Why does platinum metal make a good catalytic surface for reactant molecules?

• A. Platinum acts as an oxidizing agent, directly participating in chemical reactions by being consumed.
• B. Platinum has a high surface area and can adsorb reactant molecules, lowering the activation energy of reactions.
• C. Platinum is highly reactive and forms permanent bonds with reactant molecules, preventing their release.
• D. Platinum dissolves easily in most solvents, allowing reactants to interact freely in solution.

Answer: (B)

Verified step by step guidance

1. Understand that a catalyst provides a surface where reactant molecules can come together more easily, facilitating the reaction without being consumed.
2. Recognize that platinum metal has a high surface area and the ability to adsorb reactant molecules onto its surface, which means reactants are held close together in an optimal orientation.
3. Know that adsorption onto the platinum surface weakens bonds in the reactant molecules, effectively lowering the activation energy required for the reaction to proceed.
4. Realize that platinum does not get consumed or permanently altered during the reaction, so it can continue to catalyze multiple reaction cycles.
5. Conclude that these properties make platinum an excellent catalytic surface because it enhances reaction rates by providing a favorable environment for reactants without undergoing permanent chemical change.