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Rates of reaction
The rate of reaction is the speed at which a chemical reaction takes place ­ this is measured
by the rate at which either products are formed or reactants are used up.

Successful collisions
In order for a chemical reaction to occur reacting particles need to collide…

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If you increase the pressure of a gas there will be more particles in a given volume of the gas
and the gas molecules will be closer together which means that the particles will collide more
frequently increasing the chance of successful collisions and increasing the rate of reaction.

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Definition: A catalyst is a substance that changes the speed of reaction without
being used up or changed in the reaction

Catalysts lower the activation energy ­ the minimum energy that the reacting particles need
to collide with in order to react and form a product. This means that a…

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The rate of reaction can either be measured by how quickly the reactants are
used up or how quickly the products are formed.

It can be calculated using this:
Amount of product formed or amount reactants used / time
So if I has 50cm3 of gas produced in 2 minutes…

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Need to explain graphs

The loss in mass happened faster at first as more reacting particles
available to react with each other, more reacting particles increased the
frequency of collisions and increased chance of successful collisions occurring
­ increasing the rate of reaction. However as the reaction continues the loss…

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