Arrhenius Equation

     

Arrhenius Equation
\( k = A \; e \; ( -E_a \;/\; R\;T_a )\)
Symbol	English	Metric
\( k \) = rate constant	-	\(mol \;/\; L-s\)
\( A \) = frequency factor (different for every reaction)	\(dimensionless\)	\(dimensionless\)
\( e \) = natural log base	\(dimensionless\)	\(dimensionless\)
\( E_a \) = activation energy	\(lbf-ft\)	\(J\)
\( R \) = universal gas constant	\(lbf-ft \;/\; lbmol-R\)	\(J \;/\; kmol-K\)
\( T_a \) = absolute temperature	\(R\)	\(K\)

Arrhenius equation is the temperature dependance of the reaction rate constant which is the rate of chemical reaction.  Chemical reactions are typically expected to preceed faster at higher temeratures and slower at lower temperatures.  As the temperature rises, molecules move faster and collide, greatly increasing their likelyhood to bond.  This results in a higher kinetic energy, which has an affect on the activation energy of the reaction.  Conversely, at lower temperatures, the rate of reaction decreases.