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TOPIC: CARBON AND ITS COMPOUND
CONTENT:
PERIOD 1: CARBON(IV) OXIDE: PREPARATION AND USES
FORMATION / PREPARATION OF CARBON(IV) OXIDE (CO2)
In excess air, there is complete combustion; carbon (iv) oxide is produced but in the limited supply of air carbon normally reacts with oxygen to produce carbon(ii) oxide. The equation of reaction is given below for the two reactions.
C(s)+ O2(g) → CO2(g) + heat (sufficient supply of air)
2C(s) + O2(g) → 2CO(g) + heat (limited supply of air)
Other methods of preparation of CO2 are:
CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
CaCO3(s) → CaO(s) + CO2
2NaHCO3(s) → Na2CO3(s) + H2O +CO2(g)
Na2CO3(s) + 2HCl(aq) → 2 NaCl(aq) + H2O(l) + CO2(g)
KHCO3(s) + HNO3(aq) → KNO3(aq) + H2O(l) + 2CO2(g)
(iv) The fermentation of glucose by an enzyme (zymase)
C6H12O6(ag) → 2C2H5OH(aq) + 2CO2(g)
LABORATORY PREPARATION OF CO2 GAS
The equation for the reaction is given as shown below
CaCO3(s) + HCl(aq) → CaCl2(aq) + H2O + CO2(g)
Pure and dry CO2 is obtained by passing the gas through a solution of potassium hydrogentrioxocarbonate (IV) [KHCO3] to remove the acid impurities, hydrogen chloride and then, through conc. (or fused CaCl2 to dry the gas. It is then collected by downwards delivery, being denser than air as in the diagram above.
PHYSICAL PROPERTIES OF CO2(g)
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