Arrhenius doctrine's law, also known as the Arrhenius equation or Arrhenius rate equation, is a scientific principle that relates the rate of a chemical reaction to the temperature and activation energy of the reaction. This law was developed by Swedish chemist Svante Arrhenius in the late 19th century.
According to the Arrhenius doctrine, the rate of a chemical reaction increases exponentially with an increase in temperature. This means that as the temperature rises, the rate of the reaction also increases, and vice versa. The law provides a mathematical equation that expresses this relationship between temperature and reaction rate.
The Arrhenius equation is written as k = Ae^(-Ea/RT), where k represents the rate constant of the reaction, A is the pre-exponential factor or the frequency factor, Ea is the activation energy of the reaction, R is the ideal gas constant, and T is the absolute temperature in Kelvin.
The activation energy, Ea, determines the minimum amount of energy required for a chemical reaction to occur. It represents the energy barrier that reactant molecules must overcome in order to convert into products.
In summary, the Arrhenius doctrine's law describes the temperature dependency of chemical reaction rates, providing an equation that relates the rate constant, pre-exponential factor, activation energy, and temperature. This principle has significant applications in various scientific and industrial fields, including chemistry, biochemistry, and chemical engineering.
