(1) Consider the reaction: 2 H₂S (g) 2 H₂(g) + S₂(g) Kp = 2.4 x 10-4 at 1073 K A 2.0 L reaction vessel contains 0.112 mol H2, 0.055 mol S2, and 0.0445 mol H₂S. Answer the following questions. (a) What is the value of the equilibrium constant in terms of concentration? (b) Is this reaction at equilibrium? (c) If this reaction is not at equilibrium, which direction will the reaction proceed?
(1) Consider the reaction: 2 H₂S (g) 2 H₂(g) + S₂(g) Kp = 2.4 x 10-4 at 1073 K A 2.0 L reaction vessel contains 0.112 mol H2, 0.055 mol S2, and 0.0445 mol H₂S. Answer the following questions. (a) What is the value of the equilibrium constant in terms of concentration? (b) Is this reaction at equilibrium? (c) If this reaction is not at equilibrium, which direction will the reaction proceed?
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 61QRT
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![(1) Consider the reaction:
2 H₂S (g) = 2 H₂(g) + S₂(g)
A 2.0 L reaction vessel contains 0.112 mol H₂, 0.055 mol S2, and 0.0445 mol H₂S. Answer the
following questions.
Kp
= 2.4 x 10-4 at 1073 K
(a) What is the value of the equilibrium constant in terms of concentration?
(b) Is this reaction at equilibrium?
(c) If this reaction is not at equilibrium, which direction will the reaction proceed?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F02f21440-87e1-46d9-bb91-8d3e692a5753%2F83328f75-5d0e-44fa-bdda-702b73468f30%2Fdtkejv_processed.jpeg&w=3840&q=75)
Transcribed Image Text:(1) Consider the reaction:
2 H₂S (g) = 2 H₂(g) + S₂(g)
A 2.0 L reaction vessel contains 0.112 mol H₂, 0.055 mol S2, and 0.0445 mol H₂S. Answer the
following questions.
Kp
= 2.4 x 10-4 at 1073 K
(a) What is the value of the equilibrium constant in terms of concentration?
(b) Is this reaction at equilibrium?
(c) If this reaction is not at equilibrium, which direction will the reaction proceed?
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