NEET Chemistry: Equilibrium Practice Questions
15 free multiple-choice questions on Equilibrium for NEET Chemistry, each with the correct answer and a step-by-step explanation. Attempt a question, then reveal the solution to check your reasoning.
Practice thousands more Equilibrium questions in the app →Q1. For the equilibrium A(g) + B(g) ⇌ C(g) + D(g), if the concentration of reactant A is increased, the equilibrium will shift towards which side?
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Correct answer: B — The right side (products)
According to Le Chatelier's principle, if the concentration of a reactant (A) is increased, the system attempts to counteract this change by consuming the added reactant. This causes the equilibrium to shift in the forward direction to consume A and form more products.
Q2. In an equilibrium reaction, the value of the equilibrium constant (K_c) is directly related to the ratio of which quantities?
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Correct answer: A — Concentrations of reactants and products
The equilibrium constant (K_c) is the ratio of the product concentrations to the reactant concentrations at equilibrium.
Q3. If the system is at equilibrium, what does this imply about the net change in the amount of substance over time?
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Correct answer: C — There is no net change in the amount of substance
Equilibrium, whether static or dynamic, implies that the macroscopic properties, such as the total amount of substance, are constant over time.
Q4. A solution has a pH of 12. What is the nature of this solution?
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Correct answer: D — Strongly basic
A pH greater than 7 indicates a basic solution. Since 12 > 7, the solution is strongly basic.
Q5. What is the definition of pH in terms of hydrogen ion concentration?
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Correct answer: C — pH = [H⁺]
pH is defined as the negative logarithm (base 10) of the hydrogen ion concentration, i.e., pH = -log[H⁺].
Q6. When a product is removed from a system at equilibrium, the system will shift to:
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Correct answer: B — The right side (products).
If a product is removed, the system attempts to replace the removed product by shifting the equilibrium to the right, thus increasing the concentration of the remaining products to re-establish equilibrium.
Q7. The concentration of hydrogen ions (H⁺) in a solution is directly proportional to which measure?
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Correct answer: D — The electrical conductivity of the solution
The concentration of H⁺ ions dictates the acidity. Higher H⁺ concentration corresponds to higher acidity and, consequently, a lower pH (or higher pOH).
Q8. In a system that is at dynamic equilibrium, which of the following statements is true regarding the reaction rates?
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Correct answer: B — The rate of the forward reaction is equal to the rate of the reverse reaction
Dynamic equilibrium is a state where the rates of the forward and reverse reactions are equal, meaning the concentrations of reactants and products remain constant, but the reactions themselves are still occurring at equal rates.
Q9. Which of the following statements is true regarding the behavior of an acidic solution compared to a basic solution?
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Correct answer: B — Acidic solutions have a lower pH than basic solutions.
Acidic solutions have a higher concentration of H⁺ ions (and lower OH⁻ concentration) compared to basic solutions. Lower pH corresponds to higher acidity.
Q10. Which of the following changes will favor the forward reaction in the equilibrium A + B ⇌ C if the forward reaction is endothermic?
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Correct answer: D — Increasing the temperature.
For an endothermic reaction (where heat is a reactant), increasing the temperature shifts the equilibrium to the right (forward direction) to consume the added heat.
Q11. In a system undergoing a reversible chemical reaction, what is the defining characteristic of dynamic equilibrium?
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Correct answer: D — The forward and reverse reaction rates are equal
Dynamic equilibrium is a state where the forward and reverse reaction rates are equal, meaning the net concentrations of reactants and products remain constant, even though the reactions are still occurring simultaneously.
Q12. Which of the following best describes the state of concentrations of reactants and products when a system is at dynamic equilibrium?
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Correct answer: A — The concentrations of all species remain constant
In dynamic equilibrium, although reactions are still occurring, the net change in concentrations of reactants and products is zero, meaning their concentrations are constant over time.
Q13. If a reaction is at equilibrium, it implies that the system is reversible. What does reversibility mean in this context?
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Correct answer: D — The forward and reverse reactions are occurring simultaneously
Reversibility means that both the forward and reverse reactions are simultaneously taking place, establishing the balance necessary for equilibrium.
Q14. A solution with a pH of 7 is considered which type of solution?
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Correct answer: B — Neutral
A pH of 7 signifies that the concentration of hydrogen ions is 10⁻⁷ M, which is the definition of a neutral solution.
Q15. If the concentration of a product is reduced in a system at equilibrium, the system will adjust by shifting the equilibrium towards:
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Correct answer: B — The side with higher concentration of products
Reducing the concentration of a product creates a stress. The system compensates by shifting the reaction in the forward direction (towards the products) to replenish the reduced reactant, thereby increasing the product concentration.
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