For items 10-12. The decomposition of NH4CI (s) at a given temperature of 548 K, the Kp = 0.01072. NH4CI (s) NH4 (g) + HCl (g) 10. If 10.00 g of solid NH4CI (s) is introduced to the reaction vessel of 500 mL and the system is allowed to reach equilibrium, calculate for the partial pressure of the ammonia. NHẠCI (s) =NH4 (g) + HCl (g) C. 0.0212 atm A. 0.104 atm B. 8.41 atm D. 5.30 atm E. 0.00198 atm 11. What is the Kc of the reaction at the given temperature? C. 1.59 x 10-3 A. 2.48 x 10-9 B. 2.35 x 10-4 D. 5.16 x 10-6 12. Calculate the temperature needed to change the Kp of the reaction to twice of the initial equilibrium constant. The A,H = 176.01 kJ/mol A. 538 K B. 558 K C. 265 K D. 285 K
For items 10-12. The decomposition of NH4CI (s) at a given temperature of 548 K, the Kp = 0.01072. NH4CI (s) NH4 (g) + HCl (g) 10. If 10.00 g of solid NH4CI (s) is introduced to the reaction vessel of 500 mL and the system is allowed to reach equilibrium, calculate for the partial pressure of the ammonia. NHẠCI (s) =NH4 (g) + HCl (g) C. 0.0212 atm A. 0.104 atm B. 8.41 atm D. 5.30 atm E. 0.00198 atm 11. What is the Kc of the reaction at the given temperature? C. 1.59 x 10-3 A. 2.48 x 10-9 B. 2.35 x 10-4 D. 5.16 x 10-6 12. Calculate the temperature needed to change the Kp of the reaction to twice of the initial equilibrium constant. The A,H = 176.01 kJ/mol A. 538 K B. 558 K C. 265 K D. 285 K
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter16: Solubility And Precipitation Equilibria
Section: Chapter Questions
Problem 70AP
Related questions
Question
![For items 10-12. The decomposition of NH4C1 (s) at a given temperature of 548 K, the Kp = 0.01072.
NHẠCI (s) =NH4 (g) + HCl (g)
10. If 10.00 g of solid NH4C1 (s) is introduced to the reaction vessel of 500 mL and the system is
allowed to reach equilibrium, calculate for the partial pressure of the ammonia.
NHẠCI (s) = NH4 (g) + HCl (g)
C. 0.0212 atm
A. 0.104 atm
B. 8.41 atm
D. 5.30 atm
E. 0.00198 atm
11. What is the Kc of the reaction at the given temperature?
C. 1.59 x 10-3
A. 2.48 x 10-9
B. 2.35 x 10-4
D. 5.16 x 10-6
12. Calculate the temperature needed to change the Kp of the reaction to twice of the initial
equilibrium constant. The A,H
= 176.01 kJ/mol
A. 538 K
B. 558 K
C. 265 K
D. 285 K](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F11304275-2569-4e4f-9f66-ac5f05f22f60%2Ff66736cb-9921-4c47-a36f-2b5a394f01ef%2Fpbglwln_processed.jpeg&w=3840&q=75)
Transcribed Image Text:For items 10-12. The decomposition of NH4C1 (s) at a given temperature of 548 K, the Kp = 0.01072.
NHẠCI (s) =NH4 (g) + HCl (g)
10. If 10.00 g of solid NH4C1 (s) is introduced to the reaction vessel of 500 mL and the system is
allowed to reach equilibrium, calculate for the partial pressure of the ammonia.
NHẠCI (s) = NH4 (g) + HCl (g)
C. 0.0212 atm
A. 0.104 atm
B. 8.41 atm
D. 5.30 atm
E. 0.00198 atm
11. What is the Kc of the reaction at the given temperature?
C. 1.59 x 10-3
A. 2.48 x 10-9
B. 2.35 x 10-4
D. 5.16 x 10-6
12. Calculate the temperature needed to change the Kp of the reaction to twice of the initial
equilibrium constant. The A,H
= 176.01 kJ/mol
A. 538 K
B. 558 K
C. 265 K
D. 285 K
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