Hour Exam II. Wednesday, March 15. 7:00 – 9:00 pm. 103 Mumford HallAQG, AQI AllenAQJ BlairAQF. 150 Animal Science FisherAQB, AQC KoysAGD PearsonAQA. conflict exam 4:30 – 6:30 162 Noyes. Kinetics. Thermodynamics :. spontaneity of reaction. G < 0 spontaneous.
Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.
Hour Exam II
Wednesday, March 15
7:00 – 9:00 pm
103 Mumford
HallAQG, AQI
AllenAQJ
BlairAQF
150 Animal Science
FisherAQB, AQC
KoysAGD
PearsonAQA
conflict exam
4:30 – 6:30
162 Noyes
Thermodynamics :
spontaneity of reaction
G < 0spontaneous
2H2(g) +O2(g) 2H2O(l)
Go = 474 kJ
Go = Ho TSo
a) low T
b) high T
Ho
< 0
favorable
So
< 0
unfavorable
Thermodynamically spontaneous
very slow
thermodynamics
thermodynamics
rates of reaction
mechanism of reaction
O2(g)
2 H2O(l)
Greaction < 0
2 H2(g) +
Greactants
Gproducts
kinetics
qn qe
r
+
+
2H2(g) + O2(g)2 H2O(l) Go = 474 kJ
spontaneous
P.E.ne

+
Low Temperature
High Temperature
+
+
exothermic
endothermic
rate of reaction
[reactant]
decrease
increase
[product]
1. Temperature (K.E.)
2. Concentration
3. Orientation

1
2
A + B C

d[A] =
d[C]
dt
d[B] =
dt
a) +
b) 
+
rate =
dt
A + B 2 C
 d[A] =
dt
d[C]
dt
d[B] =
dt
rate =
A + B C
+
100
[ ]
50
0
1
2
3
4
5
time (min)
[ ] =
t
[ ] =
t
x
t (min)
0
100
100
0
x
72
1
72
28
x
2 52 52 48
x
x
3 37 37 63
x
4 27 27 73
5 19 19 81
81
 0
= 16.2 min1
ave. rate =
5
 0
(19 )
 100
ave. rate =

=
16.2 min1
5
 0
x
100
t (min)
0
100
100
0
x
[ ]
72
1
72
28
x
50
2 52 52 48
x
x
3 37 37 63
x
4 27 27 73
0
5 19 19 81
1
2
3
4
5
time (min)
overall
ave. rate =

(19
 100)
= 16.2 min1
5
 0
1st minute
ave. rate =
= 28.0 min1
 (72 )
 100
1  0
5th minute
ave. rate =
 27)
= 8.0 min1
 (19
5
 4
x
100
x
[ ]
x
50
x
x
x
0
1
2
3
4
5
time (min)
instantaneous rate
slope of line tangent to curve =
at t = 0
initial rate
fastest rate
t instantaneous
(min) rate
k
= rate
[reactant]
100
33.0
0
0.33
17223.8
25217.2
33712.2
4278.9
5196.3
0.33
0.33
0.33
0.33
0.33
rate [reactant] =
k [reactant]
k = rate constant
k = rate
[reactant]
k
independent of [reactants]
dependent on Temperature
k
[A]a
[B]b
[C]c
...
(d[A])
k
rate =
=
dt
k, a, b and c
determined experimentally
isolation method
[A]
[A]
Concentration (M)
Concentration (M)
t (ms)
t (ms)
Exp. 1
[B]i
initial rate
[A]i
(M)
(M)
(M s1)
1.0
1.0
1.0 x 103
Exp. 2
[A]i[B]I initial rate
(M)(M)(M s1)
2.0
1.0
2.0 x 103
Exp. 3
[A]i[B]I initial rate
(M)(M)(M s1)
1.0 x 103
1.0
2.0
Exp. 1
k
rate =
[A]a
[B]b
[A]i[B]I initial rate
(M)(M)(M s1)
1.01.0
a = 0
a = 1
a = 2
2 x 103 =
1 x 103
[2.0]a
[1.0]a
rate 2 =
rate 1
1.0 x 103
Exp. 2
1 x 103 =
1 x 103
rate 3 =
rate 1
[2.0]b
[1.0]b
b = 0
b = 1
b = 2
[A]i[B]I initial rate
(M)(M)(M s1)
2.01.0
rate =
k
[A]
2.0 x 103
1storder reaction
Exp. 3
[A]i[B]I initial rate
(M)(M)(M s1)
1.02.0
1x103(M s1) =
k
[1.0 M]
k = 1 x 103 s1
1.0 x 103