Question

What‌ ‌Is‌ ‌Intermediate‌ ‌Complex‌ ‌Theory‌ ‌of‌ ‌Catalysis?‌

Answer 1

A catalyst is a material that may be added to a reaction to speed up the process without being absorbed by it. Catalysts usually work by lowering the activation energy or modifying the mechanism of a reaction.

Complete answer:
-Catalysis is the contribution of a catalyst to a chemical reaction to speed up the rate of the reaction. The compound is formed with less energy than what is actually needed for the reaction to take place. The catalyst is regenerated as the unstable intermediate compound reacts with other reactants to form the desired substance.
-There are two kinds of catalysts: homogeneous and heterogeneous. Homogeneous catalysts are those that are in the same phase as the reactants (gas or liquid), whereas heterogeneous catalysts are not in the same phase as the reactants (gas or liquid).
-Homogeneous catalysis is usually based on the intermediate compound forming principle of catalysis. The activation energy decreases, and the rate of reaction accelerates as a result of the forming of intermediate complexes.
-A reaction intermediate, also known as an intermediate, is a molecular element formed from reactants (or preceding intermediates) that reacts further to produce the immediately observable products of a chemical reaction. The majority of chemical reactions are stepwise, meaning they require more than one basic step to complete.

Note:
Catalysts shorten the time it takes for a chemical reaction to start by lowering the amount of energy required. Many manufacturing processes depend on chemical reactions to transform raw materials into functional products, and catalysis is at the heart of them. Catalysts are used to make plastics and a variety of other consumer goods.