Rate constant (collisions in chemical reactions)


Collision theory qualitatively explains how chemical reactions occur and why reaction rates differ for different reactions. The collision theory states that when suitable particles of the reactant hit each other, only a certain percentage of the collisions cause any noticeable or significant chemical change; these successful changes are called successful collisions. The rate constant for a bimolecular gas phase chemical reaction quantifies the rate of the reaction.

Related formulas


kTRate constant (mol/L*sec)
ZCollision frequency (1/sec)
ρSteric factor (mol/L)
EaActivation energy (J/mol)
Rmolar gas constant
TTemperature (K)