Catalysis accelerates a chemical reaction by providing an alternative reaction mechanism with a more accessible barrier through its transition states. A catalyst participates in the route and is regenerated. At fixed temperature, catalysis changes how quickly chemical equilibrium is reached without changing the equilibrium constant; it does not make an unfavourable overall change in Gibbs free energy favourable. [ref]
Chemistry 2e by Paul Flowers and others. §12.7, opening definition and Figure 12.19: alternative mechanisms and regeneration
[ref]13.3 Shifting Equilibria: Le Châtelier’s Principle. §13.3, Effect of a Catalyst: equilibrium composition is unchanged
In his 1909 lecture, Wilhelm Ostwald recalled the introduction of the term catalysis by Jöns Jacob Berzelius and emphasized measurable acceleration rather than merely naming an unexplained force. He also discussed reaction intermediates and participation of the catalyst in the steps whose sum gives the net chemical reaction. This is a participant's retrospective account, not evidence that every catalytic reaction mechanism is the same.[ref]
On Catalysis. On Catalysis, lecture dated 12 December 1909; paragraphs beginning “The factor which Berzelius regarded” and “It is appropriate here”; editorial footnote says the lecture was reconstructed from notes
Articles by others on the same topic
Catalysis is a process that accelerates a chemical reaction by the presence of a substance called a catalyst. A catalyst is not consumed during the reaction and can be used repeatedly. It works by providing an alternative pathway for the reaction to proceed, usually with a lower activation energy compared to the non-catalyzed reaction.
