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Catalyst on Chemical Equilibrium

1850
Chemist conducting experiments with catalysts in a vintage laboratory setting, 1850.

A catalyst increases the rate of both the forward and reverse reactions equally by providing an alternative reaction pathway with a lower activation energy. While a catalyst allows a system to reach equilibrium much faster, it does not change the position of the equilibrium itself. The equilibrium concentrations of reactants and products, and the value of the equilibrium constant K, remain unchanged.

The function of a catalyst can be visualized using a reaction energy profile diagram. The catalyst lowers the energy of the transition state, which is the peak of the energy barrier between reactants and products. Crucially, it lowers this barrier by the same amount for both the forward and reverse reactions. This means the activation energy for the forward reaction ([latex]E_{a,fwd}[/latex]) and the activation energy for the reverse reaction (\(E_{a,rev}\)) are both reduced, but the difference between them, which corresponds to the overall enthalpy change of the reaction (\(\Delta H = E_{a,fwd} – E_{a,rev}\)), is not affected.

Since the equilibrium constant K is related to the standard Gibbs free energy change (\(\Delta G^{circ} = -RT \ln K\)), and catalysts do not alter the thermodynamics (\(\Delta G^{circ}\), \(\Delta H^{circ}\)) of the overall reaction, they cannot change the value of K. Their role is purely kinetic, enabling the system to achieve the thermodynamically favorable equilibrium state in a shorter amount of time. This is vital in industrial processes where reaching equilibrium quickly is economically necessary, as many thermodynamically favorable reactions are too slow to be practical without catalysis.

UNESCO Nomenclature: 2209
– Physical chemistry

Type

Abstract System

Disruption

Foundational

Usage

Widespread Use

Precursors

  • Arrhenius equation relating reaction rate to activation energy
  • concept of activation energy
  • early observations of substances speeding up reactions without being consumed (e.g., by kirchhoff, davy)

Applications

  • catalytic converters in automobiles to reduce harmful emissions
  • enzymes in biological systems acting as biocatalysts
  • Haber-Bosch process using an iron catalyst
  • contact process using a vanadium(v) oxide catalyst
  • petroleum refining and cracking

Patents:

NA

Potential Innovations Ideas

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Related to: catalyst, equilibrium, activation energy, reaction rate, kinetics, thermodynamics, equilibrium constant, forward reaction, reverse reaction, enzyme.

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Historical Context

(if date is unknown or not relevant, e.g. "fluid mechanics", a rounded estimation of its notable emergence is provided)

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