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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. - PowerPoint PPT Presentation
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Hour Exam II
Wednesday, March 15
7:00 – 9:00 pm
103 MumfordHall AQG, AQIAllen AQJBlair AQF
150 Animal ScienceFisher AQB, AQCKoys AGDPearson AQA
conflict exam4:30 – 6:30162 Noyes
Kinetics
Thermodynamics :
G < 0 spontaneous
2H2(g) +O2(g) 2H2O(l)
Ho So
Go = Ho - TSo
Thermodynamically spontaneous
spontaneity of reaction
Go = -474 kJ
a) low Tb) high T
very slow
favorableunfavorable
< 0< 0
KineticsKinetics
2 H2(g) +
rates of reactionmechanism of reaction
Greaction < 0
kinetics
O2(g) 2 H2O(l)
thermodynamics thermodynamics
Greactants
Gproducts
Kinetics
2H2(g) + O2(g) 2 H2O(l) Go = -474 kJspontaneous
P.E.P.E.n-en-e
qn qe
r
+ -
+
+
Low Temperature
High Temperature
+ +
High Temperature
exothermicendothermic
Kinetics
1. Temperature (K.E.)
rate of reaction
[reactant][product]
decreaseincrease
2. Concentration3. Orientation
differential rate laws
A + B C
rate = d[A] =
d[B] = dt
d[C] dt
A + B 2 C
rate = - d[A] = dt
- d[B] = dt
d[C] dt
A + B C +
a) +b) - dt
- - +
12
t (min)
0
ave. rate =
ave. rate =
81
= 16.2 min-1
-
16.2 min-1
x
x
x
xx
x
[ ]
0
50
100
time (min)1 2 3 4 5
100 100 01 72 72 282 52 52 483 37 37 634 27 27 73
5 19 19 81
[ ] = t
-[ ] = t
(19 )=5
5- 0- 0
- 100- 0
ave. rate =
ave. rate =
1st minute
5th minute
= 28.0 min-1 1 - 0
- (72 )
t (min)
0 100 100 01 72 72 282 52 52 483 37 37 634 27 27 73
5 19 19 81
x
x
x
xx
x
time (min)1 2 3 4 5
[ ]
0
50
100
ave. rate = - = 16.2 min-1 overall(19- 100) 5 - 0
- 27) = 8.0 min-1 5 - 4
- (19
- 100
slope of line tangent to curve =
at t = 0 initial rate
instantaneous rate
x
x
x
xx
x
time (min)1 2 3 4 5
[ ]
0
50
100
fastest rate
0
k
0.330.330.330.330.330.33
rate [reactant] =
k = rate constant
k [reactant]
= rate [reactant]
t instantaneous (min) rate
1 72 23.82 52 17.23 37 12.24 27 8.95 19 6.3
100 33.0
k = rate [reactant]
k
k
rate =
k, a, b and c
independent of [reactants] dependent on Temperature
k [A]a [B]b ...
determined experimentally
isolation method
[C]c-d[A]) = dt
Exp. 1[A]i
Exp. 2[A]i [B]I initial rate(M) (M) (M s-1)
1.0 x 10-3
2.0 x 10-3
Exp. 3[A]i [B]I initial rate(M) (M) (M s-1)
1.0 x 10-3
(M)[B]i initial rate(M) (M s-1)
1.0 1.0
t (ms)
Con
cent
ratio
n (M
)[A
]
2.0 1.0
1.0 2.0
t (ms)
Con
cent
ratio
n (M
)[A
]
Exp. 1[A]i [B]I initial rate(M) (M) (M s-1) 1.0 1.0
Exp. 2[A]i [B]I initial rate(M) (M) (M s-1) 2.0 1.0
1.0 x 10-3
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
rate 2 =rate 1
2 x 10-3 =1 x 10-3
[2.0]a
[1.0]a
b = 0b = 1b = 2rate =
1st order reaction
1x10-3 (M s-1) =
k = 1 x 10-3 s-1
rate 3 =rate 1
1 x 10-3 =1 x 10-3
[2.0]b
[1.0]b
k [1.0 M]
a = 0a = 1a = 2
rate = k[A]a[B]b
k[A]