (a) Decreasing the volume of the system. (b) Adding oxygen to the equilibrium mixture. (c) Raising the temperature of the system.