question: An equilibrium mixture contains
, (
0.27 
) and
(
1.2 ) at 350
. The volume of the container is doubled at constant temperature. Calculate the equilibrium pressure of both
and
when the new equilibrium is reached.
my solution so far: first of all i know the balanced reaction is N2O4 <--> 2NO2 and I know that when you double volume, you cut the pressure in half. le chatliers principle says that the reaction will then go to the right.
what im having problem with is the fact that I do not know nor am I given the Kp value so that I can create an equation using the ICE format. I believe the question should be set up like this:
N2O4: I = .27, C=-x, E = .27-x
NO2: I = 1.2, C = +2x, E = 1.2 + 2x
after that Im not sure what else I can do. please help. thanks.