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t 800°C, 20.00 atm of CO2(g) is stored in a 1.00 L container. 10.00 g of C (s) is then added into the ontainer. The CO2(g) then reacts with C(s) to form CO(g) according to the following reaction: CO2(g) + C(s) = 2C0(g) fter the reaction has reached equilibrium, the mass of C (s) is reduced to 9.12 g. The molar mass of is 12.00 g/mol. Determine the partial pressure of CO at equilibrium. Determine the partial pressure of CO2 at equilibrium. Write and Calculate the equilibrium constant of the above reaction. The container is compressed from 1.00 L to 0.50 L. Without doing any calculation, predict how e mass of C (s) change at the end of the reaction. this question, the volume of the C (s) is negligible compared to the volume of the container.

t 800°C, 20.00 atm of CO2(g) is stored in a 1.00 L container. 10.00 g of C (s) is then added into the ontainer. The CO2(g) then reacts with C(s) to form CO(g) according to the following reaction: CO2(g) + C(s) = 2C0(g) fter the reaction has reached equilibrium, the mass of C (s) is reduced to 9.12 g. The molar mass of is 12.00 g/mol. Determine the partial pressure of CO at equilibrium. Determine the partial pressure of CO2 at equilibrium. Write and Calculate the equilibrium constant of the above reaction. The container is compressed from 1.00 L to 0.50 L. Without doing any calculation, predict how e mass of C (s) change at the end of the reaction. this question, the volume of the C (s) is negligible compared to the volume of the container.

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter14: Chemical Equilibirum
Section: Chapter Questions
Problem 14.122QP: A chemist wants to prepare phosgene, COCl2, by the following reaction: CO(g)+Cl2(g)COCl2(g) He...
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At 800°C, 20.00 atm of CO2(g) is stored in a 1.00 L container. 10.00 g of C (s) is then added into the container. The CO2(g) then reacts with C(s) to form CO(g) according to the following reaction: CO2(g) + C(s) = 2CO(g) After the reaction has reached equilibrium, the mass of C (s) is reduced to 9.12 g. The molar mass of C is 12.00 g/mol. a) Determine the partial pressure of CO at equilibrium. b) Determine the partial pressure of CO2 at equilibrium. c) Write and Calculate the equilibrium constant of the above reaction. d) The container is compressed from 1.00 L to 0.50 L. Without doing any calculation, predict how the mass of C (s) change at the end of the reaction. In this question, the volume of the C (s) is negligible compared to the volume of the container.
Transcribed Image Text:At 800°C, 20.00 atm of CO2(g) is stored in a 1.00 L container. 10.00 g of C (s) is then added into the container. The CO2(g) then reacts with C(s) to form CO(g) according to the following reaction: CO2(g) + C(s) = 2CO(g) After the reaction has reached equilibrium, the mass of C (s) is reduced to 9.12 g. The molar mass of C is 12.00 g/mol. a) Determine the partial pressure of CO at equilibrium. b) Determine the partial pressure of CO2 at equilibrium. c) Write and Calculate the equilibrium constant of the above reaction. d) The container is compressed from 1.00 L to 0.50 L. Without doing any calculation, predict how the mass of C (s) change at the end of the reaction. In this question, the volume of the C (s) is negligible compared to the volume of the container.
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