Nitrosyl bromide decomposes according to the chemical equation below. 2 NOBr(g) = 2 NO(g) + Br2(g) When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium, 22% of the NOBr decomposes. What is the equilibrium constant, Kp, for the reaction?
Nitrosyl bromide decomposes according to the chemical equation below. 2 NOBr(g) = 2 NO(g) + Br2(g) When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium, 22% of the NOBr decomposes. What is the equilibrium constant, Kp, for the reaction?
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ISBN:9781305957404
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Chapter1: Chemical Foundations
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Nitrosyl bromide decomposes according to the chemical equation below.
2 NOBr(g) = 2 NO(g) + Br2(g)
When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium, 22% of the NOBr decomposes. What is the equilibrium constant, Kp, for the reaction?
![initially present in a 1.OL flask at 25 °C, what change in concentrations (if any) will occur in time?
5. Consider the reaction A(aq) t 2 B(aq) where K,-4.1 at 25 "C, If 0.50 M A(aq) and 1.5 M B(sq) are
CHEM 102
Equilibrium Study Guide
[A] will decrease and [B] will decrease.
76. [A] will decrease and [B] will increase.
a.
[A] will increase and [B] will decrease.
d.
[A] will increase and [B] will increase.
c.
29
[A] and [B] remain unchanged.
e.
0. An aqueous mixture of hydrocyanie acid and ammonia bas initial concentrations of 0.100 M HICNGRD
0.140 M NH3(aq). At equilibrium, the CN (ag) concentration is 0.055 M. Calculate K for the reaction.
HCN(aq) + NH3(aq) = CN (aq) + NH,'(aq)
0.22
b.
a.
0.79
c.
1.5
d.
3.9
e.
14
7. Nitrosyl bromide decomposes according to the chemical equation below.
2 NOBr(g) = 2 NO(g) + Br2(g)
When 0.260 atm of NOB is sealed in a flask and allowed to reach equilibrium, 22% of the NOBI
decomposes. What is the equilibrium constant, Kp, for the reaction?
2.3 x 10-3
b. 4.5 x 10 з
3.5 x 10-2
d. 4.8 x 10-2
8.0 x 10-2
a.
с.
e.
8. The equilibrium constant, Kc, for the following reaction is 1.0 x 10 at 1500 K.
If 0.570 M N2 and 0.570 M O2 are allowed to equilibrate at 1500 K, what is the concentration of NO?
5.7 x 106 M
N2(g) + O2(g) =2 NO(g)
а.
b. 9.0 x 104M
2.4 x 104 M
1.8 x 10-3 M
2.4 x 10-3 M
с.
d.
e.
The equilibrium constant (K.) for the following reaction is 6.7 x 10-10 at 630 °C.
N2(s) + O2(g) =2 NO(g)
What is the equilibrium constant for the reaction below at the same temperature?
NO(g) = 1/2 N2(g) + 1/2 O2(g)
a. 3.9 x 104
b. 5.5 x 104
c. 7.5 x 108
d. 1.5 x 10°
3.0 x 10°
e.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F325a91f3-8d85-4e09-afe5-577f0476af29%2F55aac2d3-8db5-49d6-b961-9ff08adeddab%2Fbbes2x9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:initially present in a 1.OL flask at 25 °C, what change in concentrations (if any) will occur in time?
5. Consider the reaction A(aq) t 2 B(aq) where K,-4.1 at 25 "C, If 0.50 M A(aq) and 1.5 M B(sq) are
CHEM 102
Equilibrium Study Guide
[A] will decrease and [B] will decrease.
76. [A] will decrease and [B] will increase.
a.
[A] will increase and [B] will decrease.
d.
[A] will increase and [B] will increase.
c.
29
[A] and [B] remain unchanged.
e.
0. An aqueous mixture of hydrocyanie acid and ammonia bas initial concentrations of 0.100 M HICNGRD
0.140 M NH3(aq). At equilibrium, the CN (ag) concentration is 0.055 M. Calculate K for the reaction.
HCN(aq) + NH3(aq) = CN (aq) + NH,'(aq)
0.22
b.
a.
0.79
c.
1.5
d.
3.9
e.
14
7. Nitrosyl bromide decomposes according to the chemical equation below.
2 NOBr(g) = 2 NO(g) + Br2(g)
When 0.260 atm of NOB is sealed in a flask and allowed to reach equilibrium, 22% of the NOBI
decomposes. What is the equilibrium constant, Kp, for the reaction?
2.3 x 10-3
b. 4.5 x 10 з
3.5 x 10-2
d. 4.8 x 10-2
8.0 x 10-2
a.
с.
e.
8. The equilibrium constant, Kc, for the following reaction is 1.0 x 10 at 1500 K.
If 0.570 M N2 and 0.570 M O2 are allowed to equilibrate at 1500 K, what is the concentration of NO?
5.7 x 106 M
N2(g) + O2(g) =2 NO(g)
а.
b. 9.0 x 104M
2.4 x 104 M
1.8 x 10-3 M
2.4 x 10-3 M
с.
d.
e.
The equilibrium constant (K.) for the following reaction is 6.7 x 10-10 at 630 °C.
N2(s) + O2(g) =2 NO(g)
What is the equilibrium constant for the reaction below at the same temperature?
NO(g) = 1/2 N2(g) + 1/2 O2(g)
a. 3.9 x 104
b. 5.5 x 104
c. 7.5 x 108
d. 1.5 x 10°
3.0 x 10°
e.
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