§9.3 the rate equation of reaction with simple order
TRANSCRIPT
§9.3 The rate equation of reaction
with simple order
Overall reactions
Reaction with definite order
Reaction without definite order
Reaction with simple order
1 12 2[H ] [I ]r kH2 + I2 = 2 HI
H2 + Cl2 = 2 HCl1 0.5
2 2[H ] [Cl ]r k
H2 + Br2 = 2 HBr0.5
2 2
2
[H ][Br ][HBr]
1 '[Br ]
r kk
It was found that reactions with same reaction order are usu
ally of same kinetic characteristics, therefore, reactions are us
ually classified on the basis of reaction order.
Reaction with simple order:
The reaction whose rate only depends on the
concentration of reactants, and both the partial order and
the reaction order is zero or plus integer is called reaction
with simple order.
r = kcn
n kinds
0 zeroth-order reaction
1 first-order reaction
2 second-order reaction
3 third-order reaction
order First Second Third Zeroth
Differential rate equation
Integrated rate equation
Linearity
Half-life
Unit of k
Comparison between reactions with different reaction orders
3.1 First-order reaction:
Reaction: A P
at t = 0 c0
at t = t c
Differential rate equation: 1
dck c
dt
can be rearranged into: 1
dck dt
c
Which can be integrated directly
01ln
ck t
c 0 1exp( )c c k t
0 1000 2000 3000 4000 5000
0.0
0.2
0.4
0.6
0.8
1.0
C /
mol
dm
-3
t / s
c~t curve of first-order reaction0 1exp( )c c k t
Only when t , can c 0, which suggests that, the first-order reaction can not complete.
0
2
cc 0
1lnc
k tc
Half-life
112
1
6932.02ln
kkt
0 1000 2000 3000 4000 5000
-5
-4
-3
-2
-1
0
ln(C
/mol
dm
-3)
t / s
lnc ~ t curve of the first-order reaction
0 1ln lnc c k t
The slope of the lnc ~ t curve is the k1
Characteristics of the first-order reaction
1) Unit of k is s-1
2) lnc is in linear proportion to t
3) can not complete
4) Half-life does not depend on c0
Example:
1) Decay of isotopes
2) Decomposition
226 226 488 86 2Ra Rn He
2 5 2 4 2
1N O N O O
2
3) Isomerization
Willard F. Libby
1960 Noble Prize
USA
1908/12/17 ~1980/09/08
Application of 14C for age determinations (radiocarbon dating)
Example:
The half-life of the first-order decay of
radioactive 14C is about 5720 years. The
natural abundance of 14C isotope is 1.1
10-13 mol% in living matter.
Radiochemical analysis of an object
obtained in an archeological excavation
shows that the 14C isotope content is 0.89
10-14 mol%.
3.2 Second-order reaction
2A P; A + B P
A + B P a b
cA= ax cB =bx
A2 A B
dCk C C
dt Differential rate equation:
))((2 xbxakdt
dx dtk
xbxa
dx2))((
txdtk
xbxa
dx0 20 ))((
txxdtk
xaba
dx
xbba
dx0 200 ))(())((
tkba
a
ba
xa
ba
b
ba
xb2)(
ln
)(
)ln(
)(
ln
)(
)ln(
tkxba
xab
ba 2)(
)(ln
)(
1
22
dck c
dt
When a = b
022
C
C
dck dt
c 2
0
1 1k t
c c
0 1000 2000 3000 4000 5000
0.0
0.2
0.4
0.6
0.8
1.0
C / m
ol d
m-3
t / s
c~t curve of second-order reaction
When c 0, t , which suggests that, the pure second-order reaction can not complete, either.
1/ 22 0
1t
k cHalf-life
0 1000 2000 3000 4000 50000
10
20
30
40
50
1/C
/ mol
dm
-3
t / s
1/c ~ t curve of second-order reaction
For pure second-order reaction
22
1
2
dck c
dt 2
0
1 12k t
c c
1/ 2
2 0
1
2t
k c
Characteristics of second-order reaction
1) Unit of k is mol-1dm3s-1
2) 1/c is in linear proportion to t
3) can not complete
4) Half-life1
02
1t
c
Increasing the initial concentration of the reactant will shorten the reaction time.
Example:
1) dimerization
2) decomposition 2 22HI = H + I
3) recombination
4) esterification 3 2 5
3 2 5 2
CH COOH+C H OH
CH COOC H +H O
→
5) hydrolysis C12H22O11 + H2O
C6H12O6 + C6H12O6
3 2 62CH = C H
C12H22O11 + H2O C6H12O6 + C6H12O6
In 1850, experiment done by Wilhelmy suggested that the rate equation of the reaction is:
12 22 11[C H O ]r k
12 22 11 2[C H O ][H O]vr k
Because the amount of water keeps nearly unchanged during the reaction, [H2O] keeps nearly constant, and the rate equation can be
then simplified as
12 22 11'[C H O ]r k Pseudo first-order reaction
612 22 11 2 3[C H O ][H O] [H O ]r k
3.3 third-order reaction
3A P
A + B + C P
2A + B P
33
1
3
dck c
dt
32 20
1 1 13
2k t
c c
32 2
0
1 16k t
c c 1 2
3 02
1
2t
k c
3A P
For A + B + C P
with same initial concentration
33
dck c
dt Differential rate equation
32 20
1 1 1
2k t
c c
Integrated rate equation32 2
0
1 12k t
c c
1 23 02
3
2t
k c
Only five third-order gaseous reactions have been observed.
2NO + X2 N2O + X2O; X = H, D
2NO + O2 2NO2;
2NO + X2 2NOX; X = Br, Cl
Are these true third order reactions ?
r = k [C6H5CHO]2[CN-]
r = k [C2H4O][H+][Br-]
3.4 Zeroth-order reaction
A P
Differential rate equation 0
dck
dt
000
c t
cdc k dt 0 0c c k t 0
1/ 202
ct
k
When c = 0, the reaction completes, the reaction time is:
0
0
ctk
The zero-order reaction can complete.
0 1000 2000 3000 4000 50000.0
0.2
0.4
0.6
0.8
1.0
C /
mo
l dm
-3
t / s
0 1000 2000 3000 4000 50000.0
0.2
0.4
0.6
0.8
1.0
C /
mo
l dm
-3
t / s
c ~ t curve for zero-order reaction
Characteristics of zeroth-order reaction
1) Unit of k is mol dm-3s-1
2) c is in linear proportion to t
3) can complete
4) When c increases, reaction time will be prolonged.
0
0
k
Ct
Examples:
Decomposition over catalysts:
1) 2N2O 2N2 + O2 over Pt wire
2) 2NH3 N2 + 3H2 over W wire
Photochemical reaction:
r = k I
I: intensity of radiation
5.5 for nth-order reaction
nr kc
tkaxan nnn
}
1
)(
1{
1
111
1
1/ 2 1 10 0
2 1
( 1)
n
n n
At
n kc c
For n 1