What is Catalyst? Definition, Meaning & Example
A substance that increases the rate of a chemical reaction without being consumed in the reaction.
TL;DR: A substance that increases the rate of a chemical reaction without being consumed in the reaction.
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Catalyst: A substance that increases the rate of a chemical reaction without being consumed in the reaction.
Explanation
Catalysts work by lowering the activation energy needed for a reaction to occur, allowing more molecules to react at a given temperature. They are not changed by the reaction, so the same catalyst can be used repeatedly. Enzymes are biological catalysts that speed up reactions in living organisms. Industrial processes use catalysts to increase production efficiency; for example, ammonia production uses iron as a catalyst. Understanding catalysts is crucial for chemistry, biology, and industrial applications. Different catalysts are required for different reactions, and some catalysts are specific to particular reactions.
Example
Manganese dioxide catalyzes the decomposition of hydrogen peroxide. Adding manganese dioxide speeds up the reaction dramatically, but the manganese dioxide remains unchanged and can be used again.
Frequently Asked Questions
How does a catalyst speed up a reaction?
A catalyst lowers the activation energy by providing an alternative reaction pathway, allowing more molecules to have enough energy to react.
Are catalysts consumed in chemical reactions?
No, catalysts are not consumed; they emerge unchanged from the reaction and can catalyze the reaction repeatedly.
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