Question 1: Define a catalyst and explain how it affects the rate of a chemical reaction.

Answer: A catalyst is a substance that increases the rate of a chemical reaction without being consumed in the process. It provides an alternative reaction pathway with lower activation energy.

Question 2: List three transition metals commonly used as catalysts in industry.

Answer: Iron, platinum, nickel.

Question 3: Describe the role of transition metals as catalysts in the Haber process for synthesizing ammonia.

Answer: Transition metals like iron act as catalysts by providing a surface for nitrogen and hydrogen molecules to adsorb, react, and then desorb as ammonia. This lowers the energy barrier and speeds up the reaction without being consumed.

Question 4: Which of the following statements is true about catalysts? A) They are consumed during the reaction. B) They lower the activation energy. C) They are only used in biological systems. D) They increase the energy of the products.

Answer: B) They lower the activation energy.

Question 5: Fill in the blank: Catalysts work by providing an __________ pathway for the reaction, which requires less energy to proceed.

Answer: alternative

Question 6: Explain why transition metals are effective catalysts in redox reactions.

Answer: Transition metals have variable oxidation states, allowing them to easily gain and lose electrons, which facilitates redox reactions by providing a surface for electron transfer.

Question 7: Describe an experiment to test the effect of surface area of a transition metal catalyst on reaction rate (theory only).

Answer: One could compare the rate of a catalytic reaction using different forms of the metal catalyst, such as powdered versus solid blocks, keeping all other variables constant. The increased surface area of powdered metal is expected to increase the reaction rate due to more active sites.

Question 8: What safety precautions should be considered when working with transition metal catalysts in a laboratory setting?

Answer: Wear protective gloves and goggles, work in a well-ventilated area or fume hood, and handle chemicals carefully to avoid inhalation or skin contact, as some catalysts or their compounds may be toxic or corrosive.

Question 9: Data Scenario: In an experiment, increasing the surface area of a platinum catalyst from a small pellet to a fine powder resulted in the reaction rate doubling. Explain why this occurs.

Answer: The larger surface area provides more active sites for the reaction to occur, increasing the number of collisions and thus doubling the reaction rate.

Question 10: Identify a real-world application where transition metal catalysts are used to improve efficiency or sustainability.

Answer: Catalytic converters in cars use platinum and palladium to convert harmful gases into less toxic emissions, improving environmental sustainability.