Question 1: Explain in your own words how increasing the temperature affects the rate of a chemical reaction.

Answer: Increasing temperature increases the reaction rate because particles move faster, leading to more frequent and energetic collisions that can overcome the activation energy barrier.

Question 2: Define the term 'activation energy'.

Answer: Activation energy is the minimum energy needed for particles to collide successfully and form products in a reaction.

Question 1: Describe how the Maxwell-Boltzmann distribution curve shifts as temperature increases.

Answer: As temperature increases, the Maxwell-Boltzmann distribution curve shifts to the right and flattens, indicating more particles have higher energy, and there are more particles with energy exceeding activation energy.

Question 2: What is collision theory and how does temperature impact it?

Answer: Collision theory states that particles must collide with sufficient energy and proper orientation for a reaction to occur. Increasing temperature increases the number of particles with enough energy to react upon collision.

Question 1: The rate constant (k) for a reaction at 300°C is 0.02 s⁻¹. When the temperature is increased to 350°C, the rate constant becomes 0.08 s⁻¹. Calculate the activation energy (Ea) using the Arrhenius equation. (R = 8.31 J mol⁻¹ K⁻¹)

Answer: Ea = 76,250 J mol⁻¹

Question 1: Describe a safe method to heat a reaction mixture to increase its temperature for rate experiments.

Answer: Use a controlled water bath or heating mantle with temperature control to safely and evenly heat the reaction mixture, while wearing safety goggles and gloves.

Question 2: Identify two variables that should be kept constant in a temperature-rate experiment.

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

Question 1: A reaction was studied at three different temperatures: 20°C, 40°C, and 60°C. The measured rates were 0.5, 2.0, and 8.0 mol/L·s, respectively. Explain how the change in temperature affects the rate and why.

Answer: As temperature increases from 20°C to 60°C, the rate increases significantly. This is because higher temperatures increase particle energy, leading to more successful collisions and a faster reaction rate, consistent with collision theory.

Question 1: Explain how increasing the temperature can improve the efficiency of a chemical manufacturing process, and mention one potential drawback.

Answer: Increasing temperature can speed up reaction rates, reducing production time and increasing efficiency. However, it can also lead to increased energy costs and may cause unwanted side reactions or degradation of products.