Carbon monoxide (carbon (II) oxide).

It can prepared in the laboratory by dehydrating oxalic acid using concentrated sulphuric acid.
H2C2O4 → CO + CO2 +H2O

The mixture of carbon monoxide and carbon dioxide are passed through a concentrated solution of potassium hydroxide or sodium hydroxide which reacts with carbon dioxide from the mixture leaving carbon monoxide. The carbon monoxide can be collected over water.

Dehydration of methanoic acid by concentrated sulphuric can produce CO.
HCOOH → CO + H2O

PROPERTIES OF CARBON MONOXIDE

(a) Physical properties of Carbon monoxide

  1. It is colorless and tasteless.
  2. It is very poisonous gas.
  3. It is odourless.
  4. It is less dense than air.
  5. It is insoluble in water.

(b)Chemical properties

  • Combustion
    It burns in air with a blue flame to produce carbon dioxide.
    CO(g) + O2 → 2CO2
  • Reducing agent.
    It is a powerful reducing agent; it removes oxygen from metal oxides.
    CuO(s)(black) + CO(g) → Cu(s)(red-brown) + CO2(g)
    PbO(yellow) + CO → Pb(s)(grey) + CO2
    ZnO(white) + CO → Zn (grey)+ CO2
    Fe2O3 + 3CO → 2Fe +3CO2

    Uses of carbon monoxide

    1. It is used as a fuel.
    2. It is used in the extraction of metals due to its reducing properties.
    Carbon monoxide Carbon dioxide
    It is a good reducing agent. It is not reducing agent.
    It is less dense than air. It is denser than air.
    It does not react with alkalis. It reacts with alkalis
    It is insoluble in water It is soluble in water.
    It does not affect the litmus paper Turns blue litmus paper red

    Note

    Carbon monoxide combines with the haemoglobin in red blood cells to form a stable compound called carboxyhaemoglobin so preventing the carriage of oxygen by the haemoglobin to other body parts. This can cause the death of an individual due to starvation of oxygen.
    Explore Form Four topics