At 1000 K, a sample of pure NO₂ gas decomposes:22NO₂(g) = 2NO(g) + O₂(g)The equilibrium constant Kp, is 158. Analysis shows that the partial pressure of O₂ is 0.41 atm at equilibrium.Part 1 of 2What is the pressure of NO? Be sure your answer has the correct number of significant digits.Part 2 of 2atmx10atmXWhat is the pressure of NO₂? Be sure your answer has the correct number of significant digits.Śx10

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Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

At 1000 K, a sample of pure NO₂ gas decomposes:
2
2NO₂(g) = 2NO(g) + O₂(g)
The equilibrium constant Kp, is 158. Analysis shows that the partial pressure of O₂ is 0.41 atm at equilibrium.
Part 1 of 2
What is the pressure of NO? Be sure your answer has the correct number of significant digits.
Part 2 of 2
atm
x10
atm
X
What is the pressure of NO₂? Be sure your answer has the correct number of significant digits.
Ś
x10

Expert Solution

Step 1

The equilibrium constant is the ratio of the pressure of products to the pressure of reactants, each raised to the power their stoichiometric coefficient.

Given that:

Partial pressure of O₂ at equilibrium= 0.41 atm

K_P = 158

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