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
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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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![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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc3642bbe-9bdc-4a17-a1cb-4f4ee175bfec%2F6ffb7e05-15fd-4edf-990d-84b9874765c5%2Fhtx8p7d_processed.png&w=3840&q=75)
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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc3642bbe-9bdc-4a17-a1cb-4f4ee175bfec%2F6ffb7e05-15fd-4edf-990d-84b9874765c5%2Fu2ja6sg_processed.png&w=3840&q=75)
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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