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Consider this equilibrium reaction at 400 K. Br2(g) + Cl2(g) = 2 BrCl(g) Kc = 7.0 If the composition of the reaction mixture at 400 K is [BrCl] = 0.00556 M, [Brz] = 0.00161 M, and [Cl] = 0.000295 M, what is the reaction quotient, Q? Q = How is the reaction quotient related to the equilibrium constant, Kc, for this reaction? O e > Kc O Q = Kc OQ < Kc

Consider this equilibrium reaction at 400 K. Br2(g) + Cl2(g) = 2 BrCl(g) Kc = 7.0 If the composition of the reaction mixture at 400 K is [BrCl] = 0.00556 M, [Brz] = 0.00161 M, and [Cl] = 0.000295 M, what is the reaction quotient, Q? Q = How is the reaction quotient related to the equilibrium constant, Kc, for this reaction? O e > Kc O Q = Kc OQ < Kc

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Consider this equilibrium reaction at 400 K. Br2(g) + Cl2(g) = 2 BrCl(g) Kc = 7.0 If the composition of the reaction mixture at 400 K is [BrCl] = 0.00556 M, [Brz] = 0.00161 M, and [Cl] = 0.000295 M, what is the reaction quotient, Q? Q = How is the reaction quotient related to the equilibrium constant, Kc, for this reaction? O e > Kc O Q = Kc OQ < Kc
Transcribed Image Text:Consider this equilibrium reaction at 400 K. Br2(g) + Cl2(g) = 2 BrCl(g) Kc = 7.0 If the composition of the reaction mixture at 400 K is [BrCl] = 0.00556 M, [Brz] = 0.00161 M, and [Cl] = 0.000295 M, what is the reaction quotient, Q? Q = How is the reaction quotient related to the equilibrium constant, Kc, for this reaction? O e > Kc O Q = Kc OQ < Kc
General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning At 500 °C, hydrogen iodide decomposes according to 2 HI(g) = H2(g) + I2(g) For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2] = 0.447 M, [I] = 0.447 M , and [HI] = 3.78 M. If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached? [HI] = M M = [2) = M
Transcribed Image Text:General Chemistry 4th Edition McQuarrie • Rock • Gallogly University Science Books presented by Macmillan Learning At 500 °C, hydrogen iodide decomposes according to 2 HI(g) = H2(g) + I2(g) For HI(g) heated to 500 °C in a 1.00 L reaction vessel, chemical analysis determined these concentrations at equilibrium: [H2] = 0.447 M, [I] = 0.447 M , and [HI] = 3.78 M. If an additional 1.00 mol of HI(g) is introduced into the reaction vessel, what are the equilibrium concentrations after the new equilibrium has been reached? [HI] = M M = [2) = M
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