Suppose a 250. mL flask is filled with 1.4 mol of I, and 2.0 mol of HI. The following reaction becomes possible: (3)°1 +(3)H 2HI(g) The equilibrium constant K for this reaction is 6.67 at the temperature of the flask. Calculate the equilibrium molarity of H,. Round your answer to two decimal places.
Suppose a 250. mL flask is filled with 1.4 mol of I, and 2.0 mol of HI. The following reaction becomes possible: (3)°1 +(3)H 2HI(g) The equilibrium constant K for this reaction is 6.67 at the temperature of the flask. Calculate the equilibrium molarity of H,. 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 250. mL flask is filled with 1.4 mol of I, and 2.0 mol of HI. The following reaction becomes possible:
H, (g) +I, (g) = 2HI (g)
The equilibrium constant K for this reaction is 6.67 at the temperature of the flask.
Calculate the equilibrium molarity of H,. Round your answer to two decimal places.
) M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F55f2574c-3119-4c10-8286-127ea34ab802%2F0abc166e-10f1-4b13-a5c1-1102a6433c78%2F1wxtdq1d_processed.png&w=3840&q=75)
Transcribed Image Text:Suppose a 250. mL flask is filled with 1.4 mol of I, and 2.0 mol of HI. The following reaction becomes possible:
H, (g) +I, (g) = 2HI (g)
The equilibrium constant K for this reaction is 6.67 at the temperature of the flask.
Calculate the equilibrium molarity of H,. Round your answer to two decimal places.
) M
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