Chemical elements
  Carbon
    Isotopes
    Energy
    Production
    Application
    Physical Properties
    Chemical Properties
      Methane
      Ethylene
      Acetylene
      Coal-Gas
      Carbon Tetrafluoride
      Tetrafluoromethane
      Carbon Tetrachloride
      Tetrachloromethane
      Carbon Tetrabromide
      Tetrabromomethane
      Carbon Tetraiodide
      Tetraiodomethane
      Carbon Oxychloride
      Carbonyl Chloride
      Phosgene
      Carbon Oxybromide
      Carbonyl Bromide
      Carbon Suboxide
      Carbon Monoxide
      Carbon Dioxide
        Preparation
        Physical Properties
        Liquid Carbon Dioxide
        Solid Carbon Dioxide
        Decomposition
        Carbonic Acid
        Carbonates
        Physiological Action
        Detection and Estimation
      Percarbonic Acid
      Carbamic Acid
      Carbamide
      Urea
      Carbon Disulphide
      Carbonyl Sulphide
      Carbon Oxysulphide
      Thiocarbonyl Chloride
      Thiocarbonic Acid
      Thiocarbamic acid
      Thiourea
      Thiocarbamide
      Perthiocarbonates
      Carbon Monosulphide
      Carbon Subsulphide
      Carbon Sulphidoselenide
      Carbon Sulphidotelluride
      Carbon Nitrides
      Cyanogen
      Dicyanogen
      Hydrocyanic Acid
      Prussic Acid
      Cyanogen Chloride
      Chlorocyanogen
      Cyanogen Bromide
      Bromocyanogen
      Cyanogen Iodide
      Iodocyanogen
      Polymerised Cyanogen Halides
      Cyanamide
      Cyanic Acid
      Cyanuric Acid
      Cyamelide
      Fulminic Acid
      Thiocyanic Acid
      Sulphocyanic Acid
      Isoperthiocyanic Acid
      Cyanogen Sulphide
      Thiocyanic Anhydride
    Diamonds
    Graphite
    Amorphous Carbon
    Coal

Preparation of Carbon Dioxide






Carbon dioxide is generally prepared in the laboratory by the action of somewhat diluted hydrochloric acid on marble:

CaCO3 + 2HCl = CaCl2 + H2O + CO2.

The appearance of the gas is preceded by the liberation of carbonic acid, H2CO3, which, being unstable, decomposes almost completely into water and carbon dioxide. The evolved gas, which contains traces of hydrochloric acid, may be purified by passing it through sodium hydrogen carbonate solution, or it may be collected over water instead of by the more usual method of upward displacement of air.

Dilute sulphuric acid cannot be employed in place of hydrochloric acid because the marble quickly becomes encrusted with almost insoluble calcium sulphate which stops the action; if, however, concentrated sulphuric acid, containing only a very little water, is used, the evolution of gas continues because an acid sulphate of calcium is formed which remains in solution.

If sodium carbonate is employed as the source of carbon dioxide the evolution of the gas is vigorous, whether dilute hydrochloric or sulphuric acid is employed.

Sodium hydrogen carbonate is a convenient source of carbon dioxide, which it evolves when gently heated in the solid state or in solution:

2NaHCO3 = Na2CO3 + H2O + CO2.

Normal sodium carbonate is not decomposed by heat until a very high temperature is reached; calcium carbonate, being the salt of a less powerful base, begins to yield its carbon dioxide at about 550° C.; magnesium carbonate, in the form of the mineral magnesite, gives off carbon dioxide when gently ignited, and is therefore sometimes employed as a source of the gas.

Carbon dioxide may also be prepared by the combustion of charcoal or coke, and purified from the atmospheric nitrogen with which it will be mixed, by causing it to combine with an alkali carbonate, whence it is again set free by the action of acids.


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