Thermodynamic versus kinetic reaction control

Thermodynamic reaction control or kinetic reaction control in a chemical reaction can decide the composition in a reaction product when competing reactions lead to different products under different reaction conditions. The distinction is relevant when product A forms faster (kinetics) than product B (The activation energy for A is lower than that of B) but B is a more stable (thermodynamics) product than A.

Reactions are considered to take place under thermodynamic reaction control when the reverse reaction is rapid and the Chemical equilibrium establishes itself quickly. In this way the thermodynamically more stable product is always favoured. Thermodynamic reaction control takes place with vigorous reaction conditions or when the reaction is allowed to continue over a long time to give a slow reaction time to reach equilibrium.

In kinetic reaction control, the forward reaction is much faster than the reverse reaction. As a result, the reaction favours the product with the lowest activation energy and goes forth regardless of relative product stabilities. Kinetic control is favoured with mild and low temperature conditions.

Examples

 * The Diels-Alder reaction of cyclopentadiene with furan serves as an example. At room temperature kinetic reaction control prevails and the less stable endo isomer 2 is the main reaction product. At 81°C and long reaction time the chemical equilibrium can assert itself and the thermodynamically stable exo isomer 1 is formed.


 * In the protonation of an enolate ion the kinetic product is the enol and the thermodynamic product is a ketone.
 * In carbohydrate acetalisation choice of acetone precursor determines reaction outcome.
 * The electrophilic addition reaction of hydrogen bromide to 1,3-butadiene at 60°C leads predominantly to the thermodynamically stable 1,4 adduct 3-bromo-1-butene but decreasing the reaction temperature to -60°C favours the kinetic 1,2 product 1-bromo-3-butene.