The equilibrium constant is 237 at a certain temperature for the reaction N2(g) + O2(g) 2 2NO(g) Calculate the concentrations of all species at equilibrium when 1.62 M of each component is added to a flask. HOW DO WE GET THERE? We will define the change in the concentrations to reach equilibrium in terms of x. Let x equal the number of moles per liter of N, consumed to reach equilibrium. N2(g) + O2(g) = 2NO(g) Initial: 1.62 1.62 1.62 Change: Equilibrium: 1.62–x -x -x +2x 1.62-x 1.62+2x Therefore, [NO]? [N2][O2] K= 237 = (1.62+2x)? (1.62 — х)(1.62 — х) What is the value of x?

The equilibrium constant is 237 at a certain temperature for the reaction N2(g) + O2(g) 2 2NO(g) Calculate the concentrations of all species at equilibrium when 1.62 M of each component is added to a flask. HOW DO WE GET THERE? We will define the change in the concentrations to reach equilibrium in terms of x. Let x equal the number of moles per liter of N, consumed to reach equilibrium. N2(g) + O2(g) = 2NO(g) Initial: 1.62 1.62 1.62 Change: Equilibrium: 1.62–x -x -x +2x 1.62-x 1.62+2x Therefore, [NO]? [N2][O2] K= 237 = (1.62+2x)? (1.62 — х)(1.62 — х) What is the value of x?

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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