# How does the activation energy affect reaction rate?

Jun 30, 2018

see below

#### Explanation:

the rate of a chemical reaction ( A+B= C+D) is given in first approximation by
$V = {K}_{v} \times \left[A\right] \times \left[B\right]$
where
K_v= K° xx e^(-E_a/(RT))
where K° depends by many factors as solvent, geiometry, type of reaction
Ea is the activation energy
R is the universal costant of gases
T is the absolute temperature
Hence highter is the activation energy, lower is the rate of the reaction
Normally if the activation energy is more than about 10Kcal/mol the reaction cannot occurr if you don't use a catalyst