At 2273K, equilibrium constant for the reaction

Question

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?

Answer 1

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

Answer 2

yes I did, but im still not getting the right answer.

I got .1136 which is not the correct answer.

Answer 3

what do you have for
initial:

change:

equilibrium

Answer 4

2NO <-> N2 O2
initial .116 0 0
change -x +x +x
equil .116-x x x

Answer 5

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.

Answer 6

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.

Answer 7

yes, I figured that one out. Thanks so much for the help!

Answer 8

that works! thank you so much!!

Answer 9

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