rate of reaction
- Created by: Margaret Hobart
- Created on: 04-05-21 08:46
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- reaction rates
- rate of reaction = amount of product used/formed / time (s)
- increase in pressure (only affects gases)
- same number of particles are now in a smaller space
- more frequent successful collisions of reactant particles
- number of particles in same space increases
- increased exposure of reactants
- more frequent successful collisions of reactant particles
- same number of particles are now in a smaller space
- increase in concentration of reactants
- number of particles in same space increases
- increases in temperature
- particle energy and speed increases
- more frequent successful collisions of reactant particles
- increased exposure of reactants
- more frequent successful collisions of reactant particles
- particle energy and speed increases
- increase in surface area of reactants
- use a powdered reactant for a larger SA
- collision theory
- A reaction will only take place if the particles collide with sufficient energy and correct orientation
- activation energy
- minimum energy required
- catalysts increase rate of reaction by providing an alternate pathway
- lowers activation energy
- maxwell-boltzmen distribution curve
- shape of graph is the same except Ea is reduced
- catalysts increase rate of reaction by providing an alternate pathway
- lowers activation energy
- more molecules with energy excess of Ea
- catalysts increase rate of reaction by providing an alternate pathway
- different distributions at different temperatures
- for higher temperatures the graph moves to the right and the peak is lower - more particles with excess Ea
- no particles have 0 energy so graph doesn't start at 0
- peak = most probable energy of particles
- between peak and Ea is the average energy of particles
- total area doesn't change with condition as the total number of particles stays the same (exc. concentration)
- increasing concentrationincreses total area - higher peak
- shape of graph is the same except Ea is reduced
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