Quiz
Question 1
(1 point)
What is Δn for the following equation in relating Kc to Kp?
N2(g) + 3 F2(g) ⇌ 2 NF3(g)
Question 1 options:
A)
4
B)
2
C)
0
D)
-3
E)
-2
Question 2
(1 point)
The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant.
H2(g) + Br2(g) ⇌ HBr(g)
Kc = 3.8 × 104
HBr(g) ⇌ H2(g) + Br2(g)
Kc = ?
Question 2 options:
A)
1.6 × 103
B)
6.4 × 10-4
C)
2.6 × 10-5
D)
5.3 × 10-5
E)
1.9 × 104
Question 3
(1 point)
For the reaction: N2(g) + 2 O2(g) ⇌ 2 NO2(g), Kc = 8.3 × 10-10 at 25°C. What is the concentration of N2 gas at equilibrium when the concentration of NO2 is five times the concentration of O2 gas?
Question 3 options:
A)
1.7 × 10-10 M
B)
6.0 × 109 M
C)
3.0 × 1010 M
D)
3.3 × 10-11 M
Question 4
(1 point)
The reaction below has a Kc value of 61. What is the value of Kp for this reaction at 400 K?
N2(g) + 3 H2(g) ⇌ 2 NH3(g)
Question 4 options:
A)
5.7 × 10-2
B)
1.9 × 10-2
C)
15
D)
61
E)
1.8
Question 5
(1 point)
Express the equilibrium constant for the following reaction.
12 NH3(g) ⇔ 6 N2(g) + 18 H2(g)
Question 5 options:
A)
K =
B)
K =
C)
K =
D)
K =
E)
K =
Question 6
(1 point)
Consider the following reaction and its equilibrium constant:
SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)
Kc = 0.33
A reaction mixture contains 0.41 M SO2, 0.13 M NO2, 0.11 M SO3 and 0.13 M NO. Which of the following statements is TRUE concerning this system?
Question 6 options:
A)
The reaction will shift in the direction of reactants.
B)
The equilibrium constant will decrease.
C)
The reaction will shift in the direction of products.
D)
The reaction quotient will decrease.
E)
The system is at equilibrium.
Question 7
(1 point)
The equilibrium constant is equal to 5.00 at 1300 K for the reaction:
2 SO2(g) + O2(g) ⇌ 2 SO3(g).
If initial concentrations are [SO2] = 6.00 M, [O2] = 0.45 M, and [SO3] = 9.00 M, the system is
Question 7 options:
A)
not at equilibrium and will shift to the left to achieve an equilibrium state.
B)
not at equilibrium and will shift to the right to achieve an equilibrium state.
C)
not at equilibrium and will remain in an unequilibrated state.
D)
at equilibrium.
Question 8
(1 point)
Determine the value of Kc for the following reaction if the equilibrium concentrations are as follows: [H2]eq = 0.14 M, [Br2]eq = 0.39 M, [HBr]eq = 1.6 M.
H2(g) + Br2(g) ⇌ 2 HBr(g)
Question 8 options:
A)
2.1 × 10-2
B)
29
C)
8.7 × 10-2
D)
3.4 × 10-2
E)
47
Question 9
(1 point)
Express the equilibrium constant for the following reaction.
5 P4O10(s) ⇌ 5 P4(s) + 25 O2(g)
Question 9 options:
A)
K =
B)
K =
C)
K =
D)
K =
E)
K = [O2]25
Question 10
(1 point)
For the isomerization reaction:
butane ⇌ isobutane
Kp equals 25 at 500°C. If the initial pressures of butane and isobutane are 5.0. atm and 0.0 atm, respectively, what are the pressures of the two gases at equilibrium?
Question 10 options:
A)
P(butane) = 0.20 atm and P(isobutane) = 5.0. atm
B)
P(butane) = 0.19 atm and P(isobutane) = 4.8 atm
C)
P(butane) = 5.0 atm and P(isobutane) = 0.80 atm
D)
P(butane) = 4.8 atm and P(isobutane) = 0.19 atm
Question 11
(1 point)
Consider the following reaction:
2 H2O(g) + 2 SO2(g) ⇌ 2 H2S(g) + 3 O2(g)
A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if Kc for the reaction at this temperature is 1.3 × 10-6.
Question 11 options:
A)
3.1 × 10-3 M
B)
0.12 M
C)
0.045 M
D)
0.058 M
E)
0.028 M
Question 12
(1 point)
The K
p
for the reaction below is 1.49 × 108 at 100.0°C:
CO(g) + Cl
2
(g) ⇌ COCl
2
(g)
In an equilibrium mixture of the three gases, P
CO
= P
Cl
2
= 2.22 × 10-4 atm. The partial pressure of the product, phosgene (COCl
2
), is ________ atm.
Question 12 options:
A)
3.02 × 1015
B)
3.31 × 104
C)
3.31 × 10-16
D)
6.67 × 1011
E)
7.34
Question 13
(1 point)
Consider the following reaction at equilibrium. What effect will removing NO2 have on the system?
SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)
Question 13 options:
A)
The reaction will shift in the direction of products.
B)
The reaction will shift in the direction of reactants.
C)
The equilibrium constant will decrease.
D)
No change will occur since SO3 is not included in the equilibrium expression.
E)
The reaction will shift to decrease the pressure.
Question 14
(1 point)
Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium pressure of CO.
CO(g) + 2 H2(g) ⇌ CH3OH(l)
Kp = 2.25 × 104
P(H2)eq = 0.52 atm
Question 14 options:
A)
1.6 × 10-4 atm
B)
8.5 × 10-5 atm
C)
6.25 × 10-3 atm
D)
1.2 × 10-5 atm
E)
8.3 × 104 atm
Question 15
(1 point)
Express the equilibrium constant for the following reaction.
4 CH3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)
Question 15 options:
A)
K =
B)
K =
C)
K =
D)
K =
E)
K =
Question 16
(1 point)
Express the equilibrium constant for the following reaction.
2 P4(s) + 10 O2(g) ⇌ 2 P4O10(s)
Question 16 options:
A)
K =
B)
K =
C)
K =
D)
K = [O2]10
E)
K =
Question 17
(1 point)
The reaction below has a Kp value of 41. What is the value of Kc for this reaction at 400 K?
N2(g) + 3 H2(g) ⇌ 2 NH3(g)
Question 17 options:
A)
2.3 × 10-5
B)
41
C)
3.8 × 10-2
D)
26
E)
4.4 × 104
Question 18
(1 point)
What is Δn for the following equation in relating Kc to Kp?
2 SO2(g) + O2(g) ⇌ 2 SO3(g)
Question 18 options:
A)
4
B)
-1
C)
-2
D)
-3
E)
1
Question 19
(1 point)
What is Δn for the following equation in relating Kc to Kp?
2 SO3(g) ⇌ 2 SO2(g) + O2(g)
Question 19 options:
A)
-2
B)
-4
C)
0
D)
1
E)
-3
Question 20
(1 point)
Consider the following reaction at equilibrium. What effect will increasing the temperature have on the system?
Fe3O4(s) + CO(g) ⇌ 3 FeO(s) + CO2(g)
ΔH°= +35.9 kJ
Question 20 options:
A)
The equilibrium constant will decrease.
B)
The reaction will shift to the right in the direction of products.
C)
The reaction will shift to the left in the direction of reactants.
D)
The equilibrium constant will increase.
E)
No effect will be observed.
Save All Responses
Submit Quiz
20 of 20 questions saved
16=wrong, for solids are not factored in. 20=wrong