Collision Theory and Its Role in Controlling the Rate of Chemical Reactions

Collision Theory and its Role in Controlling Rates of Chemical Reactions

A well-established theory, collision theory, is used to explain chemical reactions. It also explains the influences that affect their speed. This theory states that two molecules need to collide in order for the reaction to occur. There are many factors that affect whether successful collisions can be achieved. These include temperature, surface area, nature, addition of catalysts and concentration. The probability of successful collisions increases when the temperature increases (Lloyd 2020). The chances of collisions are also increased by increasing the area of reactants, as more molecules exist in the same space. Rate of reaction also depends on their nature. Reactants with weaker bonds are more likely to disintegrate and react when they come into contact. A catalyst is a great way to speed up a reaction. The addition of a catalyst can increase the rate of a reaction by providing an alternative pathway that has a lower activation energies, allowing molecules react faster. The probability of collisions increases when the solution is concentrated. Collision theory is a good way to understand how different factors influence the rate of chemical reactions. The rate of reaction can be affected by temperature, surface area, nature, additions of catalysts and concentration. This will increase the likelihood of collisions. These factors are able to influence the rate of chemical reactions.