At 1000 K, a sample of pure NO2 gas decomposes:
2NO2 (g) > 2NO (g) + O2 (g)
The equilibrium constant Kp is 158. Analysis shows that the partial pressure of O2 is 0.25 atm at equilibrium. Calculate the pressure of NO and NO2 in the mixture.
THANK YOU VERY MUCH!
2007-03-05 23:28:15 · 3 answers · asked by -three31one- 1 in Science & Mathematics ➔ Chemistry
2NO2 (g) > 2NO (g) + O2 (g)
the arrow (>) in the original look, it is upside down. with a arrow pointing to the right and left, upside down. got my point?
2007-03-05 23:30:21 · update #1
I got 1.93 for the NO2 and 1.68 for the NO.
I'm too lazy to type out the steps.
2007-03-05 23:44:46 · answer #1 · answered by chris m 1 · 0⤊ 1⤋
If pure NO2 decomposes according to the reaction, then the partial pressure of NO should be twice that of O2, or 0.50 atm. To find NO2, you need to use the Kp equation.
158 = P(NO)^2 * P(O2)/ P(NO2)^2
P(NO2)^2 = 0.50^2 * 0.25/158 = 0.000396
P(NO2) = 0.0198 ~ 0.02 atm
2007-03-06 01:12:13 · answer #2 · answered by TheOnlyBeldin 7 · 0⤊ 0⤋
2X0,25=NO and same next one
2007-03-13 05:22:55 · answer #3 · answered by Anonymous · 0⤊ 0⤋