Topic 5

Created by: Jemma1494
Created on: 03-06-21 12:12

How does a catalyst effect a reaction

It increases the rate of reaction by providing an alternate reaction pathway with a lower activation energy

This mean as more particles have enough energy to collide and react

A catalyst isn’t used up in a reaction

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Homogeneous catalyst

Catalyst in the same phase as the reactants

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Heterogeneous catalyst

Catalyst in a different phase to the reactants

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Collision theory

The number of successful collisions per unit time

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What effect does increasing temperature have on number of successful collisions

Increases due to particles having more thermal energy to collide and react

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What effect does increasing the surface area have on number of successful collisions

Increases due to particles having more area to collide with and react

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What effect does adding a catalyst have on number of successful collisions

Increases due to particles requiring less energy to collide and react

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What effect does increases the pressure have on number of successful collisions

Increases do to particles being closer together and colliding more frequently

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What effect does increasing concentration have on number of successful collisions

Increases due to more particle to collide and react

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What effect does increasing light have on number of successful collisions

Increases due to particles having more energy and being more likely to react

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Maxwell Boltzmann graph at higher temp

Graph moves to the right and down

Larger proportion of particles over the activation energy

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Maxwell Boltzmann graph at lower temp

Graph moves to the left and up

Smaller proportion of particles over the activation energy

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Other cards in this set

Card 2

Front

Homogeneous catalyst

Back

Catalyst in the same phase as the reactants

Card 3

Front

Heterogeneous catalyst

Back

Card 4

Front

Collision theory

Back

Card 5

Front

What effect does increasing temperature have on number of successful collisions

Back

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Topic 5