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3. Consider the equilibrium below: 1.6 mol of HI was placed in a 1.0 L container and allowed to reach equilibrium, what would the equilibrium concentrations be for H₂(g), I2(g) and HI(g) if the K = 36 for this reaction? H₂(g) + I₂(g) => 2HI(g)

3. Consider the equilibrium below: 1.6 mol of HI was placed in a 1.0 L container and allowed to reach equilibrium, what would the equilibrium concentrations be for H₂(g), I2(g) and HI(g) if the K = 36 for this reaction? H₂(g) + I₂(g) => 2HI(g)

Chemistry
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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could you help me understand how to do this problem and explain the steps you used please, could you also use an ICE table as well thank you.

3. Consider the equilibrium below: 1.6 mol of HI was placed in a 1.0 L container and allowed to reach equilibrium, what would the equilibrium concentrations be for H₂(g), I2(g) and HI(g) if the K = 36 for this reaction? H₂(g) + I2(g) <= ===> 2HI(g)
Transcribed Image Text:3. Consider the equilibrium below: 1.6 mol of HI was placed in a 1.0 L container and allowed to reach equilibrium, what would the equilibrium concentrations be for H₂(g), I2(g) and HI(g) if the K = 36 for this reaction? H₂(g) + I2(g) <= ===> 2HI(g)
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