The use of a catalyst Nature of The Reactants Reactions produce products by having the reacting molecules come into contact with one another. The more often they collide, the more likely the chance that product will form. If the reacting molecules moving more rapidly and in the gaseous state then product will have a more likely chance to form. This is part of an over riding Theory that forms the foundation of all kinetics work. This theory is called the Collisional Theory of Reaction Rates .
Reactions usually occur more rapidly when the reactants are in the gaseous state.
The reacting molecules dispersed in a solution is the next most favorable way for product to form at a reasonable speed. Reactions do occur in pure liquids or in solid form but the rates tend to be rather slow because the reacting molecules are very restricted in their movement among one another, and therefore, do not come into contact as often. We will be studying how concentration fills a role in affecting the Reaction Rate of a process in another section. Temerature effects will be discussed in a future section as will the effect on the rate that catalysts have. R. H. Logan, Instructor of Chemistry, Dallas County Community College District, North Lake College.