Kinetics Revision Notes

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  • Created on: 03-04-16 10:06
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Kinetics
Collision Theory
Reactions only occur when collisions take place between particles having sufficient energy. This is
called activation energy.
Activation energy ­ min. amount of KE required for particles to react.
Most collisions do not lead to a reaction because most particles don't have enough activation
energy.
MaxwellBoltzmann Distribution
Area below curve is equal to total No. of molecules
Effect of Temperature
Rate of reaction is how fast or slow a reaction takes place.
When molecules move around faster they collide more often. This is why inc. temp. Makes rate of
reaction faster so a small temperature increase can lead to a large increase in rate of reaction.
Effect of Concentration
Inc. conc. of reactants in solution particles will be closer together so collisions are more frequent.
If collisions more frequent then they'll be more chance particles react.

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Effect of Pressure
If reaction involves gases then inc. pressure of gases works the same way. Raising pressure pushes
all gas particles closer so increases No. in given vol. This increased frequency of collisions which
increases rate.
Catalysts
A substance that inc. rate of chemical reaction without being changed in chemical composition or
amount.
Catalysts work by providing alternative reaction route of lower activation energy.…read more

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