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 works by providing an alternative pathway with a lower activation energy.

Question 1: Describe how transition metals act as catalysts in reactions such as the Haber process.

Answer: Transition metals act as catalysts by providing a surface for reactant molecules to adsorb onto. This facilitates the breaking and forming of bonds, lowering the activation energy and increasing reaction rate.

Question 1: Identify the variables you would control and measure in this experiment.

Answer: Control variables include concentration of hydrogen peroxide, temperature, and amount of catalyst. The measured variable is the rate of oxygen gas production.

Question 2: List two safety precautions to consider when handling hydrogen peroxide and transition metal catalysts.

Answer: Wear safety goggles and gloves; handle hydrogen peroxide carefully to avoid spills and skin contact.

Question 1: If 0.5 mol of hydrogen peroxide decomposes in 10 seconds in the presence of a catalyst, what is the reaction rate per second?

Answer: Reaction rate = 0.5 mol / 10 s = 0.05 mol/s

Question 1: A reaction using platinum as a catalyst reaches 80% completion in 5 minutes, whereas the same reaction without a catalyst takes 20 minutes. Explain the role of platinum in this reaction.

Answer: Platinum acts as a catalyst by providing an alternative pathway with a lower activation energy, significantly increasing the reaction rate and reducing the time to completion.

Question 1: Explain how transition metal catalysts are used in the contact process for producing sulphuric acid. Include the role of the catalyst, advantages, and any safety considerations.

Answer: In the contact process, vanadium pentoxide (V2O5), a transition metal compound, acts as a catalyst to convert SO2 to SO3. The catalyst provides an alternative pathway with lower activation energy, increasing the rate of the reaction at industrial scale. Advantages include higher efficiency and faster production rates. Safety considerations involve handling the catalyst and gases safely to prevent leaks, and ensuring proper ventilation due to the toxic gases involved.

Question 1: Describe two ways in which catalysts improve environmental sustainability in industry or daily life.

Answer: Catalysts reduce energy consumption by speeding up reactions, thus lowering fuel use. They also enable cleaner production processes with fewer harmful emissions.