Chemical Equlibrium Question I am not sure about.?

[匿名]

2017-01-20 3:53 pm

更新1:

"Nitrogen Dioxide decomposes to nitric oxide and oxygen gas. When a flask initially containing pure NO2 at 0.500 ATM comes to equilibrium, the total pressure in the flask is 0.732 ATM. Calculate P(NO) at equilibrium and value of Kp for the reaction. The Kp expression and an 'ice' table are required." Formula: 2NO2(g) <--> 2NO(g) + O2(g) Thanks

更新2:

回答 (1)

wanszeto

2017-01-20 5:20 pm

✔ 最佳答案

Let y atm be the partial pressure of NO₂ reacted in establishment of reaction.

___________2NO₂(g) ⇌ 2NO(g) + O₂(g)
Initial: ___ 0.500 atm __0 atm __0 atm
change: ___ -y atm__ +y atm _ +(1/2)y atm
At eqm: (0.500-y) atm _y atm __ (1/2)y atm

Total pressure at equilibrium:
P(NO₂) + P(NO) + P(O₂) = 0.732 atm
(0.500 - y) + y + (1/2)y = 0.732
(1/2)y = 0.232
y = 0.464

Hence, P(NO) = 0.464 atm

Kp = [NO]² [O₂] / [NO₂]² = 0.464² × 0.232 / (0.500 - 0.464)² = 1.39 (to 3 sig. fig.)

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