SS1 Chemistry Lesson Note on Carbon (II) Oxide: Preparations; Properties and Uses

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CARBON(II) OXIDE

LABORATORY PREPARATION OF CO [in the fume cupboard]

Three methods can be used to prepare CO in the lab and they are as follows;

1. Ethanedioc acid crystals, [H₂C₂O₄.2H₂O]

The equation for the reaction is given as shown below;

H₂C₂O₄.2H₂O(s) ^decomposed    →      3H₂O(l) + CO(g) + CO₂(g)

Note: That conc. H₂SO₄ is a drying agent, it is there to remove the elements of water while KOH removes CO_2(g)

CO_2(g) + 2KOH_(aq)          →         K₂CO_3(aq) + H₂O_(l)

2(a) Sodium Methanoate crystals

2HCOONa_(s) + H₂SO_4(aq)          →         Na₂SO_4(aq)  +  2H₂O + 2CO_(g)

1. Methannoic acid

 

HCOOH_(l)  →       CO(g)

Show that H₂SO₄ removes water, a dehydrating agent

3. Reduction of CO_2(g) to CO as shown below

CO_2(g) + C(s)      →    2CO(g)

PHYSICAL PROPERTIES OF CO

1. It is colourless, odourless and tasteless gas.
2. It is slightly lighter than air.
3. It is only slightly soluble in water, but insoluble in alkalis.
4. It is soluble in ammoniacal solution of copper(I) chloride.
5. It is a poisonous gas, hence, prepared in fume cupboard.
6. It is a neutral gas therefore it does not have any action on the litmus paper.

  CHEMICAL PROPERTIES AND USES OF CO

1. It is used as fuel because it supports combustion.
2. It is a useful reducing agent because it is readily reduce to CO₂(g) e.g.

• CO_(g) + H₂O      →     CO_2(g) + H_2(g)
• CO_(g) + CuO_(s)      →               Cu(s) + CO₂(g)
• 3CO(g) + Fe2O_3(s)    →     2Fe_(s) + 3 CO_2(g)
• CO_(g) + PbO_(s)    →      Pb_(s)   +     CO₂(g)

Note: The product of combustion or oxidation of CO is CO_2; confirmed by its ability to turn lime water milky.

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