10.2 Catalysts Flashcards

1
Q

What is a catalyst?

A

A substance that changes the rate of reaction without any permanent change itself

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2
Q

What features do catalysts have?

A

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

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3
Q

How does a catalyst increase the rate of reaction?

A

Provides an alternate reaction pathway of lower activation energy

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4
Q

What is a homogenous catalyst?

A

A catalyst in the same physical state as the reactants

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5
Q

What happens when a homogenous catalyst is used?

A

The catalyst reacts with the reactant to form an intermediate

The intermediate then breaks down to give the product and regenerate the catalyst

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6
Q

Give two examples of a homogenous catalyst being used

A

Making esters with sulphuric acid as a catalyst (all liquids)

Ozone depletion with Cl radical (all gases)

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7
Q

What is a heterogenous catalyst?

A

A catalyst with a different physical state to the reactant

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8
Q

What happens when a heterogenous catalyst is used?

A

Reactant molecules are absorbed (weakly bonded) to the surface of the catalyst

Later the product molecules leave the surface of the catalyst

via desorption

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9
Q

What is the advantage of using catalysts?

A

Less energy so less electricity or fossil fuel is needed

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