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6. Consider the following Co(g) + H2O(g) CO2(g) + H2(g) Ko= 0.58 at 1273 K A sealed 4.00L vessel initially contains 1.00 mole CO2(g), 1.00 mole H2(g), 0.600 moles CO(g), and 0.600 moles of H20(g). Calculate the moles of H2(g) present at equilibrium.

6. Consider the following Co(g) + H2O(g) CO2(g) + H2(g) Ko= 0.58 at 1273 K A sealed 4.00L vessel initially contains 1.00 mole CO2(g), 1.00 mole H2(g), 0.600 moles CO(g), and 0.600 moles of H20(g). Calculate the moles of H2(g) present at equilibrium.

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Chemistry
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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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6. Consider the following reaction: CO(g) + H2O(g) CO2(g) + H2(g) Ko = 0.58 at 1273 K* A sealed 4.00L vessel initially contains 1.00 mole CO2(g), 1.00 mole H2(g), 0.600 moles CO(g), and 0.600 moles of H2O(g). Calculate the moles of H2(g) present at equilibrium. The NG Reference: General Chemistry 8th Ed: Ebbing and Gammon: 2005 by Houghton Mifflin. New York. page 654, print 68
Transcribed Image Text:6. Consider the following reaction: CO(g) + H2O(g) CO2(g) + H2(g) Ko = 0.58 at 1273 K* A sealed 4.00L vessel initially contains 1.00 mole CO2(g), 1.00 mole H2(g), 0.600 moles CO(g), and 0.600 moles of H2O(g). Calculate the moles of H2(g) present at equilibrium. The NG Reference: General Chemistry 8th Ed: Ebbing and Gammon: 2005 by Houghton Mifflin. New York. page 654, print 68
Expert Solution
Step 1

The balanced reaction taking place is given as,

=> CO (g) + H2O (g) ------> CO2 (g) + H2 (g)                          Kc = 0.58 

Given : Volume of vessel = 4.00 L

Initial moles of CO2 = 1.00 mol.

Initial moles of H2 = 1.00 mol.

Initial moles of CO = 0.600 mol.

And initial moles of H2O = 0.600 mol.

 

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