1. Kinetics Thermodynamics : spontaneity of reaction
G < 0 spontaneous
2H2(g) +O2(g)  2H2O(l)
Go = -474 kJ
Go = Ho - TSo
a) low T
b) high T
Ho
< 0
favorable
So
< 0
unfavorable
Thermodynamically spontaneous
very slow

2. Kinetics Kinetics: rates of reaction mechanism of reaction 2 H2(g) +
O2(g)
2 H2(g) +
 2 H2O(l)
Greaction < 0
Greactants
Gproducts
thermodynamics
kinetics

3. P.E.n-e Kinetics qn qe r 2H2(g) + O2(g) 2 H2O(l) Go = -474 kJ
spontaneous + - + -
P.E.n-e - +
qn qe r

4. Low Temperature

5. High Temperature

6. High Temperature
endothermic
P.E.
exothermic
r (distance) + -

7. Kinetics rate of reaction [reactant] decrease increase [product]
1. Temperature (K.E.)
2. Concentration
3. Orientation

8. differential rate laws
A + B  C
a) +
b) - -
[A] = -
[B] =
 t
[C]
 t
rate = +
 t
A + B  2 C
- [A] =
 t
rate =
- [B] =
 t
[C]
 t 1 2 
A + B  C +

9. [ ] 50
100 x
t (min)
100
100 x 1 72 72 28 x x x x
time (min) 1 2 3 4 5
[ ] = t 81
- 0
= 16.2 min-1
ave. rate = 5
- 0
ave. rate =
-[ ] = t -
( )
- 100 =
16.2 min-1 5
- 0

10. x
time (min) 1 2 3 4 5
[ ] 50
100
t (min)
100 1 72 28
ave. rate = -
= 16.2 min-1
overall
(19
- 100) 5
- 0
ave. rate =
1st minute
- ( )
- 100
= 28.0 min-1
1 - 0
ave. rate =
- 27)
= 8.0 min-1
5th minute
- (19 5
- 4

11. slope of line tangent to curve = instantaneous ratex
time (min) 1 2 3 4 5
[ ] 50
100
slope of line tangent to curve =
instantaneous rate
at t = 0
initial rate
fastest rate

12. k = rate constant rate  [reactant] = k [reactant] t instantaneous
(min) rate k
= rate
[reactant]
100
33.0
0.33
0.33
0.33
0.33
0.33
0.33
rate  [reactant] =
k [reactant]
k = rate constant

13. [A]a [B]b [C]c ... rate = (-D[A]) k = D t k = rate [reactant] k
independent of [reactants] k
dependent on Temperature
[A]a
[B]b
[C]c
...
rate =
(-D[A]) k =
D t
k, a, b and c
determined experimentally
isolation method