1. Consider the reaction 2 NO (g) 2 NOBr (g) Kp = 28.4 at 298 K. In a reaction mixture at equilibrium, the partial pressure of NO is 0.142 atm and Br2 is 0.166 atm. What is the partial pressure of NOBr in this mixture? 2. Consider the reaction SO₂Cl2 (9) Kp = 2.91 x 10³ at 298 K. + Br₂ (g) SO₂ (g) + Cl2 (g) In a reaction at equilibrium, the partial pressure of SO₂ is 0.180 atm and that of Cl₂ is 0.375 atm. What is the partial pressure of SO₂Cl2 in this mixture?

1. Consider the reaction 2 NO (g) 2 NOBr (g) Kp = 28.4 at 298 K. In a reaction mixture at equilibrium, the partial pressure of NO is 0.142 atm and Br2 is 0.166 atm. What is the partial pressure of NOBr in this mixture? 2. Consider the reaction SO₂Cl2 (9) Kp = 2.91 x 10³ at 298 K. + Br₂ (g) SO₂ (g) + Cl2 (g) In a reaction at equilibrium, the partial pressure of SO₂ is 0.180 atm and that of Cl₂ is 0.375 atm. What is the partial pressure of SO₂Cl2 in this mixture?

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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