1. Temperature dependence of reaction rates
Typically rates of reactions double for every 10oC rise in temperature,
Arrhenius equation
Ea: activation energy
A: frequency factor

2. An Arrhenius plot of ln k against 1/T is used to determine Ea and A
The higher the Ea the stronger the temperature dependence of the rate constant

3. However, every time two reactants collide they may not react
Collision Theory
Collisions between two (or more) atoms/molecules required for a reaction.
However, every time two reactants collide they may not react
As temperature increases:
atoms/molecules collide more frequently
kinetic energy of atoms/molecules increases
Collision theory: reaction occurs only if the reactants collide with a kinetic energy of at least the activation energy, and they do so in the correct orientation.
As we saw in an earlier demo, rates of reactions increase with temperature. In fact if the temperature of the reaction mixture is increased from 25 to 35oC, the rate almost doubles.
Why does the rate increase with temp?
To a first approximation reactions occur because of collisions between reactants.
Hence if temp increases rate at which reactants collide increases and hence one might expect that the rate increases.
As temp increases speed of molecules increase and hence more frequent collisions.
Energy (kinetic energy) also increases

4. Kinetic energy is important
It was realized that a the particle must collide with a minimum relative kinetic energy in order for the collision to result in a reaction.
“soft” collisions may not result in reaction, electron clouds have to overlap for bond formation.
And hence a minimum energy is required for reactive collisions
Etrans > Ea
This minimum energy is called the ACTIVATION ENERGY

6. Orientation is importantCl N O
Arrenhius realized the energy dependence of the rate of the reactions. However it was realized later that the orientation of the colliding partners is also important. Not all collisions between molecules with energy above the barrier resulted in products. And that’s because reactants have to be oriented. This is called the STERIC EFFECT
2 AB -> A2 + B2
2 NOCl  2 NO + Cl2

7. Animation 1
Animation 2
Animation 3

8. The factor e-Ea/RT: fraction of molecules that have at least the minimum energy required for reaction.
For an Ea = 40 kJ/mol
Temperature (K) e-Ea/RT
x 10-8
x 10-6
x 10-4
A: reflects orientation effect or steric effect

9. Measuring k as a function of T Ea to be determined

10. Reaction coordinate diagram
Activated complex or transition state - highest energy along reaction coordinate
Reactants must collide with sufficient energy to reach this point and collide in a preferred orientation to form the activated complex

11. DE = (Ea)forward - (Ea)reverse

12. Higher temperatures favor products for an endothermic reaction and reactants for an exothermic reaction
Endothermic reaction: Ea(forward) > Ea(reverse)
Exothermic reaction: Ea(forward) < Ea(reverse)

13. CH3OH(aq) + H+(aq)  CH3OH2+(aq)
CH3OH2+(aq) + Br- (aq)  CH3Br + H2O(aq)

14. Catalysis
Catalyst: a compound which speeds up the rate of a reaction, but does not itself undergo a chemical change.
Simple mechanism
A + catalyst  intermediates
intermediates  B + catalyst
Overall: A  B
Concentration of catalyst is included in k; hence k varies with concentration of catalyst

15. Presence of a catalyst provides an alternate path with a lower Ea
2H2O2(aq)  2H2O(aq) + O2(g)
In the absence of a catalyst, Ea = 76 kJ/mol
In the presence of a catalyst (I-); Ea = 57 kJ/mol;
rate constant increases by a factor of 2000

16. Catalyzed by I2

17. Pt
C2H4(g) + H2(g)  C2H6 (g)
Example of heterogenous catalysis

18. A catalyst does not effect the thermodynamics of the reaction
DG is not affected by catalyst; neither is K
Equilibrium concentrations are the same with and without catalyst; just the rate at which equilibrium is reached increases in the presence of a catalyst
K = k1/k-1; catalyst speeds up both the forward and reverse reaction

19. Enzymes
Practically all living reactions are catalyzed by enzymes; each enzyme specific for a reaction.
Enzymes typically speed up rates by times rate of uncatalyzed reactions
Ea for acid hydrolysis of sucrose: 107 kJ/mol
Ea for catalyzed acid hydrolysis of sucrose: 36 kJ/mol
Rate increase of 1012 at body temperature
E + S  ES
ES  P + E

20. “Poisoning” a catalyst
Arsenic poisoning: Ingestion of As(V) as AsO43- results in reduction to As(III) which binds to enzymes, inhibiting their action
Nerve gases - block enzyme-controlled reactions that allow nerve impulses to travel through the nerves.

21. High temperature in the engine causes oxidation of N2 to NO and NO2
Catalytic Converters
Incomplete combustion of gasoline produces CO, hydrocarbon fragments (CmHn)
High temperature in the engine causes oxidation of N2 to NO and NO2
Conversion of these pollutants to less harmful compounds is speeded up in the presence of catalysts.
2 NO(g) N2(g) + O2(g)
catalyst
CO, CmHn, O CO2, H2O
catalyst
Catalyst: pellets of Pt, Pd, Rh
animation