Consider the equilibrium system described by the chemical reaction below. For this reaction, Kp = 109 at 298 K. If the equilibrium partial pressures of Br, and NOBr at 0.0159 atm and 0.0768 atm, respectively, determine the partial pressure of NO at equilibrium.. 2 NO(g) + Br2(g) =2 NOB1(g) 1 If (x) represents the equilibrium partial pressure of NO, set up the equilibrium expression for Kp to solve for the partial pressure. Do not combine or simplify terms.. Kp = = 109

Consider the equilibrium system described by the chemical reaction below. For this reaction, Kp = 109 at 298 K. If the equilibrium partial pressures of Br, and NOBr at 0.0159 atm and 0.0768 atm, respectively, determine the partial pressure of NO at equilibrium.. 2 NO(g) + Br2(g) =2 NOB1(g) 1 If (x) represents the equilibrium partial pressure of NO, set up the equilibrium expression for Kp to solve for the partial pressure. Do not combine or simplify terms.. Kp = = 109

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 89AP

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