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

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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