Consider the reaction shown below at room temperature. 2H2(g) + S2(g) ⇋ 2H2S(g) The equilibrium constant, K, is equal to 1.1 x 107. A mixture of reactants and products at room temperature contains 0.25 M H2, 0.15 M S2, and 0.50 M H2S. (a) Is this reaction at equilibrium? (b) In which direction does the reaction proceed to reach equilibrium? (c) Assuming the reactants remain at the same equilibrium concentrations, what would the concentration of the product have to be in order to establish equilibrium?
Consider the reaction shown below at room temperature. 2H2(g) + S2(g) ⇋ 2H2S(g) The equilibrium constant, K, is equal to 1.1 x 107. A mixture of reactants and products at room temperature contains 0.25 M H2, 0.15 M S2, and 0.50 M H2S. (a) Is this reaction at equilibrium? (b) In which direction does the reaction proceed to reach equilibrium? (c) Assuming the reactants remain at the same equilibrium concentrations, what would the concentration of the product have to be in order to establish equilibrium?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter13: Chemical Equilibrium
Section: Chapter Questions
Problem 15Q: Suppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this...
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Consider the reaction shown below at room temperature.
2H2(g) + S2(g) ⇋ 2H2S(g)
The equilibrium constant, K, is equal to 1.1 x 107. A mixture of reactants and products at room temperature contains 0.25 M H2, 0.15 M S2, and 0.50 M H2S.
(a) Is this reaction at equilibrium? (b) In which direction does the reaction proceed to reach equilibrium? (c) Assuming the reactants remain at the same equilibrium concentrations, what would the concentration of the product have to be in order to establish equilibrium?
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