kinetics part iv: activation energy jespersen chapter 14 sec 5 & 6
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Kinetics Part IV: Activation Energy Jespersen Chapter 14 Sec 5 & 6. Dr. C. Yau Fall 2014. The Collision Theory. The rate of a reaction is proportional to the number of effective collisions per second among the reactant molecules . - PowerPoint PPT PresentationTRANSCRIPT
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Kinetics Part IV: Activation Energy
Jespersen Chapter 14 Sec 5 & 6
Dr. C. Yau
Fall 2014
The Collision TheoryThe rate of a reaction is proportional to the
number of effective collisions per second among the reactant molecules.
We already know concentration plays an important part in rxn rate:
Conc Freq Collision Rxn Rate
Only EFFECTIVE collisions lead to products.
Only a small fraction of collisions lead to products, based on two other factors:
1) Activation Energy
2) Molecular Orientation 2
Kinetic Energy DistributionEa = Activation energy = minimum energy needed for collision to be effective
Fig 14.11 p.666
Activation Energy is not affected by increase in temperature.
REMEMBER: This is the graph for Kinetic Energy.Don’t confuse with graph for Potential Energy.
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Collision Theory Of ReactionsFor a reaction to occur, three conditions must be met:
1. Reactant particles must collide.
2. Collision energy must be enough to break bonds/initiate.
3. Particles must be oriented so that the new bonds can form.
e.g. NO2Cl + Cl NO2 + Cl2
Eqn Summarizing 3 Factors in Collision Theory
Particulate Level:
Rxn Rate (molecules L-1 s-1) =
N x forientation x fKE
N = # collisions per second per liter of mixture
forientation = fraction of collisions with effective orientation
fKE = fraction of collisions with sufficient kinetic energy for effective collision (area under the curve with KE Ea
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Mathematically, fKE
has been found to be related to Ea and T in this equation:
a
aKE
aKE
-E
RTKE
-E ln =
RTSimplify by finding the anti ln of both sides of the equation...
-Eantiln ln = anti ln
RT
= e
f
f
f
Still remember what fKE stands for?6
Eqn Summarizing 3 Factors in Collision Theory
Macroscopic Level:
Equation has to be in terms of moles instead of molecules.
Conversion factor is
So we divide the previous equation by Avogadro’s number to get
reaction rate in units of mol L-1 s-1
7
23
1 mole of molecules
6.02x10 molecules
-1 -1
23 -1
Rxn Rate (molecules L s )
6.02x10 (molecules mol )mol
= (M/s)L s
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Temperature Effects
Changes in temperature affect the rate constant, k, according to the
Arrhenius equation:p is the steric factor
Z is the frequency of collisions.
Ea is the activation energy
R is the Ideal Gas Constant (8.314 J/(mol K)
T is the temperature (K)
We substitute A (the frequency factor) for (pZ))
E /RTaepZk
E /RTaAek This is an important equation to remember!
Graphical Determination of Ea
E /RTa
-Ea/RT
a
a
a
Ae
ln k = ln A + ln (e )
E ln k = ln A -
RTE 1
ln k = ln A - R T
E 1 ln k = - + ln A
R T
y = m x + b
k
How exactly do we determine Ea?
What do we plot on the x-axis? on the y-axis?
How do we find Ea on the graph?
You are expected to be able to derive this yourself.
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Example 14.12 p.670: Determine Ea in kJ/mol
What do we do with this data?
aE 1ln k = - + ln A
R T 10
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-5
4
-0.70slope =
5.0x10
= -1.4x10 (units?)
aE 1ln k = + ln A
R T
Then what?...
How do we find Ea?
-5
4
-0.70slope =
5.0x10
= - 1.4x10 ( ?)units
Ln
kLn k vs. 1/T
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2
Ea = slope x R
= 1.2x10 kJ/mol
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Determination of Ea from k at 2 temperatures
Ratio form: Can be used when A isn’t known.
a2
2 11
-E 1 1ln -
R T T
k
k
/RTaEAe k
You should be able to derive this equation for yourself. We did a similar derivation earlier this semester for Hvap, VP and T.
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ExampleGiven that k at 25°C is 4.61×10-1 M/s and
that at 50°C it is 4.64×10-1 M/s, what is the activation energy for the reaction?
