How do catalysts increase reaction rates without being consumed?

Catalysts increase reaction rates by lowering the activation energy needed for the reaction, without being consumed in the process.

Catalysts are substances that can speed up a chemical reaction without being used up or changed themselves. They do this by providing an alternative reaction pathway with a lower activation energy. Activation energy is the minimum amount of energy required for a reaction to occur. By lowering this threshold, more reactant particles have enough energy to react, leading to an increase in the rate of reaction.

The catalyst achieves this by forming temporary bonds with the reactant molecules, creating a new, temporary substance known as an 'intermediate'. This intermediate has a lower activation energy than the original reactants, allowing the reaction to proceed more quickly. Once the reaction is complete, the catalyst breaks away from the intermediate and is free to catalyse another reaction. This is why catalysts are not consumed in the reaction.

It's important to note that while catalysts speed up reactions, they do not change the products of the reaction or the overall energy change of the reaction. They simply make the reaction happen faster. This is why catalysts are incredibly useful in many industrial processes, as they can significantly increase production rates without altering the end product.

In summary, catalysts increase the rate of chemical reactions by providing an alternative reaction pathway with a lower activation energy, allowing more reactant particles to react. They are not consumed in the process as they form temporary bonds with the reactants, which break once the reaction is complete.