Question

How is the rate constant of a reaction related to its activation energy? Name the equation which gives the relationship.

How is the activation energy of a reaction related to its rate constant?

Answer 1

The rate constant of a reaction is exponentially related to its activation energy through the Arrhenius equation.

\[\ce{k = Ae^{-E_a/RT}}\]

Where:

k = rate constant

A = frequency factor

E_a = activation energy

R = gas constant

T = absolute temperature (in Kelvin)

This equation shows that a reaction with a higher activation energy has a smaller rate constant, meaning it proceeds more slowly, while a lower activation energy leads to a higher rate constant, and the reaction proceeds faster.

The name of the equation is the Arrhenius equation.