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Consider the following reaction: Co(g) + H20(g) → CO2(g) + H2(g) Kp = 12.7 at 1000°C Find the equilibrium partial pressure for water in atm, if a reaction mixture initially contains a CO partial pressure of 1.1150 atm and a H20 partial pressure of 1.150 atm at 1000°C Answer:

Consider the following reaction: Co(g) + H20(g) → CO2(g) + H2(g) Kp = 12.7 at 1000°C Find the equilibrium partial pressure for water in atm, if a reaction mixture initially contains a CO partial pressure of 1.1150 atm and a H20 partial pressure of 1.150 atm at 1000°C Answer:

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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Consider the following reaction: CO(g) + H20(g) CO2(g) + H2(g) K, = 12.7 at 1000°C Find the equilibrium partial pressure for water in atm, if a reaction mixture initially contains a CO partial pressure of 1.1150 atm and a H20 partial pressure of 1.150 atm at 1000°C Answer:
Transcribed Image Text:Consider the following reaction: CO(g) + H20(g) CO2(g) + H2(g) K, = 12.7 at 1000°C Find the equilibrium partial pressure for water in atm, if a reaction mixture initially contains a CO partial pressure of 1.1150 atm and a H20 partial pressure of 1.150 atm at 1000°C Answer:
Expert Solution
Step 1

Reaction:- 

Consider the following reaction:

CO(g) + H₂O(g) <------>CO2(g) + H2(g)

 

Partial pressure of CO =1.1150 atm 

Partial pressure of H₂O=  1.150atm

KP = 12.7

 

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