Question 1: Define activation energy in your own words.

Answer: Activation energy is the minimum amount of energy that particles must have to collide successfully and react.

Question 2: Explain why a reaction with a higher activation energy generally occurs more slowly than one with a lower activation energy.

Answer: Because fewer particles have enough energy to overcome the higher energy barrier, resulting in fewer successful collisions.

Question 3: What is the role of a catalyst in relation to activation energy?

Answer: A catalyst lowers the activation energy needed for a reaction, making it happen faster without being consumed.

Question 1: A reaction has an activation energy of 80 kJ/mol. If the temperature is increased, how does this affect the reaction rate? Explain your answer using scientific reasoning.

Answer: Increasing temperature provides more energy to particles, making it easier for them to overcome the activation energy barrier, thus increasing the reaction rate.

Question 2: Calculate the minimum energy (in kJ) required for 2 moles of particles to react if the activation energy is 75 kJ/mol.

Answer: 150 kJ

Question 1: Describe a simple experiment that could be used to measure the effect of temperature on activation energy in a chemical reaction. Include safety precautions.

Answer: Students could heat reactants at different temperatures and measure the reaction rate by observing product formation or gas evolution. Safety precautions include wearing goggles, gloves, and working in a well-ventilated area to handle heat and chemicals safely.

Question 2: Identify two factors, other than temperature, that can influence the activation energy of a reaction.

Answer: Presence of a catalyst and the nature of the reactants (such as their physical state or surface area).

Question 1: A factory uses a catalytic converter to reduce emissions from car exhaust. Explain how the catalyst affects the activation energy of the reactions involved.

Answer: The catalyst lowers the activation energy of the reactions, allowing harmful gases to convert into less harmful substances more quickly, thus reducing emissions.

Question 2: In everyday life, why is it easier to ignite a paper fire at higher temperatures compared to room temperature?

Answer: Higher temperatures provide particles with more energy, increasing the likelihood they can overcome the activation energy barrier and start combustion more easily.