Catalytic converter
In an automobile's exhaust system, a catalytic converter provides an environment for a chemical reaction where unburned hydrocarbons completely combust. Hence the combustion process continues but outside the engine combustion chamber where no useful energy is extracted. Toxic car gases such as unburned hydrocarbon (UHC) and carbon monoxide (CO) would not exist if the fuel to energy conversion in the engine were perfect.
A three-way catalytic converter has three simultaneous tasks:
- oxidation of carbon monoxide to carbon dioxide: 2CO + O2 ---> 2CO2
- reduction of nitrogen oxides to nitrogen: NOx ---> O2 + N2
- oxidation of hydrocarbons (unburnt fuel) to carbon dioxide and water: CnHn+2 + O2 ---> CO2 + H2O
These three reactions are most balanced at the stoichiometric point, where there is a balanced amount of oxygen to fuel in the engine. When there is more oxygen than required, then the system is said to be running lean, and the system is in oxidizing conditions. The above two oxidizing reactions (oxidation of CO and hydrocarbons) are favoured. When there is more fuel than oxygen (stoichiometrically), then the engine is running rich. The reduction of NOx is favoured.
Catalytic converters become ineffective in the presence of lead, and the
introduction of catalytic converters in the mid-1970s triggered the
end of leaded petrol.
