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For the following reaction at a certain temperature H:(g) + F2(g) = 2HF(g) the equilibrium concentrations in a 10.00-L rigid container are [H2] = 0.0600 M, [F2] = 0.0200 M, and [HF] = 0.620 M. If 0.490 moles of F2 is added to the equilibrium mixture, calculate the concentration of H2 after equilibrium is reestablished. %3D

For the following reaction at a certain temperature H:(g) + F2(g) = 2HF(g) the equilibrium concentrations in a 10.00-L rigid container are [H2] = 0.0600 M, [F2] = 0.0200 M, and [HF] = 0.620 M. If 0.490 moles of F2 is added to the equilibrium mixture, calculate the concentration of H2 after equilibrium is reestablished. %3D

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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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For the following reaction at a certain temperature H2(g) + F2(g) = 2HF(g) the equilibrium concentrations in a 10.00-L rigid container are [H>] = 0.0600 M, [F2] = 0.0200 M, and [HF] = 0.620 M. If 0.490 moles of F2 is added to the equilibrium mixture, calculate the concentration of H2 after equilibrium is reestablished.
Transcribed Image Text:For the following reaction at a certain temperature H2(g) + F2(g) = 2HF(g) the equilibrium concentrations in a 10.00-L rigid container are [H>] = 0.0600 M, [F2] = 0.0200 M, and [HF] = 0.620 M. If 0.490 moles of F2 is added to the equilibrium mixture, calculate the concentration of H2 after equilibrium is reestablished.
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