A flask that initially contained pure NO₂ was heated to 1000 K, a temperature at which the value of Kp for the decomposition of NO₂ is 167.8. 2NO₂(g) <-----> 2NO(g) + O₂(g) Given that the partial pressure of O₂ at equilibrium equals 0.121 atm calculate the partial pressures of NO₂ and NO at equilibrium. PNO=PNO₂= =

A flask that initially contained pure NO₂ was heated to 1000 K, a temperature at which the value of Kp for the decomposition of NO₂ is 167.8. 2NO₂(g) <-----> 2NO(g) + O₂(g) Given that the partial pressure of O₂ at equilibrium equals 0.121 atm calculate the partial pressures of NO₂ and NO at equilibrium. PNO=PNO₂= =

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 54QAP: Consider the following hypothetical reaction: X2(g)+R(s)X2R(g) R has a molar mass of 73 g/mol. When...

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