By Corrosion Science Doctor
The Arrhenius equation is an empirical relationship between the rate of a chemical reaction and the temperature at which it occurs. It states that the rate of a reaction is proportional to the exponential activation energy (Ea) divided by the absolute temperature (T). The equation is expressed as:
k = A e^(-Ea/RT)
Where Ea is the activation energy, A signifies the Arrhenius pre-exponential factor, h presents Plank's constant, N represents Avogadro's number, T (K) is the temperature effect and R is the universal gas constant.
The Arrhenius equation was first proposed by Swedish chemist Svante Arrhenius in 1889. He suggested that when a reaction occurs, molecules must overcome an energy barrier known as activation energy before they can react. This energy barrier can be thought of as a hill that must be climbed before a reaction can take place. The higher this barrier, the slower the reaction will be.
The Arrhenius equation allows us to calculate how much faster or slower a reaction will be at different temperatures. As temperature increases, so does the rate of reaction because more molecules have enough energy to overcome the activation energy barrier. This means that more molecules are able to react in a given amount of time, resulting in an increased rate of reaction.
The Arrhenius equation has been used extensively in chemistry and other fields to predict how different factors such as temperature and pressure affect chemical reactions. It has also been used to explain why some reactions occur faster at higher temperatures while others occur faster at lower temperatures.
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