10.2 Catalysts Flashcards
What is a catalyst?
A substance that changes the rate of reaction without any permanent change itself
What features do catalysts have?
Catalysts are not used up in a reaction
Catalysts can react with the reactant to form an intermediate or provide a surface for the reaction to take place
Catalyst is regenerated at the end of the reaction
How does a catalyst increase the rate of reaction?
Provides an alternate reaction pathway of lower activation energy
What is a homogenous catalyst?
A catalyst in the same physical state as the reactants
What happens when a homogenous catalyst is used?
The catalyst reacts with the reactant to form an intermediate
The intermediate then breaks down to give the product and regenerate the catalyst
Give two examples of a homogenous catalyst being used
Making esters with sulphuric acid as a catalyst (all liquids)
Ozone depletion with Cl radical (all gases)
What is a heterogenous catalyst?
A catalyst with a different physical state to the reactant
What happens when a heterogenous catalyst is used?
Reactant molecules are absorbed (weakly bonded) to the surface of the catalyst
Later the product molecules leave the surface of the catalyst
via desorption
What is the advantage of using catalysts?
Less energy so less electricity or fossil fuel is needed