Collision theory states that for a reaction to occur the reacting particles (atoms, ions or molecules) must collide together with enough energy to react
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Activation Energy
The minimum energy needed for a reaction to occur
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Successful Collisions
When reactant particles have achieved or exceeded the activation energy. They collide, bonds break and atoms are rearranged to form products
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Unsuccessful Collisions
Collisions that do not result in reaction and occur when reactant particles collide with less than the activation energy
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Rate
Rate is a measure of the speed at which reactants are changed into products
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Reaction Rate
The change of the concentration (amount) of a reactant or product with respect to time
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Maxwell-Boltzmann Distribution
Plot of the number of gaseous molecules against the energy they posses
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Catalyst
A substance that increases the rate of chemical reaction without itself being used up
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Homogeneous Catalyst
A catalyst that is in the same state as the reactants and products. It provides a reaction pathway of lower activation energy by forming an intermediate
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Heterogeneous Catalyst
A catalyst that is in a different state to the reactants and products. It works via chemisorption and provides and pathway of lower activation energy
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Chemisorption/Adsorption
Process where reactant molecules are absorbed onto the surface (sticks to surface) of the catalyst, bonds are weakened and product molecules are absorbed from the catalyst
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Other cards in this set
Card 2
Front
The minimum energy needed for a reaction to occur
Back
Activation Energy
Card 3
Front
When reactant particles have achieved or exceeded the activation energy. They collide, bonds break and atoms are rearranged to form products
Back
Card 4
Front
Collisions that do not result in reaction and occur when reactant particles collide with less than the activation energy
Back
Card 5
Front
Rate is a measure of the speed at which reactants are changed into products
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