A-level Chemistry Reaction rates and equlibrium
- Created by: joshhaigh15
- Created on: 22-04-21 11:52
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- Reaction Rates and Equilibrium
- Collisions
- Concentration
- Pressure
- Untitled
- Catalysts
- Homogeneous
- when catalysts and reactants are the same state
- Hetrogeneous
- when catalysts and reactants are different states
- Homogeneous
- Boltzmann Distribution
- Area under graph show the concentration of particles
- Activation energy- the energy required to start a reaction
- Catalysts lower activation energy meaning more molecules react and are produced speed up reaction Alternative route
- Catalysts
- Homogeneous
- when catalysts and reactants are the same state
- Hetrogeneous
- when catalysts and reactants are different states
- Homogeneous
- Catalysts
- Catalysts lower activation energy meaning more molecules react and are produced speed up reaction Alternative route
- Dynamic equilibrium
- Rate of reaction is the same forward as it is reverse Concentration is constant
- Chandelier Principle
- Pressure
- Higher pressure = shift to side with fewer gas molecules
- Low pressure = shift to side with greater gas molecules
- temperature
- Endothermic
- High temp = shift to right
- Low temp = shift to left
- Positive
- Exothermic
- High temp = shift to left
- Low temp = shift to right
- Negative
- Endothermic
- conentration
- More product shift left
- More Reactant shift right
- when equilibrium changes shifting the system to have minimal effect
- Pressure
- Equilibrium constant
- Kc=[E]eX[D]d/[A]aX[B]b
- Collisions
- Chandelier Principle
- Pressure
- Higher pressure = shift to side with fewer gas molecules
- Low pressure = shift to side with greater gas molecules
- temperature
- Endothermic
- High temp = shift to right
- Low temp = shift to left
- Positive
- Exothermic
- High temp = shift to left
- Low temp = shift to right
- Negative
- Endothermic
- conentration
- More product shift left
- More Reactant shift right
- when equilibrium changes shifting the system to have minimal effect
- Pressure
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