Carbon Monoxide, CO
Carbon Monoxide, CO
Direct oxidation of C in limited supply of oxygen or air
yields carbon monoxide.
2C (s) + O2 (g) + (Heat) → 2CO (g)
On small scale pure CO is prepared by dehydration of formic
acid with concentrated H2SO4 at 373K.
HCOOH
(Heat with Conc. H2SO4) → H2O + CO
On commercial scale it is prepared by the passage of steam
over hot coke. The mixture of CO and H2 thus produced is known as
Water Gas or Synthesis gas.
C (s) + H2O
(g) (Heat 473-1273 K) → CO (g)
+ H2 (g)
Water Gas
When air is used instead of steam, a mixture of CO and N2
is produced, which is called Producer Gas.
2C (s) + O2
(g) +
4N2 (g) (Heat
1273 K) → 2CO (g) + 4N2 (g)
Producer Gas
Water gas and producer gas are very important industrial
fuels. Carbon monoxide in water gas or producer gas can undergo further
combustion forming carbon dioxide with the liberation of heat.
Carbon monoxide is a colorless, odorless and almost water
insoluble gas. It is a powerful reducing agent and reduces almost all metal
oxides other than those of the alkali and alkaline earth metals, aluminium and
a few transition metals. T his property of CO is used in the extraction of many
metals from their oxides ores.
Fe2O3 (s) +
3CO (g) (Heat) → 2Fe (s)
+ 3CO2 (g)
ZnO (s) + CO (g) (Heat) → Sn (s) + CO2 (g)
In carbon monoxide molecule, there are one sigma and two 𝝅 bonds between carbon and oxygen, :C=O: . Because of the presence of a
long pair on carbon, CO molecule acts as a donor and reacts with certain metals
when heated to form metal carbonyls. The highly poisonous nature of CO arises
because of its ability to form a complex with heamoglobin, which
is about 300 times more stable than the oxygen-haemoglobin complex. This
prevents haemoglobin in the red blood corpuscles from carrying oxygen round the
body and ultimately resulting in death.
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