24. Professor Sanov runs the reaction in problem 22 and allows it to reach equilibrium at T = 740 K. He then finds the equilibrium concentrations of N₂ and H₂ to be [N₂] = 0.90 Mand [H₂] = 1.0 M. Given that Kc = 10., what is the equilibrium concentration of NH3 in Professor Sanov's experiment? (A) 0.03 (B) 0.10 (C) 0.30 (D) 0.40 (E) 1.0
24. Professor Sanov runs the reaction in problem 22 and allows it to reach equilibrium at T = 740 K. He then finds the equilibrium concentrations of N₂ and H₂ to be [N₂] = 0.90 Mand [H₂] = 1.0 M. Given that Kc = 10., what is the equilibrium concentration of NH3 in Professor Sanov's experiment? (A) 0.03 (B) 0.10 (C) 0.30 (D) 0.40 (E) 1.0
Chemistry
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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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![24. Professor Sanov runs the reaction in problem 22 and allows it to reach
equilibrium at T = 740 K. He then finds the equilibrium concentrations of N₂ and H₂
to be [N₂] = 0.90 Mand [H₂] = 1.0 M. Given that Kc = 10., what is the equilibrium
concentration of NH3 in Professor Sanov's experiment?
(A) 0.03
(B) 0.10
(C) 0.30
(D) 0.40
(E) 1.0](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcb45a7b7-d1aa-4ac7-ad98-90aa0325071f%2F6a2ad54c-16a2-4216-85fc-51b3225ef192%2Flysdy5h_processed.png&w=3840&q=75)
Transcribed Image Text:24. Professor Sanov runs the reaction in problem 22 and allows it to reach
equilibrium at T = 740 K. He then finds the equilibrium concentrations of N₂ and H₂
to be [N₂] = 0.90 Mand [H₂] = 1.0 M. Given that Kc = 10., what is the equilibrium
concentration of NH3 in Professor Sanov's experiment?
(A) 0.03
(B) 0.10
(C) 0.30
(D) 0.40
(E) 1.0
![Consider the reaction:
2 NH3(g)
N₂(g) + 3 H₂(g).
At T = 740 K, the equilibrium constant K for this reaction is Kc = 10.
22. What is the correct form of the equilibrium constant K for this reaction?
3
(A) Kc = [N₂] [H₂]³
(B) Kc =
(C) Kc =
(D) Kc
2[NH3]
[N₂] + 3 [H₂]
=
(E) Kc =
[N₂] + 3[H₂]
2[NH3]
[NH3]²
[N₂] [H₂]³
[N₂] [H₂] ³
[NH3]²](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcb45a7b7-d1aa-4ac7-ad98-90aa0325071f%2F6a2ad54c-16a2-4216-85fc-51b3225ef192%2Fy06qrzb_processed.png&w=3840&q=75)
Transcribed Image Text:Consider the reaction:
2 NH3(g)
N₂(g) + 3 H₂(g).
At T = 740 K, the equilibrium constant K for this reaction is Kc = 10.
22. What is the correct form of the equilibrium constant K for this reaction?
3
(A) Kc = [N₂] [H₂]³
(B) Kc =
(C) Kc =
(D) Kc
2[NH3]
[N₂] + 3 [H₂]
=
(E) Kc =
[N₂] + 3[H₂]
2[NH3]
[NH3]²
[N₂] [H₂]³
[N₂] [H₂] ³
[NH3]²
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