Catalysis and reaction rates are fundamental concepts in AP Chemistry. Catalysts speed up reactions by lowering the activation energy, without being consumed in the process. Reaction rates describe how quickly reactants are converted into products, influenced by factors like temperature, concentration, and the presence of catalysts. Understanding these principles is crucial for predicting and controlling chemical reactions. Let's dive in!
Match the terms with their definitions:
| Term | Definition |
|---|---|
| 1. Catalyst | A. The minimum energy required for a reaction to occur. |
| 2. Activation Energy | B. A substance that speeds up a reaction without being consumed. |
| 3. Reaction Rate | C. A series of steps that make up the overall reaction. |
| 4. Reaction Mechanism | D. A temporary species formed during a reaction mechanism. |
| 5. Intermediate | E. The speed at which reactants are converted to products. |
(Answers: 1-B, 2-A, 3-E, 4-C, 5-D)
Complete the following paragraph using the words: rate-determining, catalyst, activation energy, reaction rate, intermediates.
A __________ increases the __________ of a chemical reaction by lowering the __________. The slowest step in a reaction mechanism is called the __________ step. Species that are produced and consumed during the reaction are called __________.
(Answers: catalyst, reaction rate, activation energy, rate-determining, intermediates)
Explain how a heterogeneous catalyst works and provide a real-world example of its use.
Please log in to post your answer.
Log InEarn 2 Points for answering. If your answer is selected as the best, you'll get +20 Points! 🚀