Suppose a 500. mL flask is filled with 1.9 mol of CO, 0.60 mol of H₂O and 1.7 mol of H₂. The following reaction becomes possible:CO (g) + H₂O(g) → CO₂(g) + H₂ ((g)2The equilibrium constant K for this reaction is 1.81 at the temperature of the flask.Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places.2MXŚ?

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Suppose a 500. mL flask is filled with 1.9 mol of CO, 0.60 mol of H₂O and 1.7 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 1.81 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M X S

Suppose a 500. mL flask is filled with 1.9 mol of CO, 0.60 mol of H₂O and 1.7 mol of H₂. The following reaction becomes possible: CO(g) + H₂O(g) → CO₂(g) + H₂(g) The equilibrium constant K for this reaction is 1.81 at the temperature of the flask. Calculate the equilibrium molarity of H₂O. Round your answer to two decimal places. M X S

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 60QRT

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