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A chemist places carbon dioxide gas in a rigid container. The following reaction takes place (at a certain temperature) as follows, with a K, = 2.0 x 10*. 2 CO,(g) = 200(g) + O2(g) If a chemist starts with an initial CO, pressure of 5 atm, what are the equilibrium pressures for all species involved in this reaction? (use the small x approximation) 3.1 You must fill out the ICEE table below for full credit. Round your answer to 2 significant digits. If you need more space to show your work, you can use the backside of this page. 2 Co,(g) 2 Co(g) + O2(g) %3D Initial concentrations Change Expression Equilibrium concentrations 3.2 Is the small x-approximation valid? (yes/no) What percent of the initial CO, reacted?

A chemist places carbon dioxide gas in a rigid container. The following reaction takes place (at a certain temperature) as follows, with a K, = 2.0 x 10*. 2 CO,(g) = 200(g) + O2(g) If a chemist starts with an initial CO, pressure of 5 atm, what are the equilibrium pressures for all species involved in this reaction? (use the small x approximation) 3.1 You must fill out the ICEE table below for full credit. Round your answer to 2 significant digits. If you need more space to show your work, you can use the backside of this page. 2 Co,(g) 2 Co(g) + O2(g) %3D Initial concentrations Change Expression Equilibrium concentrations 3.2 Is the small x-approximation valid? (yes/no) What percent of the initial CO, reacted?

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.103PAE: 12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat....
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A chemist places carbon dioxide gas in a rigid container. The following reaction takes place (at a certain temperature) as follows, with a K, = 2.0 x 10*. 2 CO.(g) = 200(g) + O¿(g) If a chemist starts with an initial CO, pressure of 5 atm, what are the equilibrium pressures for all species involved in this reaction? (use the small x approximation) 3.1 You must fill out the ICEE table below for full credit. Round your answer to 2 significant digits. If you need more space to show your work, you can use the backside of this page. 2 CO,(g) = 2 CO(g) + O2(g) %3D + Initial concentrations Change Expression Equilibrium concentrations 3.2 What percent of the initial CO, reacted? Is the small x-approximation valid? (yes/no)
Transcribed Image Text:A chemist places carbon dioxide gas in a rigid container. The following reaction takes place (at a certain temperature) as follows, with a K, = 2.0 x 10*. 2 CO.(g) = 200(g) + O¿(g) If a chemist starts with an initial CO, pressure of 5 atm, what are the equilibrium pressures for all species involved in this reaction? (use the small x approximation) 3.1 You must fill out the ICEE table below for full credit. Round your answer to 2 significant digits. If you need more space to show your work, you can use the backside of this page. 2 CO,(g) = 2 CO(g) + O2(g) %3D + Initial concentrations Change Expression Equilibrium concentrations 3.2 What percent of the initial CO, reacted? Is the small x-approximation valid? (yes/no)
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