ABSTRACT
The kinetic theory of gases leads to a value for the number of collisions between two molecules, but the found value is, by far, too large when compared to the values of the rate constants k experimentally found. It has been reasonable to assume that the only reactive molecules are those possessing exceptional amounts of energy. When the rate constant of a reaction is determined at different temperatures, it is found that it increases with the temperature. From the quantitative standpoint, a straight line is obtained most often if the logarithm of the rate constant is plotted against the reciprocal of the absolute temperature T. This kind of diagram is named an Arrhenius’ plot. The enthalpy of activation is usually dominated by the breakage and the formation of bonds when the substrate is transformed into the product.
