Why Is Catalysis Important in Chemical Reactions?
What Does Catalyst Mean?
Catalysis definition or catalysis meaning can be given as the increase in the rate of a chemical reaction because of the participation of an additional substance, which is known as a catalyst. Catalyst is not consumed in the catalyzed reaction, but it can continue to act repeatedly. Even a small amount of catalyst is usually sufficient to bring about this effect. In contrast with the catalyzed mechanisms, usually, the catalyst reacts to generate a temporary intermediate, which then regenerates the original catalyst with the help of a cyclic process.
Mechanism of Catalysis
There requires less free energy to reach the transition state in the presence of a catalyst, but there will be no change in the total free energy from reactants to products. A catalyst can participate in various chemical transformations. Also, the effect of a catalyst may vary because of the presence of other substances such as promoters (which increases the activity and affect the temperature of the reaction as well) or inhibitors (which reduces the catalytic activity).
Catalyzed reactions carry lower activation energy (the rate-limiting free energy of activation) to that of the identical uncatalyzed reaction, resulting in a higher reaction rate for the same reactant concentration, at the same temperature. As in the case of other chemical reactions, the reaction rate completely depends upon the contact frequency of the reactants in the rate-determining step.
In this slowest step, the catalyst participates usually, and the reaction rate depends upon the amount of catalyst. Although catalysts are not consumed by the self reaction, they may be deactivated, inhibited, or destroyed by using the secondary processes.
Types of Catalysts
Based on whether the catalyst exists in the same phase as the substrate, catalysts are classified into Homogeneous and Heterogeneous catalysis. Biocatalysts (also called enzymes) are often seen as a separate group.
Heterogeneous Catalysts
These types of catalysts act in a different phase compared to the reactants. Most heterogeneous catalysts are solids that act either on the substrates of liquid or gaseous reaction mixture. At the same time, diverse mechanisms for the reactions on the surface are known, based on how the adsorption occurs.
The total surface area of a solid has a major effect on the reaction rate. The smaller the size of the catalyst particle, the larger the area of surface for a given mass of particles. A heterogeneous catalyst has active sites, which are called crystal faces or atoms where the reaction actually occurs. Most of the catalyst surface is catalytically inactive.
Electrocatalysts
In the electrochemistry context, specifically in fuel cell engineering, multiple metal-containing catalysts are used to enhance the half-reaction rates that comprise the fuel cell. A common type of fuel cell, named electrocatalyst is based upon the nanoparticles of platinum that are supported on the carbon particles, which are slightly larger. But, when in contact with one of the fuel cell electrodes, this platinum increases the oxygen reduction rate either to hydroxide or to water or hydrogen peroxide.
Homogeneous Catalysts
These function in the same phase as the reactants, but the mechanistic principles that are involved in the heterogeneous catalysis are generally applicable. Typically, the homogeneous catalysts are dissolved in a substrate solvent. An example of homogeneous catalysis can be the influence of H+ on the carboxylic acids’ esterification, like the formation of methyl acetate from methanol and acetic acid.
Photocatalysts
Photocatalysis is the process where the catalyst can receive light (like visible light), be promoted to an excited state, and then undergoes an intersystem crossing with the starting material, and then, returning to the ground state without being consumed. After that, the excited state of the starting material will undergo the reactions ordinarily. It could not be directly illuminated. For example, usually, the singlet oxygen is produced by photocatalysis. Photocatalysts are also considered as the primary ingredient in the dye-sensitized solar cells.
Enzymes and Biocatalysts
The enzymes and other biocatalysts are often treated as a third category. In comparison, the same mechanistic principles apply to homogeneous, heterogeneous, and biocatalysis.
Catalysis
In biology, enzymes are the protein-based compounds that catalyze metabolism and other biochemical reactions as well. Though enzymes are the most commonly called biocatalysts, certain non-protein-based biomolecules classes also exhibit the catalytic properties. These include ribozymes and synthetic deoxyribosymes and as well.
Biocatalysts are recognized to be an intermediate between the heterogeneous and homogeneous catalysts; soluble enzymes are considered to be homogeneous catalysts, whereas the membrane-bound enzymes can be kept under the heterogeneous enzymes category.
The catalysis impact factor or various factors affect the activity of enzymes (and other catalysts as well). A few of these include pH, temperature, the concentration of enzyme, products, and substrate. Water is an important reagent that acts as a catalyst. It acts in multiple bond-forming and bond-breaking reactions as well.
FAQs on Catalysis in Chemistry: Types, Mechanism & Applications
1. What exactly is catalysis in Chemistry?
Catalysis is the process of increasing the rate of a chemical reaction by adding a substance known as a catalyst. The catalyst itself is not consumed in the overall reaction, meaning it can be recovered chemically unchanged at the end.
2. What is the difference between catalysis and a catalyst?
These terms are related but distinct. Catalysis refers to the entire process or phenomenon of changing a reaction's speed. A catalyst is the actual substance that you add to make this process happen. For example, iron is the catalyst used in the catalysis of ammonia production.
3. What are the main types of catalysis?
There are two primary types of catalysis based on the physical state of the reactants and the catalyst:
- Homogeneous Catalysis: The catalyst is in the same phase (e.g., liquid, gas) as the reactants. An example is the acid-catalysed hydrolysis of esters.
- Heterogeneous Catalysis: The catalyst is in a different phase from the reactants. A common example is the use of solid nickel to catalyse the hydrogenation of vegetable oils (liquids).
4. Why is catalysis so important in real-world industries?
Catalysis is crucial because it allows industrial processes to happen faster, at lower temperatures, and with greater efficiency, saving energy and costs. For instance, it is vital in the Haber-Bosch process for making ammonia (for fertilisers) and in catalytic converters in cars to reduce pollution.
5. How does a catalyst actually speed up a reaction?
A catalyst speeds up a reaction by providing an alternative reaction pathway that has a lower activation energy. Think of it as creating a shortcut or an easier route for the reactants to become products. Since less energy is needed to start the reaction, more molecules can react in a given time, increasing the reaction rate.
6. What are enzymes and how do they relate to catalysis?
Enzymes are highly specific biological catalysts made of proteins. They speed up the millions of chemical reactions that occur in living organisms, from digesting food to building DNA. This process is known as enzymatic catalysis, and it is essential for life.
7. Can a reaction's own product act as a catalyst?
Yes, this phenomenon is called autocatalysis. It occurs when one of the products of a reaction also serves as a catalyst for that same reaction. For example, in the oxidation of oxalic acid by potassium permanganate, the manganese(II) ions (Mn²⁺) produced act as a catalyst, causing the reaction to speed up as it progresses.
8. What is the difference between a catalyst and a promoter?
A catalyst directly participates in the reaction to change its rate. A promoter, on the other hand, is a substance that doesn't have catalytic activity on its own but increases the efficiency of a catalyst when added to it. For example, in the Haber-Bosch process, molybdenum acts as a promoter for the iron catalyst.
9. Can a substance slow down a reaction instead of speeding it up?
Yes, a substance that slows down a chemical reaction is called an inhibitor or a negative catalyst. Inhibitors work by increasing the activation energy or by blocking the active sites of a catalyst, making it less effective. They are used in processes where reaction control is critical, like in food preservation.
