For the reaction 2 NO₂(g) = 2 NO(g) + O₂(g) Kp = 1.11 × 10-5 at 200 °C. A 2.50 L vessel at 200 °C is filled with NO₂(g) at an initial pressure of 2.50 atm and allowed to come to equilibrium. What will be the pressure (in atm) of NO(g) at equilibrium?

For the reaction 2 NO₂(g) = 2 NO(g) + O₂(g) Kp = 1.11 × 10-5 at 200 °C. A 2.50 L vessel at 200 °C is filled with NO₂(g) at an initial pressure of 2.50 atm and allowed to come to equilibrium. What will be the pressure (in atm) of NO(g) at equilibrium?

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

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Question

For the reaction
2 NO2(g) = 2 NO(g) + O2(g)
Kp = 1.11 × 10-5 at 200 °C. A 2.50 L vessel at 200 °C is filled with
NO₂(g) at an initial pressure of 2.50 atm and allowed to come to
equilibrium. What will be the pressure (in atm) of NO(g) at equilibrium?

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