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

Answer: Collision Theory states that chemical reactions occur when reactant particles collide with sufficient energy and proper orientation to break and form bonds.

Question 2: What two main conditions must be met for a successful particle collision to lead to a reaction?

Answer: The particles must collide with enough energy (activation energy) and with the correct orientation.

Question 3: Explain how temperature influences the rate of reaction according to Collision Theory.

Answer: Higher temperature increases the energy of particles, leading to more collisions with sufficient energy, thus increasing the reaction rate.

Question 1: Given a gas sample with a particle concentration of 2 x 10^25 particles per cubic meter, and a particle speed of 500 meters per second, calculate the collision frequency per second in a 1 cubic meter space. Use the formula: Collision frequency = 0.5 x concentration x particle speed x surface area per particle. Assume each particle has a surface area of 1 x 10^-19 m^2.

Answer: Collision frequency = 0.5 x 2 x 10^25 x 500 x 1 x 10^-19 = 5 x 10^8 collisions per second.

Question 2: If increasing the temperature from 25°C to 35°C doubles the average particle energy, by what factor does the collision energy increase? Assume energy is proportional to temperature.

Answer: The collision energy increases by a factor of 2.

Question 1: Describe a simple experiment to demonstrate how increasing reactant concentration affects the rate of reaction. Include the main variable you would change and the safety precautions you should take.

Answer: You could set up two reactions with different concentrations of reactant, such as reacting magnesium with hydrochloric acid, and measure the time taken for a set amount of gas to be produced. The main variable is the reactant concentration. Safety precautions include wearing goggles, gloves, and working in a well-ventilated area to handle acids safely.

Question 1: In an experiment, the reaction rate increased when the pressure of a gas was increased from 1 atm to 2 atm. Explain using Collision Theory why this happens.

Answer: Increasing pressure increases particle concentration, leading to more frequent collisions, which raises the reaction rate according to Collision Theory.

Question 1: Explain how Collision Theory is applied in the industrial production of sulfuric acid.

Answer: In industrial sulfuric acid production, reactions are optimized by increasing temperature and reactant concentration to increase collision frequency and energy, thus speeding up the reaction process.

Question 2: Identify one safety consideration when working with gases at high pressure to ensure collision theory experiments are conducted safely.

Answer: Ensure proper ventilation and use pressure relief devices to prevent accidents from high-pressure gases.