Summary
Edexcel A level chemistry Kinetics II summary
- Module
- Unit 16 - Kinetics II
- Institution
- PEARSON (PEARSON)
Summary of the topic Kinetics II
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collision theory rateequation experimental
for a reaction to happen . . .
methods
( Ea )
-
particles must collide with enough energy rate =
K[A ]^[ B ]m titration : take samples
particles must collide at correct orientation
-
-
number /
frequency of collisions
htm = order overall out continuously to
Measure
.
↳ more particles liner SA ) cone of
cone incr pressure incr n = order , respect
w
Product
, ,
more collisions so
higher rate .
to A.
Ignites catalysis
pH
in pH
: measure
over time
change
µ
volume
catalyst
alltocatalllsis : reaction catalysed of gas
gain)
,
by product loss mass (or
of
heterogeneous i. reactant +
catalyst
ta Energy
indiff states . Reactant adheres to plot results against
1- ook catalyst surface .
↳ absorb I
1- = 200K /f
☒i -
-
sook
KINETICS
R
SN3 -
3°
mechanisms
,
2°
R R
practicals
fÉb Is :OH%ast
I °
slow
⑦ + *
initial rate iodine clock
: I3B . -
, '
s
-
c
'
• ,
R R
'
OH
R+ :X
R l
-
starch indicator g- @
R R
-
control : temp clean equipment
,
-
may misjude blue colour rate =k[CR3X ]
rate =k[ 5206 "
][ ]
-
I
• titnmetric : iodine proponent -
,
13A SN2
-
1°Csometimes 2° )
-
withdraw samples at time intervals -0
-0
add a base to stop reaction in sample : OH H
-
µ H
7/1 .g;;×/
"
( is acid catalysed )
by
" ,
fast i
and
sample eelith NA25 203
use s c
. .
titre 8-
-
Ho
My
-
.
-
⑥
starch indicator
-
record volume of Nazszo } R
volume Nazs 203 ✗ [ 12 ]
K[C11-2RX ][ OH ]
-
rate =
(not when
-
record time g- when quenched
withdrawn ) .
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