Discuss how catalysts can make processes more energy efficient.

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1. Step 1: Define what a catalyst is in the context of chemistry. 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 a lower activation energy.
2. Step 2: Explain the concept of activation energy. Activation energy is the minimum energy required for a chemical reaction to occur. Catalysts lower this energy barrier, allowing more reactant molecules to have enough energy to react at a given temperature.
3. Step 3: Describe how lowering the activation energy affects reaction rates. By reducing the activation energy, catalysts increase the number of successful collisions between reactant molecules, thereby increasing the reaction rate.
4. Step 4: Discuss the impact of increased reaction rates on energy efficiency. Faster reactions mean that processes can be completed in less time and often at lower temperatures, reducing the energy required to maintain reaction conditions.
5. Step 5: Provide examples of industrial processes where catalysts improve energy efficiency. For instance, in the Haber process for ammonia synthesis, iron catalysts allow the reaction to occur at lower temperatures and pressures, saving energy and costs.