1. Hour Exam II Wednesday, March 15 7:00 – 9:00 pm 103 Mumford
Hall AQG, AQI
Allen AQJ
Blair AQF
150 Animal Science
Fisher AQB, AQC
Koys AGD
Pearson AQA
conflict exam
4:30 – 6:30
162 Noyes

2. 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

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

4. 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

5. Low Temperature

6. High Temperature

7. High Temperature
exothermic
endothermic + +

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

9. differential rate laws
A + B  C
a) +
b) - -
d[A] = -
d[B] = dt
d[C] dt
rate = + dt
A + B  2 C
- d[A] = dt
rate =
- d[B] = dt
d[C] dt 1 2 
A + B  C +

10. [ ] 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

11. 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

12. 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

13. 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

14. [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

15. [A] [A] Exp. 1 [B]i [A]i initial rate (M) (M) (M s-1) 1.0 1.0
t (ms)
Concentration (M)
[A]
t (ms)
Concentration (M)
[A]
[B]i
[A]i
initial rate
(M)
(M)
(M s-1)
1.0
1.0
1.0 x 10-3
Exp. 2
[A]i [B]I initial rate
(M) (M) (M s-1)
2.0
1.0
2.0 x 10-3
Exp. 3
[A]i [B]I initial rate
(M) (M) (M s-1)
1.0
2.0
1.0 x 10-3

16. rate = k [A] 1st order reaction Exp. 1 rate = k [A]a [B]b
[A]i [B]I initial rate
(M) (M) (M s-1)
a = 0
a = 1
a = 2
rate 2 =
rate 1
2 x 10-3 =
1 x 10-3
[2.0]a
[1.0]a
1.0 x 10-3
Exp. 2
rate 3 =
rate 1
1 x 10-3 =
1 x 10-3
[2.0]b
[1.0]b
b = 0
b = 1
b = 2
[A]i [B]I initial rate
(M) (M) (M s-1)
2.0 x 10-3
rate = k
[A]
1st order reaction
Exp. 3
[A]i [B]I initial rate
(M) (M) (M s-1)
1x10-3 (M s-1) = k
[1.0 M]
k = 1 x 10-3 s-1
1.0 x 10-3