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Equilibrium

Description: This quiz covers the fundamental concepts of equilibrium in chemistry.
Number of Questions: 14
Created by:
Tags: equilibrium chemical reactions thermodynamics
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What is the state of a system in which the concentrations of reactants and products do not change over time?

  1. Equilibrium

  2. Non-equilibrium

  3. Dynamic equilibrium

  4. Steady state

Show answer
Correct Option: A
Explanation:

Equilibrium is a state of balance in which the concentrations of reactants and products remain constant over time.

Which of the following factors can shift the equilibrium position of a reaction?

  1. Temperature

  2. Pressure

  3. Concentration of reactants

  4. All of the above

Show answer
Correct Option: D
Explanation:

Temperature, pressure, and concentration of reactants can all shift the equilibrium position of a reaction.

What is the relationship between the equilibrium constant (K) and the concentrations of reactants and products at equilibrium?

  1. K = [products]/[reactants]

  2. K = [reactants]/[products]

  3. K = [products]^2/[reactants]^2

  4. K = [reactants]^2/[products]^2

Show answer
Correct Option: A
Explanation:

The equilibrium constant (K) is equal to the ratio of the concentrations of products and reactants at equilibrium.

What is the relationship between the standard free energy change (ΔG°) and the equilibrium constant (K)?

  1. ΔG° = -RTlnK

  2. ΔG° = RTlnK

  3. ΔG° = -RTK

  4. ΔG° = RTK

Show answer
Correct Option: A
Explanation:

The standard free energy change (ΔG°) is related to the equilibrium constant (K) by the equation ΔG° = -RTlnK.

Which of the following reactions is an example of a homogeneous equilibrium?

  1. CaCO3(s) <=> CaO(s) + CO2(g)

  2. H2(g) + Cl2(g) <=> 2HCl(g)

  3. Fe(s) + CuSO4(aq) <=> FeSO4(aq) + Cu(s)

  4. CH3COOH(aq) + H2O(l) <=> CH3COO-(aq) + H3O+(aq)

Show answer
Correct Option: B
Explanation:

A homogeneous equilibrium is a reaction in which all of the reactants and products are in the same phase. In the reaction H2(g) + Cl2(g) <=> 2HCl(g), all of the reactants and products are gases.

Which of the following reactions is an example of a heterogeneous equilibrium?

  1. CaCO3(s) <=> CaO(s) + CO2(g)

  2. H2(g) + Cl2(g) <=> 2HCl(g)

  3. Fe(s) + CuSO4(aq) <=> FeSO4(aq) + Cu(s)

  4. CH3COOH(aq) + H2O(l) <=> CH3COO-(aq) + H3O+(aq)

Show answer
Correct Option: A
Explanation:

A heterogeneous equilibrium is a reaction in which the reactants and products are in different phases. In the reaction CaCO3(s) <=> CaO(s) + CO2(g), the reactants are in the solid phase and the product is in the gas phase.

What is the effect of increasing temperature on the equilibrium position of an exothermic reaction?

  1. The equilibrium position shifts to the left.

  2. The equilibrium position shifts to the right.

  3. The equilibrium position does not change.

  4. The equilibrium position cannot be determined.

Show answer
Correct Option: A
Explanation:

According to Le Chatelier's principle, if a reaction is exothermic (ΔH° < 0), increasing the temperature will shift the equilibrium position to the left, favoring the reactants.

What is the effect of increasing temperature on the equilibrium position of an endothermic reaction?

  1. The equilibrium position shifts to the left.

  2. The equilibrium position shifts to the right.

  3. The equilibrium position does not change.

  4. The equilibrium position cannot be determined.

Show answer
Correct Option: B
Explanation:

According to Le Chatelier's principle, if a reaction is endothermic (ΔH° > 0), increasing the temperature will shift the equilibrium position to the right, favoring the products.

What is the effect of increasing pressure on the equilibrium position of a reaction in which the number of moles of gas on the product side is greater than the number of moles of gas on the reactant side?

  1. The equilibrium position shifts to the left.

  2. The equilibrium position shifts to the right.

  3. The equilibrium position does not change.

  4. The equilibrium position cannot be determined.

Show answer
Correct Option: A
Explanation:

According to Le Chatelier's principle, if a reaction involves a decrease in the number of moles of gas, increasing the pressure will shift the equilibrium position to the side with fewer moles of gas, which is the reactant side.

What is the effect of increasing pressure on the equilibrium position of a reaction in which the number of moles of gas on the product side is less than the number of moles of gas on the reactant side?

  1. The equilibrium position shifts to the left.

  2. The equilibrium position shifts to the right.

  3. The equilibrium position does not change.

  4. The equilibrium position cannot be determined.

Show answer
Correct Option: B
Explanation:

According to Le Chatelier's principle, if a reaction involves an increase in the number of moles of gas, increasing the pressure will shift the equilibrium position to the side with more moles of gas, which is the product side.

Which of the following is a common ion effect?

  1. The addition of a salt containing a common ion to a solution decreases the solubility of a sparingly soluble salt.

  2. The addition of a salt containing a common ion to a solution increases the solubility of a sparingly soluble salt.

  3. The addition of a salt containing a common ion to a solution has no effect on the solubility of a sparingly soluble salt.

  4. The addition of a salt containing a common ion to a solution can either increase or decrease the solubility of a sparingly soluble salt, depending on the specific salt.

Show answer
Correct Option: A
Explanation:

The common ion effect is the decrease in the solubility of a sparingly soluble salt when a salt containing a common ion is added to the solution.

Which of the following is a buffer solution?

  1. A solution that contains a weak acid and its conjugate base.

  2. A solution that contains a weak base and its conjugate acid.

  3. A solution that contains both a weak acid and a weak base.

  4. A solution that contains a salt of a weak acid and a strong base.

Show answer
Correct Option: A
Explanation:

A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added to it. Buffer solutions typically contain a weak acid and its conjugate base or a weak base and its conjugate acid.

What is the pH of a buffer solution?

  1. The pH of a buffer solution is equal to the pKa of the weak acid.

  2. The pH of a buffer solution is equal to the pKb of the weak base.

  3. The pH of a buffer solution is equal to the average of the pKa and pKb of the weak acid and weak base.

  4. The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation.

Show answer
Correct Option: D
Explanation:

The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the weak acid.

What is the role of a catalyst in an equilibrium reaction?

  1. A catalyst increases the rate of the forward reaction.

  2. A catalyst increases the rate of the reverse reaction.

  3. A catalyst increases the rate of both the forward and reverse reactions.

  4. A catalyst does not affect the rate of the reaction.

Show answer
Correct Option: C
Explanation:

A catalyst increases the rate of both the forward and reverse reactions by providing an alternative pathway for the reaction to occur. This lowers the activation energy of the reaction and allows it to proceed more quickly.

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