gen chem
posted by Chem on .
At 2273K, equilibrium constant for the reaction
2NO(g)<>N2(g)+O2(g)
Kc=2.4x10^3
What would be equilibrim concentration of N2, if initial concentration of NO was 0.1160M?

Have you tried setting up an ICE chart? That's the obvious way to go.

yes I did, but im still not getting the right answer.
I got .1136 which is not the correct answer. 
what do you have for
initial:
change:
equilibrium 
2NO <> N2 O2
initial .116 0 0
change x +x +x
equil .116x x x 
Did you look at your post from last night where we arrived at K = something x 10^192? That problem didn't ask for K, it asked for pK. I'll get back on the current problem.

Make it
initial:
NO = 0.1160
N2 = 0
O2 = 0
change:
NO = 2x
N2 = x
O2 = x
equilibrium:
NO = 0.1160  2x
N2 = x
O2 = x
and solve for x. 
yes, I figured that one out. Thanks so much for the help!

that works! thank you so much!!

I'm curious about the problem last night. Was the pK about 192?