The depletion or erosion of the Ozone layer and its aftermath is a
major cause of worry for modern man. Ozone O3 is called the Blanket of
the Earth because of its screening effect where it absorbs 99% of
harmful UV rays from the Sun. Otherwise, the UV ray will alter living
Organisms (Plants and Animals) such that Plants may lose some of their
vital features like the ability for Cassava plant to produce Cassava
Tuber, Man will be faced with high incident of Skin Cancer and Eye
Cataract, and large numbers of Animals and Live-stocks such as cattle
will be faced by massive blindness.
The Modality by which Ozone in the Ozone Layer absorbs UV ray involves a simple chemical reaction where one molecule of Ozone absorbs UV light and dissociate into molecular Oxygen and atomic Oxygen as evident in the equation Below.
O3(g) → O2(g) + O(g)
Formation of Ozone
Though Ozone gas can be formed from unintentional processes such as electric sparks in vehicle Engines or common electrical appliances like the photocopying machine, deliberate formation can also be made from passing streams of Oxygen through an electric discharge system or by adopting the reaction of Nitrogen Oxides with Hydrocarbon in the presence of sunlight.
But the most unique process of formation of Ozone is the formation in the Earth's Stratosphere ie 20 to 50 Km above the Earth's surface. Here, UV rays will first split molecular Oxygen to Atomic Oxygen.
O2(g) → O(g) + O(g)
Then, atomic Oxygen will combine with molecular Oxygen in the presence of electric charge generated by lightening to form the Ozone Molecule.
O2(g) + O(g) → O3(g) + M(g)
Where M is a second product that help to carry away the excess energy.
Properties and Uses of Ozone
Ozone gas is pale-blue in colour with characteristic pungent smell like dilute Chlorine. It exist as blue liquid when cooled to -112°C, slightly soluble in water, and a poisonous gas at a concentration above 100ppm even though it is harmless at a lower concentration.
The chemical properties of Ozone are similar to that of Oxygen except that Ozone is more reactive than Oxygen. This makes it a more powerful oxidising agent than Oxygen so that it is used as a potent bleaching agent. It is used for ventilation in places where there is limited Oxygen, as a disinfectant in sewage and water purification, and plays an important role in air conditioning. Here is an example of the strong oxidising effect of Ozone:
SO2(g) + O3(g) → SO3(g) + O2(g)
Ozonizer
Ozone is a highly unstable triatomic Allotrope of Oxygen, O2 that can easily be dissociated by heat. Hence, care must be taken to avoid possible dissociation to molecular and atomic Oxygen.
2O3(g) → 3O2(g)
This is the reason why it is prepared from Oxygen in a special device called the Ozonizer. Ozonizing Oxygen involves passing dry Oxygen through one end of the Ozonizer into the inner chamber where the Oxygen is ionised by the electric discharge system made possible by a connection of two Induction Coils to Tin foil and concentric glass tubes, and out as Ozone through the outlet at the other end.
The Modality by which Ozone in the Ozone Layer absorbs UV ray involves a simple chemical reaction where one molecule of Ozone absorbs UV light and dissociate into molecular Oxygen and atomic Oxygen as evident in the equation Below.
O3(g) → O2(g) + O(g)
Formation of Ozone
Though Ozone gas can be formed from unintentional processes such as electric sparks in vehicle Engines or common electrical appliances like the photocopying machine, deliberate formation can also be made from passing streams of Oxygen through an electric discharge system or by adopting the reaction of Nitrogen Oxides with Hydrocarbon in the presence of sunlight.
But the most unique process of formation of Ozone is the formation in the Earth's Stratosphere ie 20 to 50 Km above the Earth's surface. Here, UV rays will first split molecular Oxygen to Atomic Oxygen.
O2(g) → O(g) + O(g)
Then, atomic Oxygen will combine with molecular Oxygen in the presence of electric charge generated by lightening to form the Ozone Molecule.
O2(g) + O(g) → O3(g) + M(g)
Where M is a second product that help to carry away the excess energy.
Properties and Uses of Ozone
Ozone gas is pale-blue in colour with characteristic pungent smell like dilute Chlorine. It exist as blue liquid when cooled to -112°C, slightly soluble in water, and a poisonous gas at a concentration above 100ppm even though it is harmless at a lower concentration.
The chemical properties of Ozone are similar to that of Oxygen except that Ozone is more reactive than Oxygen. This makes it a more powerful oxidising agent than Oxygen so that it is used as a potent bleaching agent. It is used for ventilation in places where there is limited Oxygen, as a disinfectant in sewage and water purification, and plays an important role in air conditioning. Here is an example of the strong oxidising effect of Ozone:
SO2(g) + O3(g) → SO3(g) + O2(g)
Ozonizer
Ozone is a highly unstable triatomic Allotrope of Oxygen, O2 that can easily be dissociated by heat. Hence, care must be taken to avoid possible dissociation to molecular and atomic Oxygen.
2O3(g) → 3O2(g)
This is the reason why it is prepared from Oxygen in a special device called the Ozonizer. Ozonizing Oxygen involves passing dry Oxygen through one end of the Ozonizer into the inner chamber where the Oxygen is ionised by the electric discharge system made possible by a connection of two Induction Coils to Tin foil and concentric glass tubes, and out as Ozone through the outlet at the other end.
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