How is a catalyst is used in a reaction?

In order to increase the frequency of successful collisions and, consequently, the rate of reaction, a catalyst offers an alternative reaction pathway with a lower activation energy, so that a higher proportion of reactant particles have energy greater than or equal to the new activation energy.

By offering an alternative pathway with a lower activation energy required for the reaction to occur, a catalyst is used to accelerate the rate of a reaction.

Adsorption is the transient attraction of a molecule to a solid surface, and it occurs first at the active sites of the catalyst where the reactants are first adsorbed.

Subsequently, the bonds within the reactant molecules weaken when they are adsorbed onto the metal because some of their electrons are being utilized to form bonds with the catalyst.

Because there is less energy required to break bonds, the reaction can occur more quickly as a result.

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This raises the number of favorable collisions and, consequently, the rate of the reaction by keeping the reactant adsorbed onto the metal in the proper orientation for the reaction to take place.

Following their separation from the metal surface, the product molecules make the active sites available to other molecules.

There is a general drop in activation energy.

A catalyst is used in a reaction to increase the rate of the reaction by lowering the activation energy required for the reaction to occur. This allows the reaction to proceed more quickly and efficiently without being consumed in the reaction itself. Catalysts provide an alternative reaction pathway with a lower activation energy, facilitating the conversion of reactants into products. After the reaction is complete, the catalyst remains unchanged and can be reused in subsequent reactions.