Collision Theory Experiment
1. Temperature increasers the number of collisions. When the
temperature is increased the particles all move quicker. If
they're moving quicker, they are going to have more collisions.
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2. Concentration (or pressure) increases the number of collision. If
the solution is made more concentrated it means there are more
particles of reactants knocking about between the water molecules,
which make collisions between the important particles more likely.
In a gas, increasing the pressure means the molecules are more
squashed up together so there are going to be more collision.
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3. Size of solid particles (or surface area) increases collisions.
If one of the reactants is a solid than breaking it up into
smaller pieces will increase its surface area. This means that the
particles around it in the solution will have more area to work on
so there will be more useful collisions.
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4. Catalysts increase the number of collisions. A catalyst works by
giving the reacting particles a surface to stick to where they can
bump into each other. This obviously increases the number of
collisions too.
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Faster collisions increase the rate of reaction
High temperatures also increase the energy of the collision, because
it makes all the particles move faster.
Faster collisions are only caused by increasing the temperature.
Reactions only happen if the particles collide with enough energy. At
a higher temperature there will be more particles colliding with
enough energy to make the reaction happen. This initial energy is
known as the activation energy, and it is needed to break the initial
bonds.
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Rate: To work out rate you the following:
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