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ACSEE (Form 6) Chemical Equilibrium — practice questions

Explore 8 free Chemical Equilibrium questions in ACSEE (Form 6) Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Chemical Equilibrium questions and exercises with answers

Showing questions 1–8 of 8.

A sealed flask of reacting gases shows no colour change for an hour. What is actually happening inside?Read the answer and worked solution →Adding a catalyst to a reversible reaction at equilibrium:Read the answer and worked solution →When the temperature of an exothermic reaction at equilibrium is raised, the equilibrium constant:Read the answer and worked solution →The solubility of carbon dioxide in a soft drink falls as temperature rises because dissolving is:Read the answer and worked solution →Does it shift the equilibrium?Read the answer and worked solution →Fault the false equilibrium claimsRead the answer and worked solution →Equilibrium, true or falseRead the answer and worked solution →Predict the shiftRead the answer and worked solution →

Worked practice questions

A sealed flask of reacting gases shows no colour change for an hour. What is actually happening inside?

  1. only the forward reaction still proceeds
  2. both reactions have completely stopped
  3. both reactions continue at equal rates
  4. the concentrations keep changing steadily
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Correct answer: C. both reactions continue at equal rates

1. Equilibrium is reached when the forward and reverse rates become equal. 2. Equal rates mean the concentrations stop changing, which is what is observed. 3. But neither reaction has stopped — both continue at the molecular level. 4. Product forms exactly as fast as it is consumed, so the system appears still while remaining active. 5. That ongoing activity beneath an unchanging appearance is exactly what dynamic describes. _Source: NECTA ACSEE 2023 Chemistry 132/1, Question 8: Chemical Equilibrium_

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Adding a catalyst to a reversible reaction at equilibrium:

  1. shifts the position towards the products
  2. shifts the position towards the reactants
  3. leaves the position of equilibrium unchanged
  4. raises the value of the equilibrium constant
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Correct answer: C. leaves the position of equilibrium unchanged

1. A catalyst provides an alternative route with a lower activation energy. 2. That route is available to the forward and the reverse reaction alike. 3. So both rates increase by the same factor and remain equal to one another. 4. Equilibrium is therefore reached sooner, but at exactly the same position. 5. The equilibrium constant depends only on temperature, so a catalyst cannot change it either. _Source: NECTA ACSEE 2023 Chemistry 132/1, Question 8: Chemical Equilibrium_

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When the temperature of an exothermic reaction at equilibrium is raised, the equilibrium constant:

  1. increases, favouring the products
  2. decreases, favouring the reactants
  3. stays the same, since K is fixed
  4. doubles for every 10 K rise
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Correct answer: B. decreases, favouring the reactants

1. For an exothermic reaction, heat can be treated as a product. 2. Raising the temperature adds heat, so by Le Chatelier's principle the system shifts to remove it. 3. That shift moves the position backwards, towards the reactants. 4. Since the equilibrium mixture now holds more reactant and less product, $K$ falls. 5. Temperature is the one factor that does change $K$, which is why a catalyst or a pressure change cannot. _Source: NECTA ACSEE 2023 Chemistry 132/1, Question 8: Chemical Equilibrium_

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More Chemistry topics

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