1. Catalysis

2. Starter: What do you know about catalysts?
Substance that changes the speed/rate of a chemical reaction, but is not used up in the reaction.
Speed up reactions by providing an alternative route with a lower activation energy
(Do not alter ∆G, ∆H or ∆S for a reaction, only the activation energy).
Speed the rate at which an equilibrium is reached by speeding up the forward and reverse reaction
They do not alter the position of the equilibrium (or the value of Kc –the equilibrium constant).
Catalysts that slow down reactions are called inhibitors (or negative catalysts).

3. Introduction
Catalyst = substance that speeds up reaction without being used up.
They provide an alternative mechanism with lower activation energy.
For an equilibrium, they speed up both reactions equally and so do not effect equilibrium position.
Heterogeneous catalyst is in different phase to the reactants.
Homogeneous catalyst is in the same phase as the reactants.

4. Introduction

5. Common Features of Catalysts
They can be very specific and only catalyse a certain reaction or class of similar reactions
Size and surface area: Often only needed in very small amounts (e.g., 2 g of Pt can catalyse the decomposition of 1000m3 of H2O2).
Solid catalysts more effective when they are a powder or as a thin layer – their surface area to volume ratio is very large.

6. Heterogeneous Catalysts
Heterogeneous catalyst is in different phase to the reactants.
Usually a solid catalyst and gaseous reactants.
Most industrial catalysts are like this
(e.g. Haber Process – Fe; Contact Process – V2O5).

7. Heterogeneous Catalysts
1) Reactants adsorbed onto surface (onto active sites).
weakens bonds
brings molecules closer
more favourable orientation
2) Reaction takes place.
The reaction happens at the surface of the catalyst
The places where the reactions happen are called “active sites”
e.g., in the Haber Process, nitrogen and hydrogen react together in the presence of an iron catalyst to produce ammonia
The N2 and H2 molecules are adsorbed on to the surface of the iron
They react together then ammonia desorbs from the surface
3) Products are desorbed (leave the surface).

8. Heterogeneous Catalysts

9. Heterogeneous Catalysts
Strength of adsorption:
Too strong (e.g. W)
Reactants cannot move round surface.
Products cannot desorb.
Too weak (e.g. Ag)
Reactants not adsorbed.
Ideal (e.g. Ni, Pt)

10. What is the contact process?

11. Importance of Variable Oxidation States
Variable oxidation states very important in heterogeneous catalysis
E.g., use of V2O5 in the Contact Process
In the second stage of H2SO4 manufacture, sulfur(IV) oxide is oxidised to sulfur(VI) oxide (2-step mechanism):
1. The vanadium(V) oxide catalyst oxidises sulfur(IV) oxide to sulfur(VI) oxide.
SO2(g) + V2O5(s) → SO3(g) + V2O4(s)
2. The vanadium(IV) oxide reacts with oxygen and the Vanadium(V) oxide is regenerated
V2O4(s) + 1/2O2(g) → V2O5(s)
Overall:
SO2(g) + 1/2O2(g) ↔ SO3(g)
Step 1: Ox state of V decreases from +5 to +4
V2O5 catalyst

12. How does a catalytic convertor work?

13. Heterogeneous Catalysts
Nature of catalyst
Large surface area.
Spread thinly over ceramic honeycomb.
To make catalysts more efficient ...
They can be expensive so more efficient catalysts mean that costs will be minimised.
Increase their SA the larger the SA, the better the efficiency
Spread the catalyst onto an inert support medium (or impregnate it into one). Increases the surface-to –mass ratio (a little goes a long way). This is usually for more expensive catalysts - e.g., catalytic converter in car finely divided Rh and Pt on a ceramic material.
(Possibly mention PdENCat – worked on during MChem ... Polymer encapsulated Pd catalyst)

14. Heterogeneous Catalysts
1) Reactants adsorbed onto surface (onto active sites).
weakens bonds
brings molecules closer
more favourable orientation
2) Reaction takes place.
The reaction happens at the surface of the catalyst
The places where the reactions happen are called “active sites”
e.g., in the Haber Process, nitrogen and hydrogen react together in the presence of an iron catalyst to produce ammonia
The N2 and H2 molecules are adsorbed on to the surface of the iron
They react together then ammonia desorbs from the surface
3) Products are desorbed (leave the surface).

15. Homogeneous Catalysts
Homogeneous catalyst is in the same phase as the reactants.
Most examples involve reactions in solution with catalyst in solution.
Some gas phase examples.

16. Homogeneous Catalysts
Catalyst reacts with a reactant to form intermediate.
2) Intermediate reacts to form product faster than original reactant (and regenerates catalyst).
e.g. acid catalyst
X + Y  products
X + H+ → HX+
2) HX+ + Y → products + H+

17. A reaction of the S2O82- ion
2 I- + S2O82- → I SO42-
Why would this be considered a slow reaction?

18. A reaction of the S2O82- ion
Fe2+
2 I- + S2O82- → I SO42-

19. Homogeneous Catalysts
2 Fe2+ + S2O82- → 2 Fe SO42-
2) 2 Fe I- → 2 Fe2+ + I2
Fe2+ is regenerated, so the two steps can repeat continuously.

20. Can also happen the other way around…
2 Fe I- → 2 Fe2+ + I2
2 Fe2+ + S2O82- → 2 Fe SO42-
Fe3+ is regenerated, so the two steps can repeat continuously.

21. Redox Titrations
May want to measure the conc of an oxidising or reducing agent
Do a redox titration
Similar to acid-base titration (find out how much acid is needed to react with a certain volume of base [or vice versa])
C2O42- react with MnO4- acidified with excess dilute sulfuric acid (H+)

22. Homogeneous Catalysts: Autocatalysis
The reaction is catalysed by one of the products (Mn2+) – this is called autocatalysis.
Such a reaction starts slowly – uncatalysed rate
As conc of the products (also the catalyst) builds up, the reaction speeds up to catalysed rate.
Then behaves as normal reaction ... Slows down as reactants are used up
e.g. transition metal catalyst: works by metal varying oxidation state
Oxidation of ethanedioic acid by manganate(VII) ions
Discuss the reaction and draw the curve on p232 of textbook
Mn2+
2MnO4- (aq)+16 H+ (aq) + 5 C2O42- (aq) → 2Mn2+ (aq) + 8 H2O (aq) +10 CO2 (aq)

23. Oxidation of ethanedioate ions
2MnO C2O H+  2Mn2+ + 5CO2 + 8H2O

24. EXAM QUESTIONS