Question 1: Define Collision Theory in the context of chemical reactions.

Answer: Collision Theory states that chemical reactions occur when reacting particles collide with sufficient energy and proper orientation.

Question 2: Explain why increasing the temperature generally increases the rate of reaction.

Answer: Increasing temperature increases particle kinetic energy, leading to more frequent and energetic collisions that surpass the activation energy.

Question 3: Describe the two main factors that determine whether a collision results in a reaction.

Answer: The collision must have sufficient energy (exceeding the activation energy) and proper orientation of the particles.

Question 1: Calculate the minimum kinetic energy (in kJ/mol) required for particles to react if the activation energy is 50 kJ/mol.

Answer: 50 kJ/mol

Question 2: If the collision frequency in a reaction mixture is 2 x 10^9 collisions per second, estimate how many collisions occur in 1 minute.

Answer: 1.2 x 10^11 collisions

Question 1: Describe an experiment to investigate how temperature affects the rate of a reaction involving sodium thiosulphate and hydrochloric acid.

Answer: Students can measure the time taken for a precipitate to form at different temperatures, keeping concentration and volume constant. The reaction rate increases with temperature due to more particles having sufficient energy to overcome the activation barrier.

Question 2: Identify two variables that should be kept constant in this experiment and explain why.

Answer: Concentration and surface area should be kept constant to ensure that temperature is the only factor affecting the reaction rate.

Question 3: List two safety precautions that should be observed when handling hydrochloric acid in experiments.

Answer: Wear safety goggles and gloves to protect against corrosive effects.

Question 1: In an experiment, increasing the concentration of reactant A from 0.1 mol/dm^3 to 0.2 mol/dm^3 doubled the reaction rate. Explain this observation in terms of Collision Theory.

Answer: Increasing concentration raises the number of particles per unit volume, leading to more frequent collisions, which increases the reaction rate.

Question 1: Explain how catalysts work in terms of Collision Theory to increase reaction rates.

Answer: Catalysts provide an alternative reaction pathway with a lower activation energy, increasing the number of particles that have sufficient energy to react upon collision.

Question 2: Describe a practical example where Collision Theory is used to improve industrial processes.

Answer: In the Haber process for ammonia synthesis, iron catalysts increase reaction rate by facilitating more effective collisions, making the process more efficient and economical.