Q. For the reaction 2A(g) ⇌ B(g) + C(g), if the concentration of B is increased, what will happen to the equilibrium?
A.
Shift to the left
B.
Shift to the right
C.
No shift
D.
Depends on temperature
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Solution
Increasing the concentration of a product shifts the equilibrium to the left to counteract the change.
Correct Answer: A — Shift to the left
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Q. For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), if the concentration of SO2 is doubled, what happens to the equilibrium constant?
A.
It doubles
B.
It remains the same
C.
It halves
D.
It quadruples
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Solution
The equilibrium constant Kc is only affected by temperature, not by changes in concentration.
Correct Answer: B — It remains the same
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Q. For the reaction 4H2(g) + 2O2(g) ⇌ 4H2O(g), what is the change in Gibbs free energy at equilibrium?
A.
Positive
B.
Negative
C.
Zero
D.
Depends on temperature
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Solution
At equilibrium, the change in Gibbs free energy (ΔG) is zero.
Correct Answer: C — Zero
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Q. For the reaction 4HCl(g) ⇌ 2H2(g) + Cl2(g), what is the effect of adding HCl on the equilibrium?
A.
Shift to the left
B.
Shift to the right
C.
No effect
D.
Depends on the temperature
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Solution
Adding more HCl will increase the concentration of reactants, causing the equilibrium to shift to the left to consume the added HCl.
Correct Answer: A — Shift to the left
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Q. For the reaction A(g) ⇌ B(g), if the concentration of A is increased, what will happen to the concentration of B at equilibrium?
A.
Increase
B.
Decrease
C.
Remain the same
D.
Cannot be determined
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Solution
Increasing the concentration of A will shift the equilibrium to the right, resulting in an increase in the concentration of B.
Correct Answer: A — Increase
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Q. For the reaction A(g) ⇌ B(g), if the concentration of B is increased, what will happen to the concentration of A at equilibrium?
A.
Increase
B.
Decrease
C.
Remain the same
D.
Cannot be determined
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Solution
According to Le Chatelier's principle, increasing the concentration of a product will shift the equilibrium to the left, decreasing the concentration of A.
Correct Answer: B — Decrease
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Q. For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what is the effect of increasing the concentration of H2?
A.
Shifts equilibrium to the right
B.
Shifts equilibrium to the left
C.
No effect
D.
Increases the rate of reaction
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Solution
Increasing the concentration of H2 will shift the equilibrium to the right to produce more CH3OH, according to Le Chatelier's principle.
Correct Answer: A — Shifts equilibrium to the right
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Q. For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if H2 is removed from the system?
A.
Shifts to the right
B.
Shifts to the left
C.
No change
D.
Increases the rate of reaction
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Solution
Removing a reactant (H2) will shift the equilibrium position to the left to produce more reactants.
Correct Answer: B — Shifts to the left
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Q. For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the concentration of H2 is increased?
A.
Equilibrium shifts to the left
B.
Equilibrium shifts to the right
C.
No change
D.
Rate of reaction decreases
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Solution
Increasing the concentration of H2 will shift the equilibrium to the right to produce more CH3OH, according to Le Chatelier's principle.
Correct Answer: B — Equilibrium shifts to the right
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Q. For the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), what will happen if the pressure is increased?
A.
Equilibrium shifts to the left
B.
Equilibrium shifts to the right
C.
No change in equilibrium
D.
Equilibrium constant increases
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Solution
Increasing pressure favors the side with fewer moles of gas. In this case, the right side has 1 mole of CH3OH compared to 3 moles on the left, so the equilibrium shifts to the right.
Correct Answer: B — Equilibrium shifts to the right
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Q. For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens if the volume of the container is decreased?
A.
Equilibrium shifts to the left
B.
Equilibrium shifts to the right
C.
No change in equilibrium
D.
Equilibrium constant changes
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Solution
Decreasing the volume increases the pressure, and according to Le Chatelier's principle, the equilibrium will shift towards the side with fewer moles of gas, which is the right side in this case.
Correct Answer: B — Equilibrium shifts to the right
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Q. For the reaction N2(g) + 3H2(g) ⇌ 2NH3(g), what happens to the equilibrium constant if the temperature is increased?
A.
Increases
B.
Decreases
C.
Remains the same
D.
Depends on the pressure
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Solution
For exothermic reactions, increasing the temperature shifts the equilibrium to the left, thus decreasing the equilibrium constant.
Correct Answer: B — Decreases
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Q. For the reaction: 3A(g) ⇌ 2B(g) + C(g), what is the expression for Kp?
A.
(P_B^2 * P_C) / (P_A^3)
B.
(P_A^3) / (P_B^2 * P_C)
C.
(P_C) / (P_A^3)
D.
(P_B^2) / (P_A^3)
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Solution
The equilibrium constant Kp is expressed as Kp = (P_B^2 * P_C) / (P_A^3).
Correct Answer: A — (P_B^2 * P_C) / (P_A^3)
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Q. For the reaction: A(g) ⇌ B(g) + C(g), if the concentration of A is increased, what will happen to the equilibrium position?
A.
Shift to the left
B.
Shift to the right
C.
No change
D.
Depends on temperature
Show solution
Solution
According to Le Chatelier's principle, increasing the concentration of a reactant will shift the equilibrium to the right.
