CO (g) + H2O (g) <-> H2 (g) + CO2 (g) has K = 1.3 at 650 degrees C. Carbon monoxide and steam have initial partial pressures of .485 atm, while hydrogen and carbon dioxide have initial pressures of .300 atm. a) calculate the partial pressure of each gas at equilibrium Once the system has reached equilibrium, indicate whether each of the following actions would cause the reaction to go forward (to the right) or reverse (to the left), or have no effect. b) Add CO2 gas c) Add helium gas d) Remove H2 gas e) The pressure is decreased by increasing the volume
CO (g) + H2O (g) <-> H2 (g) + CO2 (g) has K = 1.3 at 650 degrees C. Carbon monoxide and steam have initial partial pressures of .485 atm, while hydrogen and carbon dioxide have initial pressures of .300 atm. a) calculate the partial pressure of each gas at equilibrium Once the system has reached equilibrium, indicate whether each of the following actions would cause the reaction to go forward (to the right) or reverse (to the left), or have no effect. b) Add CO2 gas c) Add helium gas d) Remove H2 gas e) The pressure is decreased by increasing the volume
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 41P
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For the reaction
CO (g) + H2O (g) <-> H2 (g) + CO2 (g) has K = 1.3 at 650 degrees C.
Carbon monoxide and steam have initial partial pressures of .485 atm, while hydrogen and carbon dioxide have initial pressures of .300 atm.
a) calculate the partial pressure of each gas at equilibrium
Once the system has reached equilibrium, indicate whether each of the following actions would cause the reaction to go forward (to the right) or reverse (to the left), or have no effect.
b) Add CO2 gas
c) Add helium gas
d) Remove H2 gas
e) The pressure is decreased by increasing the volume
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