[starter]

This is my first post so hopefully this goes well.
Thanks in advance for any help.

At 100oC, the equilibrium constant for the reaction COCl2(g)  CO(g) + Cl2 has a value of 2.19 x 10-10. Is the following mixture at equilibrium? If not, indicate the direction in which the reaction must proceed to achieve equilibrium.

[COCl2] = 5.00 x 10-2 M, [CO] = [Cl2] = 3.31 x 10-6 M

a. yes, the system is already at equilibrium 
b. no, the forward reaction is favored 
c. no, the reverse reaction is favored

The Haber-Bosch Process, used to produce NH3, is governed by the following equilibrium, which has an equilibrium constant of K=9.6 at 573K:

N2(g) + 3H2(g) 2NH3(g)

The concentrations of the gases at a given point in time are:
[NH3] = 10 moles/l
[N2] = 3 moles/l
[H2] = 2 moles/l

Which of the following statements are TRUE, with respect to these conditions?

a. The expression for K is [NH3]2/[N2][H2]3 
b. The value of Q is greater than K, and the reaction tends to the left to achieve equilibrium. 
c. The addition of a catalyst will shift the equilibrium in favour of the formation of products. 
d. The product of this reaction is an important component of many fertilizers and explosives. 
e. Extensive fertilization results in a shift in the the coupled equilibria of the Nitrogen Biogeochemical Cycle, driving into run off rivers, lakes, and oceans. This is a major factor behind the plume of algae growth, in the Gulf of Mexico. 

For the first question i forgot how i would know if the reaction is at equilibrium, its been a while since my last chemistry class and for the second question i know that a catalyst would have no affect due to Chatelier's so that means c is wrong, i know that ammonia is used in fertilers and explosives so d is correct. The thing that confuses me is the concetration of the gases at any given point wether or not that is incorperacted into the K equation. Any help would be good. Thanks

[Yggdrasil]

Reading about equilibrium constants in your chemistry text book or on wikipedia (http://en.wikipedia.org/wiki/Equilibrium_constant) should help you answer your questions.