3. At 2200 °C, Kp = 0.0500 for the following reaction: N2(g) + O2(g) → 2 NO(g). Quantify the partial pressure of NO that is present at equilibrium after initially N₂ and 0₂ were placed in the flask with initial pressures of 0.888 atm N2 and 0.222 atm 02.
3. At 2200 °C, Kp = 0.0500 for the following reaction: N2(g) + O2(g) → 2 NO(g). Quantify the partial pressure of NO that is present at equilibrium after initially N₂ and 0₂ were placed in the flask with initial pressures of 0.888 atm N2 and 0.222 atm 02.
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter13: Fundamental Equilibrium Concepts
Section: Chapter Questions
Problem 57E: Calculate the value of the equilibrium constant Kp for the reaction 2NO2(g)+Cl2(g)2NOCl(g) from...
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Expert Solution
Step 1
N2 + O2 <=> 2NO
initial pressures
0.80....0.20
at equilibrium
0.80-x. . . 0.20-x. . .. 2x
0.050 = (2x)^2 / (0.80-x) ( 0.20 -x)
So, x = 0.0391
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