Unit 3 AOS 2 - Equilibrium and Reaction Dynamics Quiz (2B)

What is the main difference between reversible and irreversible reactions?

• Reversible reactions can only occur in one direction.

• Irreversible reactions can reach equilibrium.

• Reversible reactions can proceed in both forward and reverse directions.

• Irreversible reactions can change the position of equilibrium.

Which of the following best describes the dynamic nature of homogeneous equilibria?

• The concentrations of reactants and products remain constant over time.

• The reaction stops once equilibrium is reached.

• The forward and reverse reactions continue to occur at equal rates.

• The reaction only proceeds in the forward direction.

How does an increase in temperature generally affect the position of equilibrium in an exothermic reaction?

• It shifts the equilibrium to the right.

• It shifts the equilibrium to the left.

• It has no effect on the equilibrium position.

• It increases the concentration of reactants.

According to Le Chatelier’s principle, what happens to the equilibrium position when the concentration of a reactant is increased?

• The equilibrium shifts to the left.

• The equilibrium shifts to the right.

• The equilibrium remains unchanged.

• The equilibrium constant decreases.

• It is dependent on the concentration of reactants and products.

• It changes with the temperature of the system.

• It is always equal to 1 at equilibrium.

• It is independent of the reaction equation.

• The rate of the reaction.

• The equilibrium constant at a given temperature.

• The relative amounts of products and reactants at a specific time.

• The total energy change of the reaction.

Which factor is NOT considered when applying Le Chatelier’s principle to maximise the yield of a chemical reaction?

• Temperature

• Pressure

• Catalyst

• Concentration

• It depends on the stoichiometry of the reaction.

• It is always unitless.

How does the use of a catalyst align with the green chemistry principle of designing for energy efficiency?

• It increases the equilibrium constant.

• It lowers the activation energy, reducing energy consumption.

• It shifts the equilibrium position to the right.

• It increases the concentration of reactants.

What is the effect of decreasing the volume of a gaseous equilibrium system?

• The equilibrium shifts towards the side with more moles of gas.

• The equilibrium shifts towards the side with fewer moles of gas.

• The equilibrium constant increases.

• The equilibrium constant decreases.