The initial concentrations of four species involved in an equilibrium are: 2) [HCI] = 0.100 M, [O2] = 0.300 M and [H>O] = 0.500 M. Is the reaction at equilibrium? If not, in what direction must the reaction shift for the equilibrium to be reached? Set up K, in terms of the initial amounts and x as done in class. Do not try to solve for x. Set it up so x is positive. %3D 4 HClg) + O2) > 2 Cl2(g) + 2 H2O(2) K = 52

The initial concentrations of four species involved in an equilibrium are: 2) [HCI] = 0.100 M, [O2] = 0.300 M and [H>O] = 0.500 M. Is the reaction at equilibrium? If not, in what direction must the reaction shift for the equilibrium to be reached? Set up K, in terms of the initial amounts and x as done in class. Do not try to solve for x. Set it up so x is positive. %3D 4 HClg) + O2) > 2 Cl2(g) + 2 H2O(2) K = 52

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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The initial concentrations of four species involved in an equilibrium are: [Cl2] = 1.40 M, [HCl] = 0.100 M, [O2] = 0.300 M and [H2O] = 0.500 M. Is the reaction at equilibrium? If not, in what direction must the reaction shift for the equilibrium to be reached? Set up Kc in terms of the initial amounts and x as done in class. Do not try to solve for x. Set it up so x is positive. 4 HCl(g) + O2(g) <====> 2 Cl2(g) + 2 H2O(g) Kc = 52 At equil? ______ Direction? _______ Expression ____________
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