1. §9.5 Temperature-dependence of reaction rate -- Arrhenius equation
Extensive reading: Levine, pp Section 17.8

2. Teaching design:
BOPPPS: a best way for micro-teaching
Bridging:
Objective
Pre-assessment
Participating
Post-assessment
Summary

3. Problem: why do we use k other than r?
From the middle 19 century, people began to study the effect of temperature on the reaction rate. Many empirical relations have been founded.
5.1 Types of rate-temperature curves T k
Type I:
k increases exponentially with T.
This kind of curve can be observed in most of the reactions.
Problem: why do we use k other than r?

4. T k
Type II
This kind of k~T relation was observed in thermal explosions. At ignition temperature, the rate constant makes a sharp increase. T k
Type III
usually encountered in the catalytic reaction that has an optimum temperature.

5. The only example is 2NO + O2 = 2NO2k
Type IV:
observed in oxidation of carbon and gaseous oxidation of hydrocarbons. T k
Type V:
The only example is 2NO + O2 = 2NO2

6. 5.2 Empirical rules (1) vant’ Hoff’s Law
It was found that for homogeneous reaction, an important generalization is that reaction rate double or triple for every 10 degree increase in temperature.
in which A and B are experimental / empirical constants.

7. (2) Arrhenius equation C12H22O11 + H2O  C6H12O6 + C6H12O6
In 1889, Arrhenius made detailed theoretical consideration on the hydrolysis of sucrose.
C12H22O11 + H2O  C6H12O6 + C6H12O6
in which sucrose molecules were surrounded by water, if all sucrose molecules could react directly with water, the reaction should completed instantly. However, this is not the case.
Arrhenius postulated that only a small part of sucrose molecules with higher energy (activated molecules) can react with water and, therefore, the reaction can only proceed at a low rate.
By taking enough energy, the common sucrose molecules can change into activated molecules. The energy needed for this conversion was called activation energy. [A very important concept!]

8. Defined the activation energy (Ea)
Arrhenius extended the ideas of vant’ Hoff and suggested a similar empirical equation.
Arrhenius equation
Dimension analysis
Is the simplification reasonable?
Defined the activation energy (Ea)
The first definition of activation energy: experimental activation energy

9. If Ea is independent on temperature, integration of the equation
yields
A is the pre-exponential factor which has the same unit as the rate constant.
In those five r ~ T relation types, only Type I obeys Arrhenius equation. Type I is usually named as Arrhenius type.

10. 5. 3 Experimental measurement activation energy
Graphic method
Calculation method
Graphic method:
to plot lnk against 1/T [Arrhenius plot], for the reaction of Arrhenius type, a straight line may be obtained, the slope of which equals –Ea/R

11. ClCOOCH3 + H2O  CO2 + CH3OH + H+ + Cl
T / K
273.72
278.18
283.18
288.14
104 k / s-1
0.4209
0.7016
1.229
2.087
198.18
308.16
318.29
5.642
14.05
32.65
R =
Ea = kJmol-1, A =1.32  109
A is very large

12. (2) Calculation method:
Constant
T / K
273.72
278.18
283.18
288.14
104 k / s-1
0.4209
0.7016
1.229
2.087
198.18
308.16
318.29
5.642
14.05
32.65

13. 5. 4 Tolman’s definition of Ea
The minimum energy that the molecules must absorb before the reaction can take place is known as the activation energy.
According to Tolman, the activation energy of elementary reaction is the difference between the average energy of the activated molecules and the average energy of total molecules:
Boltzmann distribution

14. 5.5 Ea and energy change of reaction
the difference in thermodynamic energy
reactant, product, activated state, reaction path. 22
When Ea,->Ea,+, U < 0, the reaction is exothermic.

15. principle of micro-reversibility
When Ea,-< Ea,+, U > 0, the reaction is a endothermic one.
For a strong endothermic reaction, the activation energy for backward reaction is very small.
What about Ea, +?
principle of micro-reversibility
Potential curve

16. 5.6 Activation energy of a overall reaction?
Only the activation energy of elementary reaction has definite physical meaning.
The activation energies of some overall reactions can be taken as a combination of the activation energy of elementary reactions composing of the overall reaction. The activation energy of some overall reactions, usually named as apparent activation energy, may be meaningless physically.

17. 5. 7 Theoretical evaluation of Ea:
The activation energy can be related to the energy change of the reaction. The energy change can be calculated using dissociation energy of chemical bond.
To do this, some empirical rules may be used:
Dissociation reaction:
Cl-Cl  2 Cl
Ea will not be less than and need not be larger than the dissociation energy of the bond, i.e., Ea = DCl-Cl
Dissociation energy of the bond is different from energy of bond.

18. 2) Combination reaction of radicals
2CH3·  CH3CH3
Ea = 0
3) Radicals react with molecules:
A + BC  AB + C
If the reaction is a exothermal one, Ea  5% DB-C;
4) Molecules react with molecules:
AB + CD  AC + BD
If the reaction is exothermal, Ea = 30% (DAB + DCD)

19. 5. 8 Ea on reaction rate
Half-life of first-order reaction with different activation energy
Ea / kJmol-1 40 60 80
100
120
t1/2
210-5 s
0.066 s
5.6 h
11.6 d
68.7 y
Ea ranges between 40 ~ 400 kJ mol-1.
For first-order reaction,
when Ea increases by 4 kJ mol-1, k decreases by 80%. The effect of Ea on reaction rate is significant.
Reaction with Ea less than 80 kJ mol-1 belongs to fast reactions. To study their kinetics, special methods have to be used.
For reaction with Ea larger than 100 kJ mol-1 , it is too slow to study.

20. 5. 9 Temperature on reaction rate
T2 > T1
Ea,1 T1 T2
Ea,2
What about the fraction of activated molecule increases?
Can your find another way to increase the fraction of activated molecules?

21. 5. 10 Temperature-dependence of Ea
The Arrhenius plots for some reactions are curved, which suggests that the activation energy of these reactions is a function of temperature. At this situation, the temperature dependence of k can be usually expressed as:
This equation suggests that, Ea depends on temperature.
Problem:
Discussion the relationship between this equation and vant’ Hoff empirical equation

22. The value of m, usually be 0, 1, 2, 1/2, etc. , is not very large
The value of m, usually be 0, 1, 2, 1/2, etc., is not very large. Therefore, mRT is not very large with comparison to Ea.
In a relatively small temperature range, Ea seems independent on temperature.
However, for some reaction such as:
CCl3COOH  CHCl3 + CO2, m = -10.7
CH3Br + H2O  CH3OH + H+ + Br, m = -34.3
The effect of temperature on the activation energy of these reactions is too large to ignore.

23. To measure activation energy of the reaction over a large span of temperature would result in exceptional difficulties.
When T , A = k. Is this correct?
How can we measure the activation energy of a reaction?

24. Unimolecular reaction Termolecular reaction
5.11 A on reaction rate
Type of reaction
Unimolecular reaction
Bimolecular reaction
Termolecular reaction A
1013 s
1011
mol-1dm3s-1
109
mol-2dm6s-1
5.12 Application of Arrhenius equation
1) make explanation for some experimental results;
2) calculate the reaction rate at different temperature;
3) determine the optimum temperature for reaction.

25. T. T. Ching, S. C. Kwong and S. C. Kim, JACS, 2012, 134: 11388-11391