Equilibrium Position in Chemical Reactions

This video tutorial covers part three of topic six on chemical reactions from the Cambridge IGCSE syllabus. It explains reversible reactions and equilibrium, including the concept of equilibrium in closed systems. The video discusses hydrated and anhydrous compounds, their transformations, and the effects of heat and water. It also explores factors affecting equilibrium, such as temperature, pressure, and concentration, and how these changes shift the equilibrium position. The role of catalysts in speeding up reactions without affecting equilibrium is also highlighted. The video concludes with a call to action for viewers to engage with the channel.

What is the main characteristic of a reversible reaction?

• It is always exothermic.

• It requires a catalyst to occur.

• The products can react to form the original reactants.

• It only proceeds in one direction.

What happens to hydrated copper(II) sulfate when it is heated?

• It becomes hydrated and turns blue.

• It remains unchanged.

• It dissolves in water.

• It becomes anhydrous and turns white.

How does adding water to anhydrous cobalt(II) chloride affect its form?

• It becomes hydrated and turns blue.

• It becomes hydrated and turns pink.

• It becomes anhydrous and turns blue.

• It remains anhydrous and turns pink.

What effect does raising the temperature have on a reversible reaction where the forward reaction is endothermic?

• It has no effect on the equilibrium.

• It stops the reaction completely.

• It shifts the equilibrium towards the endothermic reaction.

• It shifts the equilibrium towards the exothermic reaction.

In a gaseous reaction, what happens to the equilibrium position when pressure is increased?

• It shifts towards the side with more gas molecules.

• It shifts towards the side with fewer gas molecules.

• It remains unchanged.

• It shifts towards the side with equal gas molecules.

What is the effect of decreasing the pressure on a reaction with more gas molecules on the reactant side?

• Equilibrium shifts to the right.

• Equilibrium shifts to the left.

• Equilibrium remains unchanged.

• Equilibrium shifts to the side with fewer gas molecules.

How does increasing the concentration of reactants affect the equilibrium position?

• It shifts towards the reactants.

• It shifts towards the side with fewer molecules.

• It shifts towards the products.

• It remains unchanged.

What is the role of a catalyst in a chemical reaction at equilibrium?

• It changes the position of equilibrium.

• It increases the rate of reaction without affecting equilibrium.

• It decreases the rate of reaction.

• It stops the reaction from reaching equilibrium.

What happens to the equilibrium position if the concentration of products is too high?

• It shifts towards the reactants.

• It remains unchanged.

• It shifts towards the products.

• It shifts towards the side with more molecules.

Which of the following does not affect the position of equilibrium?

• Pressure changes

• Temperature changes

• Concentration changes

• Catalyst addition