Q. What is the effect of adding a catalyst to a chemical equilibrium?
A.
Increases the yield of products
B.
Increases the rate of reaction
C.
Shifts the equilibrium position
D.
Has no effect on the equilibrium
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Solution
A catalyst speeds up the rate of both the forward and reverse reactions equally, thus having no effect on the position of equilibrium.
Correct Answer: D — Has no effect on the equilibrium
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Q. What is the effect of adding an inert gas at constant volume on the equilibrium of a reaction?
A.
Shifts the equilibrium to the right
B.
Shifts the equilibrium to the left
C.
No effect on the equilibrium position
D.
Increases the equilibrium constant
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Solution
Adding an inert gas at constant volume does not change the partial pressures of the reactants and products, thus it has no effect on the equilibrium position.
Correct Answer: C — No effect on the equilibrium position
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Q. What is the effect of adding an inert gas at constant volume on the equilibrium of the reaction A(g) ⇌ B(g)?
A.
Shifts to the right
B.
Shifts to the left
C.
No effect
D.
Increases the rate of reaction
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Solution
Adding an inert gas at constant volume does not change the partial pressures of the reactants or products, hence no effect on equilibrium.
Correct Answer: C — No effect
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Q. What is the effect of increasing the pressure on the equilibrium of the reaction: 2N2(g) + 3H2(g) ⇌ 2NH3(g)?
A.
Shifts to the left
B.
Shifts to the right
C.
No effect
D.
Increases the rate of reaction
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Solution
Increasing the pressure will shift the equilibrium to the right, favoring the formation of NH3, as there are fewer moles of gas on the product side.
Correct Answer: B — Shifts to the right
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Q. What is the equilibrium constant expression for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g)?
A.
Kc = [NH3]^2 / ([N2][H2]^3)
B.
Kc = [N2][H2]^3 / [NH3]^2
C.
Kc = [NH3]^2 / [N2][H2]
D.
Kc = [N2][H2] / [NH3]^2
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Solution
The equilibrium constant Kc is given by the ratio of the concentration of products to reactants, raised to the power of their coefficients.
Correct Answer: A — Kc = [NH3]^2 / ([N2][H2]^3)
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Q. What is the equilibrium constant expression for the reaction: 2A + B ⇌ C?
A.
[C]/([A]^2[B])
B.
[A]^2[B]/[C]
C.
[C]/[A][B]
D.
[A][B]/[C]
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Solution
The equilibrium constant K is given by the expression K = [C]/([A]^2[B]) for the reaction 2A + B ⇌ C.
Correct Answer: A — [C]/([A]^2[B])
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Q. What is the relationship between Kp and Kc for the reaction aA(g) + bB(g) ⇌ cC(g) + dD(g)?
A.
Kp = Kc(RT)^(d+c-b-a)
B.
Kp = Kc(RT)^(a+b-c-d)
C.
Kp = Kc/(RT)^(d+c-b-a)
D.
Kp = Kc/(RT)^(a+b-c-d)
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Solution
The relationship between Kp and Kc is given by Kp = Kc(RT)^(Δn), where Δn = (d+c) - (a+b).
Correct Answer: A — Kp = Kc(RT)^(d+c-b-a)
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Q. What is the relationship between the equilibrium constant (K) and the reaction quotient (Q)?
A.
K = Q at equilibrium
B.
K > Q at equilibrium
C.
K < Q at equilibrium
D.
K is independent of Q
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Solution
At equilibrium, the reaction quotient Q is equal to the equilibrium constant K.
Correct Answer: A — K = Q at equilibrium
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Q. What is the relationship between the equilibrium constants Kp and Kc for a gaseous reaction?
A.
Kp = Kc
B.
Kp = Kc(RT)^(Δn)
C.
Kp = Kc/RT
D.
Kp = Kc(RT)^(Δn) where Δn is the change in moles of gas
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Solution
The relationship between Kp and Kc is given by Kp = Kc(RT)^(Δn), where Δn is the change in the number of moles of gas.
Correct Answer: B — Kp = Kc(RT)^(Δn)
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Q. What is the value of the equilibrium constant Kc for the reaction: 2A ⇌ B + C if at equilibrium [A] = 0.5 M, [B] = 0.2 M, and [C] = 0.3 M?
A.
0.12
B.
0.30
C.
0.60
D.
1.20
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Solution
Kc = [B][C] / [A]^2 = (0.2)(0.3) / (0.5)^2 = 0.12 / 0.25 = 0.48.
