GCSE Chemistry - Reversible Reactions and Equilibrium #49

The video tutorial explains the concept of chemical equilibrium, focusing on reversible reactions. It describes how forward and backward reactions occur at different rates and how equilibrium is achieved when these rates equalize. The position of equilibrium can shift based on conditions like temperature. The tutorial also covers the exothermic and endothermic nature of reversible reactions, using the example of hydrated and anhydrous copper sulphate. A closed system is necessary for equilibrium to be reached. The video concludes with a recap of key points.

What does a double arrow in a chemical equation signify?

• An irreversible reaction

• A completed reaction

• A reversible reaction

• A one-way reaction

At equilibrium, what happens to the concentrations of reactants and products?

• They become equal

• They decrease

• They increase

• They stop changing

What determines the position of equilibrium in a chemical reaction?

• The initial concentrations

• The temperature and pressure

• The color of the reactants

• The presence of a catalyst

How does adding heat to a reaction affect the position of equilibrium?

• It shifts to the left

• It shifts to the right

• It becomes undefined

• It remains unchanged

What is required for a reversible reaction to reach equilibrium?

• A high concentration of reactants

• An open system

• A low concentration of products

• A closed system

In a reversible reaction, if the forward reaction is endothermic, what is true about the backward reaction?

• It requires a catalyst

• It is exothermic

• It is also endothermic

• It does not occur

What happens to hydrated copper sulphate when it is heated?

• It remains unchanged

• It turns into blue crystals

• It forms anhydrous copper sulphate

• It dissolves in water