1.Select the items below which are equilibrium processes.

a) Water evaporating and condensing in a closed container.

b) CO₂ in a closed can of soda.

c) Carbonate buffer system in blood.

2. Consider the reaction below. If the reaction were put on ice, what would happen?

N2()+2H2()N2H4() =95kJ

a) No shift would occur

b) Make more N₂ and H₂

c) Make more N₂H₄

3. If there are no reactants remaining in the system, what is the value of Q?

a) zero

b) infinity

c) one

d) depends on the reaction

4. If a system is at equilibrium what is true?

a) Q > K

b) Q and K both equal 1

c) Q < K

d) Q = K

5. Consider the reaction below. If more gaseous carbon dioxide were added to a container at equilibiurm, what would be the relationship of Q with K?

CO₂ (g) + H₂O (l) <=> H₂CO₃ (aq)

a) Not enough information.

b) Q < K

c) Q > K

d) Q = K

6. The value of Q can be used to.... (Select all that apply)

a) determine where a reaction is in regards to reaching equilibrium.

b) determine the nonstandard value of G.

c) determine the value of K.

d) determine the enthalpy of the reaction.

7. If G is negative what is true about the value of K?

a) It will be smaller than one, reactants favored.

b) It will be smaller than one, products favored.

c) It will be larger than one, reactants favored.

d) It will be larger than one, products favored.

8. When calculating K, one must...

a) use initial concentrations.

b) use concentrations immediately after the reaction begins.

c) use equilibrium concentrations.

d) use concentrations at any point during the reaction.