1a
-1 -1 -1
4 .64 10 M /s -E 1 1ln -
4 .61x10 M /s 8 .314 J m ol K 323K 298K
x
Ea= 188 J/mol = 2 x102 J/mol
a2
2 11
-E 1 1ln -
R T T
k
k
Can you think of a reason why the graphical method would give a more accurate value for Ea?
a2
1 2 1
-1a
-1 -1 -1
-1 -1a-1 -1
a
6 5 5
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-Ek 1 1ln =
k R T T
-E4.64x10 1 1ln =
4.61x10 8.314 J mol K 323 K 298 K
-Eln 1.00 = 0.00309 K - 0.00335 K
8.314 J mol K-E
0.005 = 8.314 J m
-1-1 -1
-1
2a
0
9
0
(0.00026 K )ol K
0.005 8.314 J molE = 188.66... 2x10 J/mol
0.00026
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Working With The Arrhenius Equation
Given the following data, predict k at 75°C using the graphical approach.
k (M/s) T °C
0.000886 25
0.000894 50
0.000908 100
0.000918 150
ANS k=9.01×10-4M/s
Trendline: y = -36.025x – 6.908
k = ? at T = 75oC
/RTaEAe kaE 1
ln k = - + ln AR T
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T deg C k 1/T (in K-1) ln k25 0.000886 0.003355705 -7.02879360750 0.000894 0.003095975 -7.019804783
150 0.000918 0.002364066 -6.993313167
100 0.000908 0.002680965 -7.004266179
0.00230.0024
0.00250.0026
0.00270.0028
0.00290.003
0.00310.0032
0.00330.0034
-7.03
-7.025
-7.02
-7.015
-7.01
-7.005
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-6.995
-6.99
f(x) = − 36.0249500146574 x − 6.90800232199207R² = 0.999727511024572
ln k vs. 1/T
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In the reaction 2N2O5(g) 4 NO2(g) + O2(g) the following temperature and rate constant information is obtained. What is the activation energy of the reaction?A. 102 kJ mol-1
B. -102 kJ mol-1
C. 1004 kJ mol-1
D. -1004 kJ mol-1
E. none of these
T (K) k (s-1)
338328318
4.87(10-3)1.50(10-3)4.98(10-4)
Practice with Example 14.12 p.672, Exer.26,27,28
If we are to determine Ea graphically, what do we graph?Slope = -1.224x104 K and y-intercept = 30.9, what are the units? What is Ea?
aE 1ln k = + ln A
R T
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Potential Energy Diagrams
The product is said to be “thermodynamically favored” over the reactant. LEARN THIS TERMINOLOGY.
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Potential Energy Diagrams• demonstrate the energy needs and
products as a reaction proceeds• tell us whether a reaction is exothermic or
endothermic• tell us if a reaction occurs in one step or
several steps• show us which step is the slowest
Do not confuse PE diagram with KE diagram! Learn the terminology!
So, remember which is the KE diagram?
Potential Energy DiagramWhat would the potential energy diagram
look like for an endothermic reaction?
Make a sketch of a PE diagram for an endothermic reaction.
Where do we look to find the activation energy?
Where do we look to find the heat absorbed during the reaction?
What is thermodynamically favored?21
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Catalysts• speed a reaction, but
are not consumed by the reaction
• may appear in the rate law
• lower the Ea for the reaction
• may be heterogeneous or homogeneous
Ea of uncatalyzed rxn
Ea of catalyzed rxn
PE
Reaction Coordinate
PE Graph
KE Graph: Effect of Catalyst
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Fra
cti
on
of
Mo
lecu
les
Kinetic Energy
Ea without catalyst
Ea with catalyst
000000
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Catalytic Actions• may serve to weaken bonds through
induction• may serve to change polarity through
amphipathic/surfactant effects• may reduce geometric orientation effects• Heterogeneous catalyst: reactant and
product exist in different states.• Homogeneous catalyst: reactants and
catalyst exist in the same physical state
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Example of a heterogeneous catalyst
Note: Fe is never consumed.Catalysts do not have to be in large amounts.
Well-known “The Haber Process.”
Fe3H2 (g) + N2 (g) 2NH3 (g)
Fe