Suppose a 500, mL, flask is filled with 1.9 mol of H and 1.6 mol of HI. The following reaction becomes possible: H2(g) + I2(g) ~ 2HI (p) The equilibrium constant K for this reaction is 6.54 at the temperature of the flask. Calculate the equilibrium molarity of I2, Round your answer to two decimal places.
Suppose a 500, mL, flask is filled with 1.9 mol of H and 1.6 mol of HI. The following reaction becomes possible: H2(g) + I2(g) ~ 2HI (p) The equilibrium constant K for this reaction is 6.54 at the temperature of the flask. Calculate the equilibrium molarity of I2, 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 1.9 mol of H and 1.6 mol of HI. The following reaction becomes possible:
H2(g) + I2(g) ~ 2HI (p)
The equilibrium constant K for this reaction is 6.54 at the temperature of the flask.
Calculate the equilibrium molarity of I2, Round your answer to two decimal places.
![Suppose a 500. mL flask is filled with 1.9 mol of H, and 1.6 mol of HI. The following reaction becomes possible:
H, (g) +I,(g) - 2HI(g)
The equilibrium constant K for this reaction is 6.54 at the temperature of the flask.
Calculate the equilibrium molarity of L. Round your answer to two decimal places.
) M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3f1fd93d-5095-4c3a-92a6-9fc6ee5d6acd%2F823992df-bd32-4cf5-b007-101594e3c962%2Fp85k592_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Suppose a 500. mL flask is filled with 1.9 mol of H, and 1.6 mol of HI. The following reaction becomes possible:
H, (g) +I,(g) - 2HI(g)
The equilibrium constant K for this reaction is 6.54 at the temperature of the flask.
Calculate the equilibrium molarity of L. Round your answer to two decimal places.
) M
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