There are many factors that influence the products of chemical reactions. All reactions are affected differently when exposed to these agents. Temperature is just one of many factors that can change things about reactions. When exposed to temperature change, the activation energy of a reaction can be reached much more quickly (or slowly) than it would have been. As the temperature increases, the rate of the reaction increases. Temperature contributes very flexibly to the speed of reactions and chemical reactions in general. Temperature changes can affect almost all parts of a reaction, such as the kinetic energy of molecules, the speed of enzymes, and how quickly activation energy is reached. While temperature changes many things in reactions, some factors in reactions can change the temperature. Kinetic energy is a measure of how fast molecules are moving at a given time. Kinetic energy can be affected by temperature change, as are many other parts of a reaction. The higher the temperature, the greater the kinetic energy becomes. An increase in kinetic energy can influence the speed of a reaction which occurs by increasing the speed of movement of the molecules. Kinetic energy is also modified by air pressure, which can also be influenced by temperature; the higher the pressure and temperature, the greater the kinetic energy and therefore the faster the reaction occurs. Kinetic energy can also influence temperature; when the kinetic energy increases, the temperature also increases. This happens because chemical reactions can be endothermic or exothermic. When a reaction is endothermic, kinetic energy becomes potential energy, meaning that heat is absorbed and temperature has an effect on kinetic energy. On the other hand, when a reaction... middle of paper ......that has a very low activation energy, it means that it happens very quickly or almost instantaneously. On the other hand, there are very many reactions that have exceptionally high activation temperatures, and these reactions take much longer to occur. With this in mind, it's important to remember that not all collisions create a reaction. Millions of molecules collide with each other every second, but not all of them react. The molecules must have reached adequate kinetic energy to break the bonds of the reactants and create products. “When two billiard balls collide, they simply bounce off each other… To… start a reaction, the collisions must be sufficiently energetic (kinetic energy) to cause this bond breaking.” (boundless.com). The bonds of reactions can only be broken when molecules of certain kinetic energies collide.