Suppose a 250. mL flask is filled with 1.4 mol of H₂ and 1.5 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) The equilibrium constant K for this reaction is 0.310 at the temperature of the flask. Calculate the equilibrium molarity of H₂. Round your answer to two decimal places. M X
Suppose a 250. mL flask is filled with 1.4 mol of H₂ and 1.5 mol of HI. The following reaction becomes possible: H₂(g) +1₂(g) → 2HI(g) The equilibrium constant K for this reaction is 0.310 at the temperature of the flask. Calculate the equilibrium molarity of H₂. 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 10QRT
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![Suppose a 250. mL flask is filled with 1.4 mol of H₂ and 1.5 mol of HI. The following reaction becomes possible:
H₂(g) +1₂(g) → 2HI(g)
The equilibrium constant K for this reaction is 0.310 at the temperature of the flask.
Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
M
X](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4a877453-5cf6-4ba4-83fd-09eb44e95a97%2F9917d403-2cd4-4cd5-b4e8-79c637b2d82e%2F78cjhv_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Suppose a 250. mL flask is filled with 1.4 mol of H₂ and 1.5 mol of HI. The following reaction becomes possible:
H₂(g) +1₂(g) → 2HI(g)
The equilibrium constant K for this reaction is 0.310 at the temperature of the flask.
Calculate the equilibrium molarity of H₂. Round your answer to two decimal places.
M
X
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