• Catalysts can be divided into two types:
  • Homogeneous?catalysts
  • Heterogeneous?catalysts

   

• Homogeneous?means that the catalyst is in the?same phase?as the reactants
  • For example, the reactants and the catalysts are all in solution

   

• Heterogeneous?means that the catalyst is in a?different phase?to the reactants
  • For example, the reactants are gases, but the catalyst used is a solid

• Ammonia production via the?Haber Process?is a classic example of the use of a?heterogeneous?catalyst

N2?(g) + 3H2?(g)???2NH3?(g)

• The Haber Process occurs in five stages

1. 1. Hydrogen and nitrogen are obtained from natural gas and air respectively and pumped into the compressor
   2. The gases are compressed to about 200 atmospheres
   3. The pressurised gases, at around 450?oC, are pumped into a tank containing beds of solid?iron?which is a heterogeneous?catalyst, where some of the hydrogen and nitrogen react to form ammonia
   4. Unreacted hydrogen, nitrogen and the ammonia product pass into a cooling tank where the ammonia is liquefied and removed
   5. The unreacted hydrogen and nitrogen are recycled back into the system and start over again

The production of ammonia by the Haber Process

Conditions

Temperature: 450oC

• A?higher?temperature favours the reverse reaction as it is endothermic (takes in heat) so a higher yield of?reactants?would be made
• Lower?temperature favours the forward reaction as it is exothermic (releases heat) so a higher yield of?products?will be made
  • However, at a lower temperature the rate of reaction is very?slow
• So 450oC is a compromise temperature between having a?lower yield?of products but being made more quickly

Pressure: Approximately 20 MPa

• Lower?pressure favours the reverse reaction as the system will try to increase the pressure by creating more molecules (4 molecules of gaseous reactants) so a higher yield of?reactants?will be made
• Higher?pressure favours the forward reaction as it will try to decrease the pressure by creating less molecules (2 molecules of gaseous products) so a higher yield of?products?will be made
• However, high pressures can be dangerous and very expensive equipment is needed
• So, 20 MPa is a?compromise?pressure between a lower yield of products being made?safely?and?economically

Catalyst

• A catalyst of iron is used to speed up the reaction
• Without a catalyst, the required temperature and pressure for the Haber Process would be much higher, more dangerous, more expensive and less environmentally friendly

Benefits of catalysts

• Catalysts speed up the rate of reaction, meaning the use of a catalyst may mean lower temperatures and pressures can be used
  • This can save energy costs as there is reduced energy demand for providing high temperatures and less electrical pumping costs for producing the high pressures usually required
  • This can mean fewer CO2?emissions from burning fossil fuels
• Catalysts can also enable different reactions to be used, with better atom economy and with reduced waste, or fewer undesired products or less use of hazardous solvents and reactants
• Catalysts are often enzymes, generating very specific products, and operating effectively close to room temperature and pressure