Describe how the enthalpy of reaction remains unchanged when a catalyst is used in the reaction.

<p>This is a Long Answer Type Question as classified in NCERT Exemplar</p><p><strong>Ans:&nbsp;</strong>Catalyst action is a complicated concept. A catalyst aids in the formation of temporary bonds during a chemical reaction. The objective of a catalyst is to lowers the activation energy. A catalyst is a substance that increases the rate of a reaction without itself undergoing any permanent chemical change. The action of the catalyst can be explained by intermediate complex theory. According to this theory, a catalyst participates in a chemical reaction by forming temporary bonds with the reactants resulting in an intermediate complex. This has transitory existence and decomposes to yield products and the catalyst.</p><p>A small amount of the catalyst can catalyst a large number of reactants. A catalyst does not alter Gibbs energy? G of a reaction. The difference in energy between reactants and products is constant.</p><p>It is also found that a catalyst does not change the equilibrium constant of a reaction rather, it helps in attaining the equilibrium faster, that is, it catalyses the forward as well as the backward reactions to the same extent so that the equilibrium state remains the same enthalpy of reaction means the difference in energy between reactant and product it will also remain unchanged.&nbsp;</p>

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