According to the adsorption theory of catalysis, the speed of the reaction increase because:
- The concentration of reactant molecules at the active centers of the catalyst becomes high due to adsorption
- In the process of adsorption, the activation energy of the molecules becomes large
- Adsorption produces heat which increases the speed of the reaction
- Adsorption lowers the activation energy of the reaction.
The Correct Option is D
Solution and Explanation
According to the adsorption theory of catalysis, the speed of a reaction increases because adsorption of reactant molecules onto the surface of the catalyst lowers the activation energy barrier for the reaction. This makes it easier for reactant molecules to undergo the reaction and increase the reaction rate.
So, the correct option is (D): Adsorption lowers the activation energy of the reaction.
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Concepts Used:
Catalysis
All reactants need to overcome certain energy, better known as activation energy in order to form products. This activation energy is the difference between the energy of the transition state and the reactant species.
Types of Catalysis:
Catalysis of chemical reactions is generally divided into two categories:
- Homogeneous Catalysis: Homogeneous catalysis of chemical reactions is a process where the reactants involved in the reaction and the catalyst are in the same phase. For example hydrolysis of sugar in the presence of sulphuric acid.
- Heterogeneous Catalysis: Heterogeneous catalysis of chemical reactions is a process where the reactants involved in the reaction and the catalyst are in different phases. For example reaction of hydrogen and nitrogen in the presence of finely divided iron to form ammonia.