Suppose a 500. mL flask is filled with 2.0 mol of H₂ and 1.1 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g): 2HI(g) The equilibrium constant K for this reaction is 8.57 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
Suppose a 500. mL flask is filled with 2.0 mol of H₂ and 1.1 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g): 2HI(g) The equilibrium constant K for this reaction is 8.57 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
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 10QRT
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![Suppose a 500. mL flask is filled with 2.0 mol of H₂ and 1.1 mol of HI. The following reaction becomes possible:
H₂(g) +1₂(g) → 2HI(g)
The equilibrium constant K for this reaction is 8.57 at the temperature of the flask.
Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5baeb348-f2b1-4f74-ae31-a382a1308bdc%2F104bddf7-36a2-4428-b92f-039cc0f4aeb3%2F4x30re_processed.png&w=3840&q=75)
Transcribed Image Text:Suppose a 500. mL flask is filled with 2.0 mol of H₂ and 1.1 mol of HI. The following reaction becomes possible:
H₂(g) +1₂(g) → 2HI(g)
The equilibrium constant K for this reaction is 8.57 at the temperature of the flask.
Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
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