At 1000oC, 10.00 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 9.00 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.
At 1000oC, 10.00 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 9.00 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.
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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At 1000oC, 10.00 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 9.00 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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