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Collision Theory Science Simply Explained

Collision Theory Science Simply Explained

May 8, 2009

Collision theory science is a hypothesis, suggested by Max Trautz and William Lewis in 1916 that clearly illustrates how chemical responses take place and why reaction rates vary for various reactions. The collision theory is founded on the presumption that for a reaction to happen it is required for the reacting type (molecules or atoms) to draw near or to collide with each other. It is in essence a set of doctrines which describe the effects of various influences on the speed of a reaction. It is primarily used to illustrate why varying the particle measurement, temperature or denseness of reactants will change the reaction rate.

A primary comprehension of collision theory science allows us to foresee the types of experiments we may be able to conduct which will alter the rate of a chemical reaction. A pre defined quantity of energy is required to manufacture a chemical modification so the reaction must be oriented by a means favourable to the required rearrangement of molecules and electrons.

There are a variety of methods in which you can stimulate the reaction to occur for example, warming it up, varying the surface area, altering the pressure, concentration or by introducing some form of accelerator. Furthermore, the theory presumes that the greater part of collisions do not initiate a reaction, other than those in which the colliding mediums have a kinetic energy larger than a specific minimum, named ‘activation energy’.

Collision Theory Science

Collision Theory Science

Expanding the temperature range of a reaction boosts the kinetic energy of the particles which in turn increases the quantity of collisions meaning the reaction rate also rises. However, as the temperature surges, not simply does the amount of collisions per second rise but in addition the ratio of collisions which have a kinetic energy the same or larger than Ea, the activation energy, increases. This upsurge in possible energy is directly aligned to an energy limit over which the reactant atoms must cross if the reaction is to go ahead.

Considering that atomic or molecular frequencies of collisions can be considered with some level of exactness exclusively for gases (through implementation of the kinetic assumption), the application of the collision theory is ordinarily restrcited to gas phase reactions.

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