Topic 15.3

Question 1

Heterogenous catalyst

Answer 1

Different state to the reactants.
-Catalyst is usually a solid and takes place on the surface.
-Eg. Haber process (iron catalyst)
-Eg. Contact process (vanadium oxide catalyst)

Question 2

Homogenous catalyst

Answer 2

Same phase as the reactants.
-Most reactions take place In solution (all species are either liquids or dissolved in solution).
-Reactions proceed via an intermediate species formed from a reactant and the catalyst, which reacts further and regenerates the catalyst.
S2O8^2- + 2I- —> I2 + 2SO4^2-
S2O8^2- + 2Fe^2+ —> 2Fe^3+ + 2SO4^2-
2Fe^3+ + 2I^- —> 2Fe^3+ + I2
(common questions)

Question 3

Solid catalyst

Answer 3

Adsorption on surface
-Active site–> proximity of molecules Lowe, weaken covalent bonds
-Desrobed from surface

Question 4

Poisoning of catalyst

Answer 4

-Impurities block active sites.
-Can ruin catalyst.
-Catalyst has no effect on rate of reaction (lowers its efficiency).
–> Increased chemical costs, cleaning, reduces production
(Haber process-> sulfur impurities)

Question 5

Autocatalysis

Answer 5

-1 product acts as a catalyst
-More product -> higher rate of reaction
-eg. redox MnO4^- C2O4^- (MnO4^- acts as a catalyst)
2MnO4^- + 16H+ + 5C2O4^2- —> 2Mn^2+ + 8H2O + 10CO2
Intermediate: 4Mn^2+ + MnO4^- + 8H+ –> 5Mn^3+ + 4H2O
2Mn^3+ + C2O4^2- –> 2CO2 + 2Mn^2+
—> Heat to start- rate of reaction will continue to increase

Question 6

How does a homogenous catalyst work?

Answer 6

-At least one reaction is adsorbed onto the surface (ie. forms bonds to the atoms in the solid surface).
-The places on the surface where molecules are adsorbed are called active sites.
-In an effective catalyst, the molecule can move about the surface, bonding to different active sites.
-The adsorption of reactants onto the surface can result in increased reaction in a number of ways:
a) adsorption onto the surface effectively concentrates the reactants (ie. brings them closer to the gas phase- increasing likelihood of collisions).
b) it may weaken some of the bonds in the molecule, making reaction easier.
c) it may position the molecule in a favourable orientation for reaction.

Question 7

If adsorption is too weak:

Answer 7

Not many molecules will be adsorbed so the catalyst will have very little effect.

Question 8

If adsorption is too strong:

Answer 8

Molecules will not be able to move around the active sites and so be less likely to meet another reactant and so be less likely to react.
(Also many products will tend to remain adsorbed on the surface).

Question 9

Ideal catalyst

Answer 9

Nickel and platinum- ideal adsorption strength.
(Ag has too weak adsorption, W too strong adsorption).

Question 10

The nature of the catalyst

Answer 10

-The larger the surface area, the less quantity of catalyst that is needed.
-Maximising surface area of catalyst, has important cost savings.
-Surface area is maximises by using a thin coating of the catalyst on some type of support medium (eg, honeycomb structure).

Question 11

Acid catalyst in esterification

Answer 11

Question 12

Transition metal catalyst (double -ve)

Answer 12