The activation energy is defines as the minimum energy which particles need to collide to start a reaction.
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Maxwell-Boltzmann distribution
The Maxwell-Botzman energy distribution shows the spread of energies that molecules of a gas or liquid have at a particular temperature.
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Increasing temperature
As the temperature increases the distribution shifts towards having more molecules with higher energies.
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Rates of reaction
The rate of reaction is defined as the change in concentration of a substance in unit time.
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Effect of increasing concentration and pressure
At higher concentrations (and pressures) there are more particles per unit volume and so the particles collide with a greater frequency and there will be a higher frequency of effective collisions.
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Catalyst
Catalysts increase the rate of reaction without getting used up. They do this by providing an alternative route or mechanism with a lower activation energy.
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Effect of increasing surface area
Increasing surface area will cause collisions to occur more frequently between the reactant particles and this increases the rate of reaction.
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Heterogeneous catalyst
They are usually solids whereas the reactants are gaseous or in the solution.
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Other cards in this set
Card 2
Front
The Maxwell-Botzman energy distribution shows the spread of energies that molecules of a gas or liquid have at a particular temperature.
Back
Maxwell-Boltzmann distribution
Card 3
Front
As the temperature increases the distribution shifts towards having more molecules with higher energies.
Back
Card 4
Front
The rate of reaction is defined as the change in concentration of a substance in unit time.
Back
Card 5
Front
At higher concentrations (and pressures) there are more particles per unit volume and so the particles collide with a greater frequency and there will be a higher frequency of effective collisions.
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