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.
Chemistry
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Chapter17: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 118CP: Consider the reaction H2(g)+Br2(g)2HBr(g) where H = 103.8 kJ/mol. In a particular experiment, equal...
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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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