# Interpretation of Arrhenius Equation

Arrhenius equation represents the dependence of the rate constant

*k*of a reaction on the absolute temperature*T*:where the factor refers to the fraction of collisions (also effective collisions) that have the sufficient activation energy to collide and form products and

*A*is the number of effective collision per unit time. Therefore, the product of*A*and is the number of collisions that actually lead to the formation of products.# Determination of activation energy

where

*k*_{1}and*k*_{2}are rate constants at temperatures*T*_{1}and*T*_{2}kelvin, respectively. Knowing these values,*E*can be calculated. Care must be taken to insert the value of_{a}*R*in a unit in which*E*is desired._{a}# Main characteristics of arrhenius equation

- The larger the activation energy of a reaction, the smaller is the value of rate constant.
- The larger the activation energy of a reaction, the greater is the influence of change in temperature on rate constant.
- For lower temperature range, increase in temperature causes more change in the value of
*k*than the same increase in temperature of high temperature range.