Suppose a 500. mL flask is filled with 0.70 mol of H:0, 0.60 mol of CO2 and 1.5 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO:(g) + H₂(g) The equilibrium constant K for this reaction is 0.441 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M S V Suppose a 500. ml. flask filled with 0.70 mol of H₂O, 0.60 mol of CO₂, and 1.5 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.441 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M X 3 5
Suppose a 500. mL flask is filled with 0.70 mol of H:0, 0.60 mol of CO2 and 1.5 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO:(g) + H₂(g) The equilibrium constant K for this reaction is 0.441 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M S V Suppose a 500. ml. flask filled with 0.70 mol of H₂O, 0.60 mol of CO₂, and 1.5 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) + CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 0.441 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M X 3 5
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 62QRT
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![Suppose a 500. mL flask is filled with 0.70 mol of H₂O, 0.60 mol of CO2 and 1.5 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The
equilibrium constant K for this reaction is 0.441 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M S
V
M
3
Suppose a 500. mL. flask is filled with 0.70 mol of H₂O, 0.60 mol of CO₂ and 1.5 mol of H₂. The following reaction becomes possible:
CO(g) + H₂O(g) CO₂(g) + H₂(g)
The equilibrium constant X for this reaction is 0.441 at the temperature of the flask.
Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places.
3
Ć](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc284736a-ec13-4483-9a71-a221e8520063%2F860f11f2-3dc6-484d-8e0d-20e8453c0cd3%2F4ox1ag_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Suppose a 500. mL flask is filled with 0.70 mol of H₂O, 0.60 mol of CO2 and 1.5 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The
equilibrium constant K for this reaction is 0.441 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M S
V
M
3
Suppose a 500. mL. flask is filled with 0.70 mol of H₂O, 0.60 mol of CO₂ and 1.5 mol of H₂. The following reaction becomes possible:
CO(g) + H₂O(g) CO₂(g) + H₂(g)
The equilibrium constant X for this reaction is 0.441 at the temperature of the flask.
Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places.
3
Ć
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