Suppose a 500. mL flask is filled with 1.0 mol of CO, 1.8 mol of CO₂ and 0.90 mol of H₂. The following reaction becomes possibl CO(g) + H₂O(g) + CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.932 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places. M X
Suppose a 500. mL flask is filled with 1.0 mol of CO, 1.8 mol of CO₂ and 0.90 mol of H₂. The following reaction becomes possibl CO(g) + H₂O(g) + CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.932 at the temperature of the flask. Calculate the equilibrium molarity of CO2. Round your answer to two decimal places. M X
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 61QRT
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Step 1
Given equilibrium is
CO(g) + H2O(g) ⇄ CO2(g) + H2(g)
Initial moles of CO = 1.0 mol
Initial moles of CO2 = 1.8 mol
Initial moles of H2 = 0.90 mol
Equilibrium constant , K = 0.932
Volume of flask = 500. mL = 0.500 L
Equilibrium molarity of CO2 = ?
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