Suppose a 250. mL flask is filled with 1.9 mol of Cl₂ and 0.10 mol of HCl. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl(g) The equilibrium constant K for this reaction is 0.856 at the temperature of the flask. Calculate the equilibrium molarity of HC1. Round your answer to two decimal places. M X
Suppose a 250. mL flask is filled with 1.9 mol of Cl₂ and 0.10 mol of HCl. The following reaction becomes possible: H₂(g) + Cl₂(g) → 2HCl(g) The equilibrium constant K for this reaction is 0.856 at the temperature of the flask. Calculate the equilibrium molarity of HC1. 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 62QRT
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![O KINETICS AND EQUILIBRIUM
Calculating equilibrium composition from an equilibrium constant
Suppose a 250. mL flask is filled with 1.9 mol of Cl₂ and 0.10 mol of HCl. The following reaction becomes possible:
H₂(g) + Cl₂(g) → 2HCl(g)
The equilibrium constant K for this reaction is 0.856 at the temperature of the flask.
Calculate the equilibrium molarity of HC1. Round your answer to two decimal places.
M
X](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe6263ceb-2148-4d04-a273-847311b190a4%2F8f7c4657-9754-404e-80b7-1773bf758157%2Fimos4lh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:O KINETICS AND EQUILIBRIUM
Calculating equilibrium composition from an equilibrium constant
Suppose a 250. mL flask is filled with 1.9 mol of Cl₂ and 0.10 mol of HCl. The following reaction becomes possible:
H₂(g) + Cl₂(g) → 2HCl(g)
The equilibrium constant K for this reaction is 0.856 at the temperature of the flask.
Calculate the equilibrium molarity of HC1. Round your answer to two decimal places.
M
X
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