How Collision Theory Affects Rate Of Reaction
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Collision theory can affect the rate of reaction by having an effect on what four things?
The nature of reactants Particle size Concentration Catalyst
Write a note on how collision theory can affect the rate of reaction through the nature of the reactants (2)
Reactions with covalent compounds involve bond breaking taking place during a collision This breaking of bonds requires energy and hence these types of reactions have a much higher activation energy than reactions which merely involve oppositely-charged ions colliding with each other in solution
What must happen in all reactions with covalent compounds?
Bond breaking must take place during a collision
During a reaction with covalent compounds, when must bond breaking occur?
During a collision
What is required to break bonds?
Energy
In general why do reactions with covalent compounds require more energy than those with ionic compounds.
Because energy is required to break the bonds in covalent compounds
Why do reactions involving ions not require a large amount of energy?
As these merely involve oppositely-charged ions colliding with each other in solution
Write a note on how collision theory can affect the rate of reaction through particle size. (2)
The smaller the particle size, the more surface are is exposed and, therefore, the greater the number of collisions taking place Since the number of collisions that take place is greatly increased, the number of these collisions that are effective will also increase
Why does the smaller particle size mean a greater number of collisions will take place?
Because the smaller the particle size, the more surface are that is exposed
Write a note on how collision theory can affect the rate of reaction through concentration. (2)
If the concentration of the reactants is increased, the number of collisions will also be increased because the particles are closer together Therefore, the number of effective collision will be increased giving rise to an increased rate of reaction
Why is the number of collisions increased if the concentration of the reactants is increased?
Because the particles are closer together
Write a note on how collision theory can affect the rate of reaction through catalysts.
A catalyst works by providing an alternative reaction pathway with a lower activation energy Therefore, more reactant molecules now posses the energy required for effective collisions to occur Therefore, the rate of reaction increases
How does a catalyst work?
A catalyst works by providing an alternative reaction pathway with a lower activation energy
A catalyst provides an alternative reaction pathway with a lower activation energy, how does this affect rate of reaction?
This allows more reactant molecules to posses the energy required for effective collisions to occur