Rates of Reactions
- Created by: Lena Fray
- Created on: 17-09-15 12:28
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- Rate Of Reactions
- Calculation
- Rate of Reaction = Amount of reactant used or amount of product formed
- divided by time
- Rate of Reaction = Amount of reactant used or amount of product formed
- Activation Energy
- The minimum amount of energy need for a reaction to happen
- If there is not enough energy then....
- There is no reaction
- They the particles collide with enough energy then...
- They react and form a product
- If there is not enough energy then....
- The minimum amount of energy need for a reaction to happen
- Factors that effect it
- Catalysts
- lower the activation need
- So more particles are able to react
- They are NOT used up
- lower the activation need
- Concentration/Pressure
- means there are more reacting particles in the solution
- A higher ratio
- this means more reactions happen
- means there are more reacting particles in the solution
- Temprature
- Increasing makes the reaction faster
- because it gives the particles more energy
- So they are more likely to collide
- as they will hold at least the activation energy.
- So they are more likely to collide
- because it gives the particles more energy
- Increasing makes the reaction faster
- Surface Area
- The larger the surface are the faster the reaction.
- the more reacting particles exposed
- so more collisions happen
- the more reacting particles exposed
- The larger the surface are the faster the reaction.
- Catalysts
- Measuring
- Whats produced
- Make sure you state the length of time
- Volume produced
- Mass
- Whats produced
- Collision Theory
- Parties must collide with sufficient energy in order to react
- This is known as ACTIVATION ENERGY
- Parties must collide with sufficient energy in order to react
- Calculation
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