Correct Answer: B — Shift to the right
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Q. If the concentration of reactants is increased in a system at equilibrium, what will happen to the position of equilibrium?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Depends on temperature
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Solution
According to Le Chatelier's principle, increasing the concentration of reactants will shift the equilibrium position to the right, favoring the formation of products.
Correct Answer: A — Shift to the right
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Q. If the equilibrium constant Kc for a reaction is 10 at a certain temperature, what is the value of Kc for the reverse reaction?
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Solution
The equilibrium constant for the reverse reaction is the reciprocal of the forward reaction, so Kc' = 1/Kc = 0.1.
Correct Answer: A — 0.1
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Q. If the equilibrium constant Kc for a reaction is 10, what can be said about the position of equilibrium?
A.
Products are favored
B.
Reactants are favored
C.
Equilibrium is at the center
D.
No conclusion can be drawn
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Solution
A Kc value greater than 1 indicates that the products are favored at equilibrium.
Correct Answer: A — Products are favored
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Q. If the forward reaction is exothermic, what effect does increasing the temperature have on the equilibrium position?
A.
Shifts to the right
B.
Shifts to the left
C.
No effect
D.
Increases the rate of reaction
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Solution
According to Le Chatelier's principle, increasing the temperature of an exothermic reaction shifts the equilibrium position to the left, favoring the reactants.
Correct Answer: B — Shifts to the left
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Q. In a closed system, if the volume is decreased, what will happen to the equilibrium of the reaction 2A(g) + B(g) ⇌ 3C(g)?
A.
Shift to the left
B.
Shift to the right
C.
No change
D.
Depends on temperature
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Solution
Decreasing the volume increases the pressure, and the equilibrium will shift towards the side with fewer moles of gas, which is the left side.
Correct Answer: A — Shift to the left
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Q. In a dynamic equilibrium, which of the following statements is true?
A.
The rates of the forward and reverse reactions are equal
B.
The concentrations of reactants and products are equal
C.
The reaction has stopped
D.
The system is at rest
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Solution
In a dynamic equilibrium, the rates of the forward and reverse reactions are equal, but the concentrations of reactants and products may not be equal.
Correct Answer: A — The rates of the forward and reverse reactions are equal
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Q. In a reaction at equilibrium, if the concentration of products is decreased, what will happen?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Depends on the temperature
Show solution
Solution
Decreasing the concentration of products will shift the equilibrium to the right to produce more products, according to Le Chatelier's principle.
Correct Answer: A — Shift to the right
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Q. In a reaction at equilibrium, if the temperature is decreased, what will happen to the equilibrium position if the reaction is exothermic?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Depends on the concentration
Show solution
Solution
For an exothermic reaction, decreasing the temperature shifts the equilibrium to the right, favoring the formation of products.
Correct Answer: A — Shift to the right
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Q. In a reaction at equilibrium, if the temperature is increased, what will happen to the equilibrium constant Kc for an endothermic reaction?
A.
Increase
B.
Decrease
C.
No change
D.
Depends on concentration
Show solution
Solution
For an endothermic reaction, increasing temperature shifts the equilibrium to the right, increasing Kc.
Correct Answer: A — Increase
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Q. In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the concentration of SO2?
A.
Shifts to the right
B.
Shifts to the left
C.
No effect
D.
Increases the rate of reaction
Show solution
Solution
Increasing the concentration of a reactant shifts the equilibrium position to the right, favoring the formation of products (SO3).
Correct Answer: A — Shifts to the right
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Q. In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what is the effect of increasing the pressure on the equilibrium?
A.
Shift to the left
B.
Shift to the right
C.
No effect
D.
Depends on the temperature
Show solution
Solution
Increasing the pressure will shift the equilibrium towards the side with fewer moles of gas, which is the right side in this case (2 moles of SO3).
Correct Answer: B — Shift to the right
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Q. In the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), what will happen if SO3 is removed from the system?
A.
Equilibrium shifts to the left
B.
Equilibrium shifts to the right
C.
No change
D.
Equilibrium constant increases
Show solution
Solution
Removing SO3 will shift the equilibrium to the right to produce more SO3, according to Le Chatelier's principle.
Correct Answer: B — Equilibrium shifts to the right
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Q. In the reaction CO(g) + 2H2(g) ⇌ CH3OH(g), if the pressure is increased, which direction will the equilibrium shift?
A.
To the left
B.
To the right
C.
No shift
D.
Depends on temperature
Show solution
Solution
Increasing pressure shifts the equilibrium towards the side with fewer moles of gas, which is the right side in this case.
Correct Answer: B — To the right
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Q. In the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g), what happens if the temperature is increased?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Increase in Kp
Show solution
Solution
If the reaction is exothermic, increasing the temperature will shift the equilibrium to the left, favoring the reactants.
Correct Answer: B — Shift to the left
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Q. What happens to the equilibrium constant if the reaction is reversed?
A.
K remains the same
B.
K is doubled
C.
K is inverted
D.
K is halved
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Solution
When a reaction is reversed, the equilibrium constant for the reverse reaction is the reciprocal of the equilibrium constant for the forward reaction.
Correct Answer: C — K is inverted
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Q. What happens to the equilibrium constant when a reaction is reversed?
A.
It remains the same
B.
It doubles
C.
It is inverted
D.
It is halved
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Solution
When a reaction is reversed, the equilibrium constant is inverted (1/K).
Correct Answer: C — It is inverted
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