Table of Contents
- 1 What industrial processes use catalysts?
- 2 What are two advantages of using catalysts in industrial reactions?
- 3 Why are catalysts used in industrial processes involving reversible reactions?
- 4 Why do industry use heterogeneous catalysts?
- 5 Why do catalysts make it easier for reactions to proceed?
- 6 Why are different catalysts used?
- 7 Why is heterogeneous catalyst preferred in industrial processes than homogenous catalyst?
- 8 How does automobile industry benefits from catalysts?
What industrial processes use catalysts?
Heterogeneous catalysis
Process | Catalyst |
---|---|
Catalytic cracking of gas oil | Zeolite |
Reforming of naphtha | Platinum and rhenium on alumina |
Making epoxyethane | Silver on alumina |
Making sulfuric acid | Vanadium(V) oxide on silica |
What are two advantages of using catalysts in industrial reactions?
Catalysts speed up the rate of reactio, which saves money because the plant doesn’t have to operate for as long to produce the same amount of product. Catalysts allow the reaction to work at a much lower temperature. This reduces the energy used up in a reaction which is good for sustainable development.
Why are catalysts used in industry GCSE?
A catalyst provides an alternative reaction pathway that has a lower activation energy than the uncatalysed reaction. However, it does increase the frequency of successful collisions because more particles have energy greater than the activation energy, therefore there are more successful collisions.
Why are catalysts used in industrial processes involving reversible reactions?
Using a catalyst Catalysts do not change the equilibrium concentrations of reacting substances in reversible reactions. It also allows a lower temperature to be used, which saves energy but also increases the yield of the reaction.
Why do industry use heterogeneous catalysts?
Heterogeneous catalysts play an important role in industrial chemical production. They are preferred due to their robustness and lower operational cost, in particular through easier recovery/separation from the products allowing chemical processes to be streamlined.
How does catalysts play an important role in production of biofuels?
The presence of catalyst increases the rate of the reaction, thereby increasing the yield of the product. Various catalysts are used in the transesterification process for biodiesel production.
Why do catalysts make it easier for reactions to proceed?
Catalysts make this process more efficient by lowering the activation energy, which is the energy barrier that must be surmounted for a chemical reaction to occur. As a result, catalysts make it easier for atoms to break and form chemical bonds to produce new combinations and new substances.
Why are different catalysts used?
A catalyst is a substance which changes the rate of reaction but is unchanged at the end of the reaction. Only a very small amount of catalyst is needed to increase the rate of reaction between large amounts of reactants….Effect of catalysts.
Catalyst | Reaction catalysed |
---|---|
Vanadium(V) oxide | Making sulfuric acid |
Why are industrial processes important?
The process actually used in industry is the one that allows the material to be produced at the lowest possible cost. Chemists in industry study chemical changes to find out the most convenient and economical way of using them to make the product required.
Why is heterogeneous catalyst preferred in industrial processes than homogenous catalyst?
Homogeneous catalysts occupy the same phase as the reaction mixture, while heterogeneous catalysts occupy a different phase. Homogeneous catalysts allow for greater interaction with the reaction mixture than heterogeneous catalysts.
How does automobile industry benefits from catalysts?
The automotive catalyst is used in the exhaust system of vehicles to control the emission of harmful gases, such as hydrocarbons, carbon oxides, nitrogen oxides, and other particulate matter, into the atmosphere. It helps convert harmful gases into less toxic gases such as nitrogen and carbon dioxide.