Describe how the enthalpy of a reaction remains unchanged when a catalyst is used in the reaction.
Describe how the enthalpy of a reaction remains unchanged when a catalyst is used in the reaction.
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 the 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 the products and the catalyst.
Catalysts do not participate in the reaction but increase the speed of the reaction.
The intermediate formed with the catalyst possesses much lower potential energy than the intermediate formed in the normal reaction. The following diagram shows the impact of using a catalyst on the potential energy and thus the activation energy.
Enthalpy of reaction (△H) is a state function and is defined as the difference in enthalpies between the products and the reactants.
The use of a catalyst lowers the activation energy but does not affect the enthalpies of the products and the reactants.
Thus, the enthalpy of the reaction remains unchanged when a catalyst is used in the reaction.
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 the 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 the products and the catalyst.
Catalysts do not participate in the reaction but increase the speed of the reaction.
The intermediate formed with the catalyst possesses much lower potential energy than the intermediate formed in the normal reaction. The following diagram shows the impact of using a catalyst on the potential energy and thus the activation energy.
Enthalpy of reaction (△H) is a state function and is defined as the difference in enthalpies between the products and the reactants.
The use of a catalyst lowers the activation energy but does not affect the enthalpies of the products and the reactants.
Thus, the enthalpy of the reaction remains unchanged when a catalyst is used in the reaction.
