Question 1: Define a reversible reaction in your own words.

Answer: A reaction where the reactants can convert to products and the products can convert back to reactants under certain conditions.

Question 2: Explain the concept of dynamic equilibrium in reversible reactions.

Answer: Dynamic equilibrium occurs when the forward and reverse reactions happen at the same rate, so the concentrations of reactants and products remain constant over time.

Question 1: Given that the concentration of reactant A decreases from 0.5 mol/L to 0.3 mol/L in 10 seconds during a reversible reaction, calculate the rate of the forward reaction in mol/(L·s).

Answer: 0.02 mol/(L·s)

Question 2: The equilibrium constant (Kc) for a reaction is calculated using the formula Kc = [Products]/[Reactants]. If at equilibrium, the concentration of products is 0.8 mol/L and reactants is 0.2 mol/L, what is the value of Kc?

Answer: Kc = 4.0

Question 1: Describe a simple experiment that demonstrates reversible reactions and explain the safety precautions involved.

Answer: One example is the reaction between iodine and starch, which is reversible under different temperature conditions. Safety precautions include handling chemicals with gloves and eye protection, and working in a well-ventilated area to avoid inhaling fumes.

Question 2: Identify three variables that can affect the position of equilibrium in a reversible reaction.

Answer: Temperature, concentration of reactants or products, and pressure (for gaseous reactions).

Question 1: In a reversible reaction, increasing the temperature shifts the equilibrium toward the reactants. Explain why this happens and give an example of such a reaction in industry.

Answer: This occurs because the reaction absorbs heat, favoring the endothermic direction. An example is the Haber process for ammonia synthesis, where temperature control influences yield.

Question 2: A reversible reaction reaches equilibrium with a concentration ratio of products to reactants as 3:1. If the concentration of reactants is increased, predict how the system will respond.

Answer: The reaction will shift toward producing more reactants to restore equilibrium, decreasing product concentration.