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Consider this equilibrium reaction at 400 K. Br, (g) + Cl, (g) = 2 BrCl(g) K. = 7.0 If the composition of the reaction mixture at 400 K is [BrCl] = 0.00684 M, [Br,] = 0.00193 M, and [Cl,] = 0.000354 M, %3D %3D what is the reaction quotient, Q? How is the reaction quotient related to the equilibrium constant, K, for this reaction? Oe < K, O e > K. O 0 = K,

Consider this equilibrium reaction at 400 K. Br, (g) + Cl, (g) = 2 BrCl(g) K. = 7.0 If the composition of the reaction mixture at 400 K is [BrCl] = 0.00684 M, [Br,] = 0.00193 M, and [Cl,] = 0.000354 M, %3D %3D what is the reaction quotient, Q? How is the reaction quotient related to the equilibrium constant, K, for this reaction? Oe < K, O e > K. O 0 = K,

Chemistry
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
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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. Br, (g) + Cl, (g) = 2 BrCI(g) Ke = 7.0 If the composition of the reaction mixture at 400 K is [BrCI] what is the reaction quotient, Q? = 0.00684 M, [Br,] = 0.00193 M, and [Cl,] = 0.000354 M, %3D How is the reaction quotient related to the equilibrium constant, K, for this reaction? O0 < K, O 0 > K, 0 = K,
Transcribed Image Text:Consider this equilibrium reaction at 400 K. Br, (g) + Cl, (g) = 2 BrCI(g) Ke = 7.0 If the composition of the reaction mixture at 400 K is [BrCI] what is the reaction quotient, Q? = 0.00684 M, [Br,] = 0.00193 M, and [Cl,] = 0.000354 M, %3D How is the reaction quotient related to the equilibrium constant, K, for this reaction? O0 < K, O 0 > K, 0 = K,
Expert Solution
Step 1

The equilibrium reaction taking place is given as,

=> Br2 (g) + Cl2 (g) ------> 2 BrCl (g)                                   Kc = 7.0 

Given : [BrCl] = 0.00684 M

[Br2 ] = 0.00193 M

And [Cl2 ] = 0.000354 M

 

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