NEW
Font size
WorksheetsUnit 7 Equilibrium Expression
Total questions: 21
Worksheet time: 21mins
After the equilibrium represented above is established, some pure O2 (g) is injected into the reaction vessel at a constant temperature. After equilibrium is reestablished, which of the following has a lower value compared to its value at the original equilibrium?
Keq for the reaction.
The total pressure in the reaction vessel.
The amount of SO3 (g) in the reaction vessel.
The amount of O2 (g) in the reaction vessel.
The amount of SO2 (g) in the reaction vessel.
Which of the following changes alone would cause a decrease in the value of Keq for the reaction represented above?
Decreasing the temperature.
Increasing the temperature.
Decreasing the volume of the reaction vessel.
Increasing the volume of the reaction vessel.
Adding a catalyst
Which of the following compounds is NOT appreciably soluble in water but is soluble in dilute hydrochloric acid?
Mg(OH)2 (s)
(NH4)2CO3 (s)
CuSO4 (s)
(NH4)2SO4 (s)
Sr(NO3)2 (s)
What is the molar solubility in water of Ag2CrO4?
8 x 10-12 M
2 x 10-12 M
(4 x 10−12)M
3(4 x 10−12)M
3(2 x 10−12)M
In a qualitative analysis for the presence of Pb2+, Fe2+, and Cu2+ ions in an aqueous solution, which of the following will allow the separation of Pb2+ from the other ions at room temperature?
Adding dilute Na2S (aq) solution.
Adding dilute HCl(aq) solution
Adding dilute NaOH(aq) solution
Adding dilute NH3(aq) solution
Adding dilute HNO3(aq) solution
On the basis of the solubility curves shown above, the greatest percentage of which compound can be recovered by cooling a saturated solution of that compound from 90oC to 30oC?
NaCl
KNO3
K2CrO4
K2SO4
Se2(SO4)3
In a saturated solution of Zn(OH)2 at 25oC, the value of [OH-] is 2.0 x 10-6 M. What is the value of the solubility product constant, Ksp, for Zn(OH)2 at 25oC?
4.0 x 10-18
8.0 x 10-18
1.6 x 10-17
4.0 x 10-12
2.0 x 10-6
I only
III only
I and II only
II and III only
I, II, and III
The reaction mixture represented above is at equilibrium at 298K, and the molar concentrations are [X] = 2.0 M, [Y] = 0.5 M, and [Z] = 4.0 M. What is the value of the equilibrium constant for the reaction at 298K?
0.50
2.0
4.0
16
32
The diagram above represents a mixture of NO2(g) and N2O4(g) in a 1.0 L container at a given temperature. The two gases are in equilibrium according to the equation 2NO2(g) ↔ N2O4(g). Which of the following must be true about the value of the equilibrium constant for the reaction at this temperature?
K = 0
0 < K < 1
K = 1
K > 1
There is not enough information to determine the relative value of K.
I only
II only
I and II only
II and III only
I, II, and III
The value of Ksp for PbCl2 is 1.6 x 10-5. What is the lowest concentration of Cl- (aq) that would be needed to begin precipitation of PbCl2 (s) in 0.010 M Pb(NO3)2?
1.6 x 10-7 M
4.0 x 10-4 M
1.6 x 10-3 M
2.6 x 10-7 M
4.0 x 10-2 M
At 25°C, the equilibrium constant for the reaction represented above has a value of 1.3. At 50°C, the value of the equilibrium constant is less than 1.3. Based on this information, which of the following must be correct?
The reaction rate decreases as the temperature is increased.
The reaction is thermodynamically favorable only at temperatures above 25°C.
At 25°C, Δ G° for the reaction is positive.
At 25°C, Δ S° for the reaction is positive.
At 25°C, Δ H° for the reaction is negative.
Given the value of the equilibrium constants K1 and K2 for the reactions represented above, what is the value of the equilibrium constant, K3, for the following reaction?
2 S(s) + 3 O2 (g) ↔ 2 SO3 (g)
K3 = ?
1 x 10130
3 x1080
1 x 1065
2 x 1040
7 x 1024
At 450oC, 2.0 moles each of H2(g), I2(g), and HI(g) are combined in a 1.0 L rigid container. The value of Kc at 450oC is 50. Which of the following will occur at the system moves toward equilibrium?
More H2(g) and I2(g) will form.
More HI(g) will form.
The total pressure will decrease.
No net reaction will occur, because the number of molecules is the same on both sides of the equation.
As the reaction progresses toward equilibrium, the rate of the forward reaction
increases until it becomes the same as the reverse reaction rate at equilibrium
stays constant before and after equilibrium is reached
decreases to become a constant nonzero rate at equilibrium
decreases to become zero at equilibrium
Which of the following statements about Kp, the equilibrium constant for the reaction, is correct?
Kp > 1
Kp < 1
Kp = 1
It cannot be determined whether Kp > 1, Kp < 1, or Kp = 1 without additional information.
Additional Cl2(g) is injected into the system at equilibrium. Which of the following graphs best shows the rate of the reverse reaction as a function of time? (Assume that the time for injection and mixing of the additional Cl2(g) is negligible.)
COCl2(g) decomposes according to the equation above. When pure COCl2(g) is injected into a rigid, previously evacuated flask at 690 K, the pressure in the flask at 690 K, the pressure in the flask is initially 1.0 atm. After the reaction reaches equilibrium at 690 K, the total pressure in the flask is 1.2 atm. What is the value of Kp for the reaction at 690 K?
0.040
0.050
0.80
1.0
A sealed rigid vessel contains BaO2(s) in equilibrium with BaO(s) and O2(g) as represented by the equation above. Which of the following changes will increase the amount of BaO2(s) in the vessel?
Removing a small amount of O2(g)
Removing a small amount of BaO(s)
Adding He gas to the vessel
Lowering the temperature
Which of the following explains the effect on the equilibrium constant, Kc, when the temperature of the reaction system is increased to 650 K?
Kc will increase because the activation energy of the forward reaction increases more than that of the reverse reaction.
Kc will increase because there are more reactant molecules than product molecules.
Kc will decrease because the reaction is exothermic.
Kc is constant and will not change.
