Question

How does catalyst affect the activation energy of a chemical reaction?

Answer 1

A catalyst is a substance that diminishes the activation energy expected to begin a chemical response and therefore, additionally expands the pace of the chemical reaction. It is so more reactant atoms crash into enough energy to conquer the more modest energy barrier

Complete answer:
The activation energy of a chemical reaction is firmly identified with its rate. In particular, the higher the activation energy, the more slow the chemical reaction will be. This is on the grounds that particles can just finish the reaction whenever they have arrived at the highest point of the activation energy barrier.
Most substance responses that occur in cells resemble the hydrocarbon combustion model: the activation energy is excessively high for the responses to continue fundamentally at encompassing temperature. From the outset, this appears to be an issue; all things considered, you can't set off a flash within a cell without causing harm. Luckily, it's conceivable to bring down the activation energy of a reaction, and to accordingly expand response rate. The way toward accelerating a reaction by decreasing its activation energy is known as catalysis, and the factor that is added to bring down the activation energy is known as a catalyst.

Note: A catalyst builds reaction rates in a somewhat extraordinary manner from different techniques for expanding reaction rate. The capacity of a catalyst is to bring down the activation energy with the goal that a more prominent extent of the particles have enough energy to respond. A catalyst can bring down the activation energy for a reaction by situating the reacting particles so that effective collisions are almost certain and responding with the reactants to frame a halfway that requires lower energy to shape the product