Activation energy (AQA GCSE Chemistry): Flashcards
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Definition of activation energy
Definition of activation energy
Minimum energy particles need to start a chemical reaction
Symbol for activation energy
Symbol for activation energy
What happens if particles collide without enough
What happens if particles collide without enough
They bounce off each other, no reaction occurs
What energy diagrams show
What energy diagrams show
How energy changes during a reaction
Product energy vs reactant energy in exothermic reactions
Product energy vs reactant energy in exothermic reactions
Products have less energy than reactants
Product energy vs reactant energy in endothermic reactions
Product energy vs reactant energy in endothermic reactions
Products have more energy than reactants
Energy change in exothermic reactions
Energy change in exothermic reactions
Energy is given out to the surroundings
Energy change in endothermic reactions
Energy change in endothermic reactions
Energy is taken in from the surroundings
First requirement for a chemical reaction to occur
First requirement for a chemical reaction to occur
Particles must collide
Energy requirement for successful particle collision
Energy requirement for successful particle collision
Must collide with at least the activation energy
Orientation requirement for successful particle collision
Orientation requirement for successful particle collision
Must collide at the correct angle
What catalysts do
What catalysts do
Speed up reactions without being used up themselves
How catalysts speed up reactions
How catalysts speed up reactions
Provide a different pathway with lower activation energy
Do catalysts change the overall energy change of a reaction?
Do catalysts change the overall energy change of a reaction?
No, the overall energy change stays the same
Do exothermic reactions need activation energy?
Do exothermic reactions need activation energy?
Yes, all reactions need activation energy