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Reaction Rate - Coggle Diagram
Reaction Rate
Collision Theory
collisions with enough energy
energy
increase temperature
particles have more energy
more likely to collide
explains why
different reaction occur at different rates
concentration
more molecules present
more collisions
Collision of molecules
must occur
for reaction to occur
suggests ways to change rate of reaction
correctly orientated
part of
Activation Energy
higher activation energy
slower reaction rate
barrier between reactants and products
enough energy
reaction occurs
not enough energy
no reaction
collide and bounce apart
still reactants
minimum amount of energy reactants must have
to undergo a reaction
increase temperature
why affect reaction rate
frequency and force of collision increase
energy level of molecules increase
reaction rate faster
Molecular Orientation
more complex molecules
fewer effective collsions
liquids and gases
constantly moving
high probability effective collision will occur
molecules need to collide with correct orientation
proper atoms line up with each other
bonds can break and reform
if not
bounce off each other
Factors Affecting
Temperature
increase in temperature
keeps activation energy same
increase particle kinetic energy
more molecules with higher energy
collide easier
rate of reaction increases
from absorbed heat
Concentration of reactants
Increase reactant concentration
more collisions occurring
number of molecules with energy increase
increase reaction rate
directly proportional to reaction rate
Surface Area
liquid can bump into solid on surface of solid only
Heterogenous reactions
rate of reaction increase
if stirred
faster reaction
increase surface area
more contact from solution
expose more solid particles to liquid
example
removal of harmful pollutants
catalytic exhausts
modern motor cars
such as
carbon monoxide
nitrogen oxides
unburnt fuel
Catalysts
heterogenous catalyst
reactant particles absorb to them
break or weaken bonds
no change to them
increase reaction rate
lower activation energy
example
biological
enzymes
definitions
reaction rate
rate of change of concentration over time
length of reaction
rate at which reactant used up
effective collision
chemical bonds broken
products forms
ineffective collision
no product formation