Arrhenius equation describes the effect of temperature on the rate constant of a chemical reaction. It is given by:

k = Ae^(-Ea/RT)

where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant, and T is the temperature in Kelvin.

Explanation:

Temperature is a measure of the average kinetic energy of the molecules in a substance. When the temperature is increased, the molecules move faster and collide more frequently. This increases the chance of successful collisions between reactant molecules, leading to an increase in the reaction rate.

Arrhenius equation explains this relationship between temperature and reaction rate by stating that the rate constant (k) of a reaction increases exponentially with increasing temperature. The activation energy (Ea) is the minimum energy required for a reaction to occur, and it determines the rate at which the reaction proceeds.

The pre-exponential factor (A) takes into account the frequency of collisions between reactant molecules. It is a constant that depends on the nature of the reaction and the reactants involved.

The Arrhenius equation is widely used to describe the temperature dependence of chemical reactions in various fields, including chemistry, biology, and materials science.

Conclusion:

In summary, the Arrhenius equation is used to describe the effect of temperature on the rate constant of a chemical reaction. It explains that the rate constant increases exponentially with increasing temperature, due to an increase in the frequency and energy of collisions between reactant molecules.