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 temperature generally increases the rate of a reaction according to Collision Theory.

Answer: Increasing temperature increases the energy of particles, leading to more frequent and more energetic collisions that can overcome the activation energy barrier.

Question 1: What two conditions must be met for a successful collision to result in a chemical reaction?

Answer: Particles must collide with sufficient energy (greater than or equal to the activation energy) and in the correct orientation.

Question 2: Describe how the frequency of successful collisions changes when the concentration of reactants increases.

Answer: Higher concentration increases the number of particles per unit volume, leading to more frequent collisions and thus a higher rate of reaction.

Question 1: Calculate the average energy of particles at a temperature of 300 K. (Use the formula: E = (3/2)kT, where k = 1.38 x 10^-23 J/K).

Answer: E = (3/2) × 1.38 × 10^-23 J/K × 300 K = 6.21 × 10^-21 Joules

Question 2: If the frequency factor (A) for a reaction is 1 x 10^12 s^-1 and the activation energy (Ea) is 50 kJ/mol, calculate the rate constant (k) at 298 K using the Arrhenius equation: k = A e^(-Ea/RT). (R = 8.314 J/mol·K).

Answer: k = 1 × 10^12 × e^(-50000 / (8.314 × 298)) ≈ 2.4 × 10^4 s^-1

Question 1: Describe a simple experiment to demonstrate how increasing temperature affects the rate of a reaction between vinegar and baking soda.

Answer: Mix equal amounts of vinegar and baking soda at different temperatures (e.g., cold, room temperature, hot) and measure the time taken for the reaction to complete or the amount of gas produced. The experiment shows that higher temperatures increase reaction rate due to more frequent and energetic collisions.

Question 2: Identify two safety precautions to consider when increasing the temperature of a reaction in a laboratory setting.

Answer: Use heat-resistant gloves and eye protection; ensure proper ventilation and avoid overheating to prevent accidents.

Question 1: A reaction speeds up when the pressure of a gas reactant is increased. Explain this observation using Collision Theory.

Answer: Increasing pressure reduces the volume, increasing the concentration of gas particles, which leads to more frequent collisions and a higher reaction rate.

Question 2: Explain how catalysts influence reaction rates according to Collision Theory.

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

Question 1: Explain how collision energy and particle orientation affect the rate of a chemical reaction. Include in your answer how temperature and catalysts modify these factors.

Answer: Reaction rate depends on particles colliding with sufficient energy (above the activation energy) and proper orientation. Increasing temperature raises the average energy of particles, leading to more collisions with enough energy. Catalysts lower the activation energy, allowing more collisions to result in successful reactions without changing the temperature.