How does a catalyst increase the rate of a reaction? Group of answer choices it allows reacting molecules to more easily form the transition state it causes a localized increase in the concentration of reactants it increases the temperature of the reaction none of the above it makes the reaction more exergonic

It allows reacting molecules to more easily form the transition state

Explanation:

Catalysts are substances that modify the rate of a chemical reaction without changing the final product of it. Sometimes light or an external electric field also performs a catalytic task.

Catalysts are usually collected at the end of the reaction without having changed, so very small amounts are needed, but over time they undergo a process of wear or even "poisoning" that makes them unusable, especially when they work at high temperature, since they volatilize slowly.

A catalyst cannot cause a reaction that cannot be carried out by itself. There is practically a catalyst for each reaction: they are specific to each one, making the activation energy less.

The way to act catalysts is to change the mechanism of the reaction, providing a simpler path, so the reaction time is shorter. They take an active part in the reaction, forming intermediate compounds that decompose rapidly regenerating the catalyst, so it is not consumed. In this way, the catalyst changes the mechanism of the reaction and causes it to pass through a different path of lower activation energy.