"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact thisreaction is one of the ways hydrogen is made industrially.A chemical engineer studying this reaction fills a 100 L tank with 13. mol of carbon monoxide gas and 23. mol of water vapor. When the mixture has come toequilibrium he determines that it contains 4.0 mol of carbon monoxide gas, 14. mol of water vapor and 9.0 mol of carbon dioxide.The engineer then adds another 8.0 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of hydrogen after equilibrium isreached the second time. Round your answer to 2 significant digits.molx10×Ś

Answer:Given reaction:In the reaction, 2 moles of gases (1 mole CO and 1 mole H2O) are forming 2…

Answered: "Synthesis gas" is a mixture of carbon…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter14: Chemical Equilibrium

Section: Chapter Questions

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"Synthesis gas" is a mixture of carbon monoxide and water vapor. At high temperature synthesis gas will form carbon dioxide and hydrogen, and in fact this
reaction is one of the ways hydrogen is made industrially.
A chemical engineer studying this reaction fills a 100 L tank with 13. mol of carbon monoxide gas and 23. mol of water vapor. When the mixture has come to
equilibrium he determines that it contains 4.0 mol of carbon monoxide gas, 14. mol of water vapor and 9.0 mol of carbon dioxide.
The engineer then adds another 8.0 mol of water, and allows the mixture to come to equilibrium again. Calculate the moles of hydrogen after equilibrium is
reached the second time. Round your answer to 2 significant digits.
mol
x10
×
Ś

Expert Solution

Step 1: Equilibrium constant expression for the given reaction

Answer:

Given reaction:

$CO left parenthesis straight g right parenthesis plus straight H subscript 2 straight O left parenthesis straight g right parenthesis rightwards harpoon over leftwards harpoon CO subscript 2 left parenthesis straight g right parenthesis plus straight H subscript 2 left parenthesis straight g right parenthesis$

In the reaction, 2 moles of gases (1 mole CO and 1 mole H₂O) are forming 2 moles of gases (1 mole CO₂ and 1 mole H₂), therefore, change in number of gaseous moles during the reaction is 0 and equilibrium constant expression for this reaction will be:

$straight K equals fraction numerator straight n subscript CO subscript 2 end subscript cross times straight n subscript straight H subscript 2 end subscript over denominator straight n subscript CO cross times straight n subscript straight H subscript 2 straight O end subscript end fraction$

Here, n represents the number of moles of respective specie.

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