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.
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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.
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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