Correct Answer: C — 0.60
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Q. What is the value of the equilibrium constant Kp for the reaction 2NO2(g) ⇌ N2O4(g) at a certain temperature?
A.
Kp = (P_N2O4) / (P_NO2)^2
B.
Kp = (P_NO2)^2 / (P_N2O4)
C.
Kp = (P_N2O4)^2 / (P_NO2)
D.
Kp = (P_NO2) / (P_N2O4)^2
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Solution
Kp is defined as the partial pressure of products over reactants, raised to the power of their coefficients.
Correct Answer: A — Kp = (P_N2O4) / (P_NO2)^2
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Q. What is the value of the equilibrium constant Kp for the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g) at 25°C?
A.
0.5
B.
1.0
C.
0.1
D.
Depends on the initial concentrations
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Solution
The value of Kp is specific to the reaction conditions and cannot be determined without knowing the initial concentrations or the extent of the reaction.
Correct Answer: D — Depends on the initial concentrations
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Q. Which of the following changes will increase the yield of products in an exothermic reaction at equilibrium?
A.
Increase the temperature
B.
Decrease the pressure
C.
Increase the concentration of reactants
D.
Add a catalyst
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Solution
Increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.
Correct Answer: C — Increase the concentration of reactants
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Q. Which of the following changes will NOT affect the position of equilibrium in a closed system?
A.
Adding a catalyst
B.
Changing the concentration of reactants
C.
Changing the pressure
D.
Changing the temperature
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Solution
A catalyst speeds up the rate of both the forward and reverse reactions equally, thus it does not change the position of equilibrium.
Correct Answer: A — Adding a catalyst
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Q. Which of the following changes will NOT affect the position of equilibrium?
A.
Adding a catalyst
B.
Changing the concentration of reactants
C.
Changing the temperature
D.
Changing the pressure
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Solution
A catalyst speeds up the rate of reaching equilibrium but does not change the position of equilibrium or the equilibrium constant.
Correct Answer: A — Adding a catalyst
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Q. Which of the following changes will shift the equilibrium to the right for the reaction: N2(g) + 3H2(g) ⇌ 2NH3(g)?
A.
Increase in pressure
B.
Decrease in temperature
C.
Increase in volume
D.
Addition of NH3
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Solution
Increasing pressure shifts the equilibrium to the side with fewer moles of gas, which is the right side in this case.
Correct Answer: A — Increase in pressure
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Q. Which of the following factors does NOT affect the equilibrium constant (K) of a reaction?
A.
Temperature
B.
Concentration of reactants
C.
Pressure
D.
Nature of reactants and products
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Solution
The equilibrium constant K is only affected by temperature. Changes in concentration or pressure will shift the position of equilibrium but not change the value of K.
Correct Answer: B — Concentration of reactants
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Q. Which of the following factors does NOT affect the equilibrium constant (K)?
A.
Temperature
B.
Concentration of reactants
C.
Pressure
D.
Nature of reactants and products
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Solution
The equilibrium constant K is only affected by temperature. Changes in concentration or pressure will shift the position of equilibrium but not change the value of K.
Correct Answer: B — Concentration of reactants
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Q. Which of the following statements about the equilibrium constant (K) is true?
A.
K changes with temperature
B.
K changes with concentration
C.
K is always greater than 1
D.
K is independent of pressure
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Solution
The equilibrium constant K is dependent on temperature; it changes if the temperature of the system changes.
Correct Answer: A — K changes with temperature
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Q. Which of the following statements is true about a system at equilibrium?
A.
The concentrations of reactants and products are equal
B.
The rate of the forward reaction equals the rate of the reverse reaction
C.
No reactions occur
D.
The system is at rest
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Solution
At equilibrium, the rates of the forward and reverse reactions are equal, not necessarily the concentrations.
Correct Answer: B — The rate of the forward reaction equals the rate of the reverse reaction
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Q. Which of the following statements is true about the equilibrium constant Kp?
A.
Kp is always equal to Kc
B.
Kp depends on temperature
C.
Kp is independent of pressure
D.
Kp is always greater than Kc
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Solution
Kp is dependent on temperature and can vary with changes in temperature.
Correct Answer: B — Kp depends on temperature
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Q. Which of the following statements is true regarding the equilibrium constant Kc?
A.
Kc is temperature dependent
B.
Kc is pressure dependent
C.
Kc is concentration dependent
D.
Kc is independent of the reaction
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Solution
The equilibrium constant Kc is dependent on temperature; changing the temperature will change the value of Kc.
Correct Answer: A — Kc is temperature dependent
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