3. Consider the reaction Br2 (g) + Cl2 (9) 2 BrCl (g) Kp = 1.11 x 10 at 150 K. A reaction mixture initially contains a Br₂ partial pressure of 0.993 atm and a Cl₂ partial pressure of 0.967 atm at 150 K. Calculate the equilibrium partial pressure of each reactant and product. 4. Consider the reaction CO (g) + H₂O (g) CO₂ (g) + H₂ (g) A reaction mixture initially contains a CO partial pressure of 1.768 atm and a H₂O partial pressure of 2.324 atm at 2000 K. Calculate the equilibrium partial pressures of each reactant and product. p= 0.0611 at 2000K.
3. Consider the reaction Br2 (g) + Cl2 (9) 2 BrCl (g) Kp = 1.11 x 10 at 150 K. A reaction mixture initially contains a Br₂ partial pressure of 0.993 atm and a Cl₂ partial pressure of 0.967 atm at 150 K. Calculate the equilibrium partial pressure of each reactant and product. 4. Consider the reaction CO (g) + H₂O (g) CO₂ (g) + H₂ (g) A reaction mixture initially contains a CO partial pressure of 1.768 atm and a H₂O partial pressure of 2.324 atm at 2000 K. Calculate the equilibrium partial pressures of each reactant and product. p= 0.0611 at 2000K.
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 56QAP: Sulfur oxychloride, SO2Cl2, decomposes to sulfur dioxide and chlorine gases. SO2Cl2(g)SO2(g)+Cl2(g)...
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Transcribed Image Text:3. Consider the reaction
Br2 (g) + Cl2 (g)
2 BrCl (g)
Kp = 1.11 x 104 at 150 K.
A reaction mixture initially contains a Br2 partial pressure of 0.993 atm and a Cl2 partial pressure of
0.967 atm at 150 K. Calculate the equilibrium partial pressure of each reactant and product.
4. Consider the reaction
CO₂ (g) + H2 (g)
A reaction mixture initially contains a CO partial pressure of 1.768 atm and a H₂O partial pressure
of 2.324 atm at 2000 K. Calculate the equilibrium partial pressures of each reactant and product.
CO (g) + H₂O (g)
Kp = 0.0611 at 2000K.
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