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Chemical Equilibrium

This quiz covers the fundamental concepts of equilibrium in chemistry.

14 Questions Published
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Questions

Question 1 Multiple Choice (Single Answer)

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
Question 2 Multiple Choice (Single Answer)

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
Question 3 Multiple Choice (Single Answer)

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
Question 4 Multiple Choice (Single Answer)

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
Question 5 Multiple Choice (Single Answer)

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)
Question 6 Multiple Choice (Single Answer)

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)
Question 7 Multiple Choice (Single Answer)

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.
Question 8 Multiple Choice (Single Answer)

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.
Question 9 Multiple Choice (Single Answer)

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.
Question 10 Multiple Choice (Single Answer)

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.
Question 11 Multiple Choice (Single Answer)

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.
Question 12 Multiple Choice (Single Answer)

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.
Question 13 Multiple Choice (Single Answer)

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.
Question 14 Multiple Choice (Single Answer)

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.
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