At 1,900 K, the equilibrium constant for the reaction below is Kc = 2.13. Br2(g) 2 Br(g) What is the percent dissociation of Br2 at 1,900 K, if the initial concentration of Br2 is 1.75mol L-1 ? Give your answer accurate to two significant figures. Do not include the % sign as part of your answer. The percent dissocation of Br2 is % ? Hints: If the initial concentration of Br2 is Co and the concentration of Br2 decreases by x(because of dissociation), then the percent dissociation of Br2 is equal to 100(x/ Co). You may have to use the quadratic formula to solve this problem. The quadratic formula, given below, can be used to find the solutions to the equation ax² + bx+c = 0.

At 1,900 K, the equilibrium constant for the reaction below is Kc = 2.13. Br2(g) 2 Br(g) What is the percent dissociation of Br2 at 1,900 K, if the initial concentration of Br2 is 1.75mol L-1 ? Give your answer accurate to two significant figures. Do not include the % sign as part of your answer. The percent dissocation of Br2 is % ? Hints: If the initial concentration of Br2 is Co and the concentration of Br2 decreases by x(because of dissociation), then the percent dissociation of Br2 is equal to 100(x/ Co). You may have to use the quadratic formula to solve this problem. The quadratic formula, given below, can be used to find the solutions to the equation ax² + bx+c = 0.

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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