Summary Unit 3.1.5. - Kinetics

3. 1. 5. KINETICS
=
enables chemists to determine how change in conditions affects the speed of Chem reaction
.




3. 1. 5. 1. COLLISION THEORY

activation (Ea) to
energy required
minimum for reaction
energy
-
-
a occur

reactions can
only occur when collisions take place between particles HAVING SUFFICIENT ENERGY
-




energy equal
most collisions t reaction not
enough particles have or
greater than Ea
-




3. 1. 5.2 MAXWELL BOLTZMANN DISTRIBUTION the distribution of of molecules (question specific) at
energies a
- =
.




a
most probable particular temperature
number of ,




A:÷÷:*
molecules 1
atoms lions ,
average energy
particles no
upper limit
important features :



"


: :canomie:c::
"

item: one:times:: :: :*:
two particles
! no for a molecule no touch Kross of x-axis
mat
energy
-




!
thwarting :Yi:B molecules with
energy greater than equal to Ea are able to react



no
energy lost
from the
system when collide
-




of l
in sample gas liquid molecules & HAVE HIGH EVERY
:
some
-




MOVE FAST

MOVE SLOWLY & HAVE LOW ENERGY

MAJORITY -


AVERAGE ENERGY



increased temperature




µt
(more
energy)
lower peak higher peak
-




-




to the
right
-



c
decrease
:*:p::
'




y J


energy mmmm
Ea
catalyst lowers Ea energy
mmm
-
-



Ea
Eat catalyst Eat catalyst