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USES OF OXYGEN

  1. Oxygen is put in cylinders for use where natural supply is not sufficiently enough.

This is mainly in:

(i) Mountain climbing/Mountaineering-at high altitudes, the concentration of air/oxygen is low.

Mountain climbers must therefore carry their own supply of oxygen for breathing.

(ii) Deep sea diving-Deep sea divers carry their own supply of Oxygen.

(iii) Saving life in hospitals for patients with breathing problems and during anaethesia.

 

  1. A mixture of oxygen and some other gases produces a flame that is very hot.

(i) Oxy-acetyline/ethyne flame is produced when Ethyne/acetylene gas is burnt in pure oxygen.

The flame has a temperature of about 3000oC.It is used for welding/cuttingmetals.

(ii)Oxy-hydrogen flame is produced when Hydrogen is burn in pure oxygen. The flame has a temperature of about 2000oC.It is used also for welding/cuttingmetals.

 

  1. Oxy-hydrogen mixture is used as rocket fuel
  2. A mixture of charcoal, petrol and liquid Oxygen is an explosive.
See also  SCHEME OF WORK FOR CHEMISTRY SS 1

(d) Chemical properties of Oxygen /combustion.

Oxygen is a very reactive non-metal. Many elements react with oxygen through burning to form a group of compounds called Oxides. Burning/combustion is the reaction of Oxygen with an element/substances. Reaction in which a substance is added oxygen is called Oxidation reaction. Burning/combustion is an example of an oxidation reaction.

 

Most non-metals burn in Oxygen/air to form an Oxide which in solution / dissolved in water is acidic in nature. They turn blue litmus red. e.g. Carbon(IV)oxide/CO,Nitrogen(IV)oxide/NO,Sulphur(IV)oxide/SO2. Some non-metals burns in Oxygen/air to form an Oxide which in solution / dissolved in water is neutral in nature. They don’t turn blue or red litmus. e.g. Carbon(II)oxide/CO, Water/HO.

 

All metals burns in Oxygen/air to form an Oxide which in solution/dissolved in water is basic/alkaline in nature. They turn red litmus blue. e.g. Magnesium oxide/MgO, Sodium Oxide/ NaO. Copper(II)oxide/CuO Elements/substances burn faster in pure Oxygen than in air. Air contains the inactive part of air that slows the rate of burning of substances/elements.

See also  BALANCING OF REDOX REACTIONS

 

See also

OXYGEN

THE ATMOSPHERE

PROPERTIES OF ACIDS

INTRODUCTION TO ACIDS, BASES AND INDICATORS

 

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