Question 1: Define a reversible reaction and explain how it differs from an irreversible reaction.

Answer: A reversible reaction is a chemical process where the products can convert back into the original reactants under certain conditions, unlike an irreversible reaction which proceeds in only one direction.

Question 2: Describe the mechanism that allows a reversible reaction to reach equilibrium.

Answer: In a reversible reaction, forward and backward reactions occur simultaneously. When the rates are equal, the system reaches chemical equilibrium where the concentrations of reactants and products remain constant.

Question 3: What is meant by 'dynamic equilibrium' in the context of reversible reactions?

Answer: Dynamic equilibrium is a state where the forward and backward reactions happen at the same rate, so the concentrations of reactants and products stay constant over time.

Question 1: A reversible reaction has a forward rate of 0.05 mol/L·s and a backward rate of 0.05 mol/L·s at equilibrium. What is the reaction rate at equilibrium?

Answer: 0.05 mol/L·s

Question 2: If the concentration of reactant A decreases from 1.0 M to 0.6 M over 10 minutes, calculate the average rate of the reaction in mol/L·min.

Answer: (1.0 - 0.6) mol/L ÷ 10 min = 0.04 mol/L·min

Question 1: Describe a simple experimental setup to demonstrate a reversible reaction in the laboratory. Include the key variables that should be controlled.

Answer: Use a system like the reaction between iodine and starch, where temperature or concentration can be varied. Control variables include temperature, concentration of reactants, and agitation to observe the reversible nature.

Question 2: Identify two safety precautions to consider when conducting experiments involving reversible reactions.

Answer: Wear appropriate protective equipment such as gloves and goggles, and ensure proper ventilation to avoid inhaling fumes.

Question 1: A reversible reaction reaches equilibrium after 30 minutes with concentrations of 0.8 M of reactant and 0.2 M of product. If the reaction conditions are changed to increase temperature, describe what likely happens to the concentrations at equilibrium and why.

Answer: Increasing temperature may shift the equilibrium depending on whether the reaction is endothermic or exothermic. Typically, if the reaction is endothermic, the concentration of reactant may increase and the product decrease; if exothermic, the opposite may occur, due to Le Châtelier's principle.

Question 1: Explain how the Haber process for ammonia synthesis is an example of a reversible reaction and why it is important for industrial production.

Answer: The Haber process is a reversible reaction between nitrogen and hydrogen gases to produce ammonia. It is important because it allows for the continuous synthesis and recycling of reactants to maximize ammonia yield, essential for fertilizers.

Question 2: Describe how reversible reactions play a role in carbon dioxide capture technology used to reduce greenhouse gases.

Answer: Reversible reactions, such as absorption and desorption of CO2 in chemical scrubbers, allow CO2 to be captured from emissions and later released for storage or reuse, aiding in reducing greenhouse gases.