Calculate the Ko for this reaction at 500 K. gases has partial pressures of 0.095 atm, 0.171 atm and 0.28 atm for NO, Cl2 and NOCI, respectively. equilibrium 2 NOg) + Cl2g) 2 NOClig) is established at 500 K. An equilibrium mixture of the three Answer: Kp = 51

Calculate the Ko for this reaction at 500 K. gases has partial pressures of 0.095 atm, 0.171 atm and 0.28 atm for NO, Cl2 and NOCI, respectively. equilibrium 2 NOg) + Cl2g) 2 NOClig) is established at 500 K. An equilibrium mixture of the three Answer: Kp = 51

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

Provide a solution using the given answer.

The equilibrium 2 NOg)
gases
equilibrium 2 NO(g) + Cl2(g) 2 NOCI9) is established at 500 K. An equilibrium mixture of the three
bas partial pressures of 0.095 atm, 0.171 atm and 0.28 atm for NO, Cl2 and NOCI, respectively.
Calculate the Kp for this reaction at 500 K.
gases has partial pressures of 0.095 atm, 0.171 atm and 0.28 atm for NO, Cl2 and NOCI, respectively.
Answer: Kp = 51
phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas: PCl3tg) + Clzg)
PCI5(g). A gas vessel is charged with a mixture of PCIą and Cl2 which is allowed to equilibrate at 450 K.
At equilibrium, the partial pressures of the three gases are What is the value of Kp at this temperature?
Answer: K, = 66.8
%3D

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