Question 1: A reversible reaction is a chemical reaction where the reactants can form products, and those products can also react to form the original reactants. This process can reach a state called dynamic equilibrium. Explain in your own words what is meant by 'dynamic equilibrium' in reversible reactions.

Answer: Dynamic equilibrium is a state in a reversible reaction where the forward and reverse reactions occur at the same rate, resulting in no overall change in concentration of reactants and products.

Question 1: Describe the difference between a reversible reaction and an irreversible reaction.

Answer: A reversible reaction can proceed in both directions and reach equilibrium, while an irreversible reaction proceeds in only one direction, forming products that do not revert back.

Question 2: In a reversible reaction, what does the term 'closed system' mean and why is it important?

Answer: A closed system is one where no reactants or products can enter or leave, which is important for maintaining the conditions necessary for the reaction to reach equilibrium.

Question 1: A reversible reaction has a forward rate constant (k") of 0.05 mol/L·s and a reverse rate constant (k") of 0.03 mol/L·s. Calculate the ratio of the concentrations of products to reactants at equilibrium using the expression K".

Answer: K" = 0.05 / 0.03 = 1.67

Question 1: Describe a simple experiment to demonstrate the concept of a reversible reaction, including the main variables you would control.

Answer: One possible experiment involves the reaction between iodine and starch in a solution where the reaction can be reversed by changing conditions such as temperature or concentration. Control variables include temperature, concentration of reactants, and pH. Safety precautions involve handling chemicals with gloves and eye protection.

Question 1: In an experiment, the concentration of reactant A decreases initially while the concentration of product B increases. After some time, both concentrations stabilise. Explain what this indicates about the reaction system.

Answer: This indicates the reaction has reached equilibrium, where the rates of the forward and reverse reactions are equal, resulting in stable concentrations.

Question 1: Explain how the concept of reversible reactions is utilised in the Haber process for ammonia production, and why controlling reaction conditions is important.

Answer: In the Haber process, nitrogen and hydrogen react reversibly to form ammonia. Controlling temperature and pressure shifts the equilibrium position to optimise ammonia yield. High pressure favours the forward reaction, and an iron catalyst speeds up the process while maintaining a manageable reaction rate.