Given the equation CH4 (g) + H2O (g) --> CO (g) + 3H2 (g). At 298K, take equilibrium constant K = 1.19x10^-25. At T=1004K, the equilibrium constant is 3.0. At 1004K, the initial partial pressure PCH4 = 30 atm, PH2O = 50 atm and equilibrium is reached at this temperature. After equilibrium is reached, what is the partial pressure and mole fraction of all components?
Given the equation CH4 (g) + H2O (g) --> CO (g) + 3H2 (g). At 298K, take equilibrium constant K = 1.19x10^-25. At T=1004K, the equilibrium constant is 3.0. At 1004K, the initial partial pressure PCH4 = 30 atm, PH2O = 50 atm and equilibrium is reached at this temperature. After equilibrium is reached, what is the partial pressure and mole fraction of all components?
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
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 15Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...
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Given the equation CH4 (g) + H2O (g) --> CO (g) + 3H2 (g). At 298K, take equilibrium constant K = 1.19x10^-25. At T=1004K, the equilibrium constant is 3.0. At 1004K, the initial partial pressure PCH4 = 30 atm, PH2O = 50 atm and equilibrium is reached at this temperature.
After equilibrium is reached, what is the partial pressure and mole fraction of all components?
please write correctly last time equation is not redable if possible write on paper
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