inetics
rate and collision theory
rate of reaction change of concentration amountof a reactant or product pe
nit time chang time
not all collisions result in a reaction
collision theory
for a reaction to occur the particlesmust collide in the rightdirection and
vision must have energygreater than or equal to the activation energy of the
eaction activation energy minimum amount ofenergyrequired for a reaction
o occur
Maxwell Boltzmann Distribution
shows energy in gas particles they move at differentspeeds so have
different amounts of kinetic energy
graph starts at 10,0 as no particles have zero
kinetic energy
graph is equal to the total number
area under
of molecules in the sample
changing reaction conditions will alter the shape
of the curve so that the number of particleswith
energy greater than the activation energy is
different
effect of temperature increased
emperature means increased kinetic
nergy so collisions occur more often and
with greaterenergy in a given time so rate
f reaction increases
maxwell boltzmann distribution
hifts to the right
effect of conc and pressure when conc is increased more molecule
Courin the same volumemeaningthey are packed closer together collisions
ecome more likely and chance of collision occurring with energy greater
han the activation energy increases increasing pressure has a similar
ffect as molecules are packed closer together into a smaller volume
no effect on Maxwell Boltzmann distribution as kinetic energy of
articles does not change
effect ofcatalyst catalyst increase rate of
e action without beingusedup in the reaction s it
rovides an alternative reaction path that requires
lower activation energy
rate and collision theory
rate of reaction change of concentration amountof a reactant or product pe
nit time chang time
not all collisions result in a reaction
collision theory
for a reaction to occur the particlesmust collide in the rightdirection and
vision must have energygreater than or equal to the activation energy of the
eaction activation energy minimum amount ofenergyrequired for a reaction
o occur
Maxwell Boltzmann Distribution
shows energy in gas particles they move at differentspeeds so have
different amounts of kinetic energy
graph starts at 10,0 as no particles have zero
kinetic energy
graph is equal to the total number
area under
of molecules in the sample
changing reaction conditions will alter the shape
of the curve so that the number of particleswith
energy greater than the activation energy is
different
effect of temperature increased
emperature means increased kinetic
nergy so collisions occur more often and
with greaterenergy in a given time so rate
f reaction increases
maxwell boltzmann distribution
hifts to the right
effect of conc and pressure when conc is increased more molecule
Courin the same volumemeaningthey are packed closer together collisions
ecome more likely and chance of collision occurring with energy greater
han the activation energy increases increasing pressure has a similar
ffect as molecules are packed closer together into a smaller volume
no effect on Maxwell Boltzmann distribution as kinetic energy of
articles does not change
effect ofcatalyst catalyst increase rate of
e action without beingusedup in the reaction s it
rovides an alternative reaction path that requires
lower activation energy
