3618345
Description
Controlling the Rate
- Collision Theory
- Reactant molecules must collide
with enough energy for chemical
reaction to occur
- Activation energy (Ea) -
minimum kinetic energy
required for reaction to occur
- Activated Complex -
Intermediate stage, high
energy, unstable
arrangement of atoms
- Energy given out when new bonds
form as atoms rearranged into
product molecules
- Reactant molecules must collide
with enough energy for chemical
reaction to occur
- Reaction Rates
- average rate = change in quantity/change
in time
- relative rate =
1/t
- average rate = change in quantity/change
in time
- Altering Factors
- Temperature
- Temp increase, then
particles have more kinetic
energy and so an increased
chance of possible
collisions
- Temp increase, then
particles have more kinetic
energy and so an increased
chance of possible
collisions
- concentration
- Conc increase, then more
particles, so more collisions so
increase in rate of reaction
- Conc increase, then more
particles, so more collisions so
increase in rate of reaction
- Particle size
- Particle size decrease, then larger
surface area, increased chance of
collisions, faster rate
- Particle size decrease, then larger
surface area, increased chance of
collisions, faster rate
- Use of Catalyst
- Lowers Activation Energy,
provides alternative route,
provides surface for reaction to
occur on
- Homogenous - same state
Heterogenous - different state
- Lowers Activation Energy,
provides alternative route,
provides surface for reaction to
occur on
- Temperature
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