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The Effect of a Catalyst

Reversible chemical reactions will eventually achieve equilibrium. At equilibrium, the rate of the formation of products is equal to the rate of the formation of reactants. Reaction progress towards this equilibrium state can be accelerated through the addition of catalysts or heat to the system.Catalysts are compounds that can accelerate the progress of a reaction without being consumed. Common examples of catalysts include acid catalysts and enzymes. A schematic depiction of the effect of a catalyst on a reaction coordinate can be seen in the figure below. Catalysts allow reactions to proceed by a different reaction pathway involving a lower-energy transition state. By lowering the energy of the rate-limiting step (the transition state), catalysts reduce the required energy of activation and allow a reaction to proceed and, in the case of a reversible reaction, reach equilibrium more rapidly.

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