What is the Difference Between Homogeneous and Heterogeneous Catalyst?
🆚 Go to Comparative Table 🆚The main difference between homogeneous and heterogeneous catalysts lies in the phase they occupy during the reaction. Here are the key differences:
- Homogeneous Catalysts:
- These catalysts exist in the same phase (gas or liquid) as the reactants.
- They are typically made up of only one mechanism.
- Homogeneous catalysts usually have well-defined active sites, with catalysts often being single-atom transition metals stabilized by ligands.
- Separation of products from the catalyst is generally expensive, as the only exception is in biphasic catalysis.
- Heterogeneous Catalysts:
- These catalysts are in a different phase from the reactants.
- Heterogeneous catalysts are made up of multiple mechanisms.
- Their active sites are not well-defined, as they might be only a few percent of the metal (usually small particles), and different zones of the same particle might have different active sites.
- Separation of products from the catalyst is usually straightforward.
In summary, homogeneous catalysts are in the same phase as the reactants and have well-defined active sites, while heterogeneous catalysts occupy a different phase and have less well-defined active sites.
Comparative Table: Homogeneous vs Heterogeneous Catalyst
Here is a table comparing the differences between homogeneous and heterogeneous catalysts:
| Feature | Homogeneous Catalysts | Heterogeneous Catalysts |
|---|---|---|
| Phase | Occupy the same phase as the reactants (gas or liquid) | Occupy a different phase from the reactants |
| Interaction | Greater interaction with the reaction mixture due to being in the same phase | Less interaction with the reaction mixture because they are in different phases |
| Separation | Difficult to separate from the reaction mixture | Easier to separate from the reaction mixture |
| Examples | Reaction between persulfate ions and iodide ions | Hydrogenation of alkenes on a solid catalyst |
Both homogeneous and heterogeneous catalysts function to lower the activation energy required for a reaction to occur. However, homogeneous catalysts have a higher degree of interaction with the reaction mixture due to being in the same phase, while heterogeneous catalysts have a lower degree of interaction because they are in different phases.
- Homogeneous vs Heterogeneous Reactions
- Homogeneous vs Heterogeneous
- Homogeneous vs Heterogeneous Nucleation
- Homogeneous vs Heterogeneous Equilibrium
- Catalyst vs Enzyme
- Organic vs Inorganic Catalysts
- Catalyst vs Reagent
- Catalytic vs Non Catalytic Reaction
- Catalytic vs Stoichiometric Reagents
- Catalyst vs Inhibitor
- Positive vs Negative Catalyst
- Homogeneous vs Isotropic
- Catalyst vs Intermediate
- Homocyclic vs Heterocyclic Compounds
- Pure Substance vs Homogeneous Mixture
- Homolysis vs Heterolysis
- Photocatalysis vs Electrocatalysis
- Catalytic Cracking vs Hydrocracking
- Homolytic vs Heterolytic Fission