[cmquer]

1.FeO (s) + CO (g) <-- --> Fe (s) + CO2  (g)

Kp = 0.403 at 1000°C

What are the equilibrium partial pressures of CO (g) and CO2 (g) when 1.00atm of CO (g) and excess FeO (s) react in a sealed container at 1000°C?

2.A reaction is of the type: A (g) + B (g) <-- --> C (g). An unmeasured quantity of C is introduced into a 1.0dm3 container and is allowed to come to equilibrium. At this time a sample is analysed and found to be 1.0M in C. If under the conditions of the experiment the equilibrium constant Kc is 1.0 x 10^6 mol-1 dm3, what is the equilibrium concentration (in M) of B?

3.for the following equilibrium system, which of the changes will form more CaCO3?
      CO2 (g) + Ca(OH)2 (s) <-- --> CaCO3 (s) + H2O (l)  △H°=-113kJ
(a) Decrease temperature at constant pressure (no phase change)
(b) Increase volume at constant temperature
(c) Increase partial pressure of CO2
(d) Remove one-half of the initial CaCO3


Can anyone help?
THANK YOU.

[Yggdrasil]

Please read the Forum Rules.  You should that show you've at least attempted to answer the problem before we will help you.  However, I will give you some hints:

1)  Start with the expression for K_p in terms of the partial pressures of the reactants and products.

2)  This one is a bit tricky.  Try using an ICE table.  Or, from the reaction stoichiometry, what do you know about the concentrations of A and B?

3)  Think about Le Chatelier's principle.