11. The relationship between kp and Kc for the following equilibrium reaction is equal to: CO(g)+3H2(g) CHA(g) + H2O (g) A) Kp = Kc (RT) B) Kp = Kc (RT) C) Kp = Kc (RT)2 D) Kp=Kc 12. If the acetic acid dissociation constant is k,= 1.8 X 10-5, and its concentration before dissociation (0.15M), the concentration of [H+] is equal to the following equilibrium equation. CH:COO +H+ CH:COOH A)4.26 X 10-3 B) 6.41 X 104 C) 2.62 X 104 D)1.64 X 10-3 13. When dissolved (1.93 g) of HNO2 acid (MW = 47) and dilute the volume to 500 ml, the [ H ]in the solution was 7.63X10-3 M, the value of the dissociation constant Ka was equal to : A) 7.8 X 104 B) 6 X 104 C) 4 X104 D) 2 X 104
11. The relationship between kp and Kc for the following equilibrium reaction is equal to: CO(g)+3H2(g) CHA(g) + H2O (g) A) Kp = Kc (RT) B) Kp = Kc (RT) C) Kp = Kc (RT)2 D) Kp=Kc 12. If the acetic acid dissociation constant is k,= 1.8 X 10-5, and its concentration before dissociation (0.15M), the concentration of [H+] is equal to the following equilibrium equation. CH:COO +H+ CH:COOH A)4.26 X 10-3 B) 6.41 X 104 C) 2.62 X 104 D)1.64 X 10-3 13. When dissolved (1.93 g) of HNO2 acid (MW = 47) and dilute the volume to 500 ml, the [ H ]in the solution was 7.63X10-3 M, the value of the dissociation constant Ka was equal to : A) 7.8 X 104 B) 6 X 104 C) 4 X104 D) 2 X 104
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
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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Solve 11,12,and 13
No steps needed
![11. The relationship between kp and Kc for the following equilibrium reaction is
equal to:
CO(g)+3H2(g) CH(g)
+ H2O (g)
A) Kp = Kc (RT)-1
B) Kp = Kc (RT)
C) Kp = Kc (RT)2
D) Kp=Kc
12. If the acetic acid dissociation constant is ka= 1.8 X 105, and its concentration
before dissociation (0.15M), the concentration of [H+] is equal to the following
equilibrium equation.
CH;COO +H*
CH3COOH
A)4.26 X 10-3
B) 6.41 X 104
C) 2.62 X 104
D)1.64 X 10-3
13. When dissolved (1.93 g) of HNO2 acid (MW = 47) and dilute the volume to
500 ml, the [ H ]in the solution was 7.63X10-3 M, the value of the dissociation
constant Ka was equal to :
A) 7.8 X 104
B) 6 X 104
C) 4 X10+
D) 2 X 104](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fda57e861-1192-4125-ade2-707126d6bb10%2F56f067b2-2b9c-4600-bdb8-49f61226fc55%2F24sdsd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:11. The relationship between kp and Kc for the following equilibrium reaction is
equal to:
CO(g)+3H2(g) CH(g)
+ H2O (g)
A) Kp = Kc (RT)-1
B) Kp = Kc (RT)
C) Kp = Kc (RT)2
D) Kp=Kc
12. If the acetic acid dissociation constant is ka= 1.8 X 105, and its concentration
before dissociation (0.15M), the concentration of [H+] is equal to the following
equilibrium equation.
CH;COO +H*
CH3COOH
A)4.26 X 10-3
B) 6.41 X 104
C) 2.62 X 104
D)1.64 X 10-3
13. When dissolved (1.93 g) of HNO2 acid (MW = 47) and dilute the volume to
500 ml, the [ H ]in the solution was 7.63X10-3 M, the value of the dissociation
constant Ka was equal to :
A) 7.8 X 104
B) 6 X 104
C) 4 X10+
D) 2 X 104
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