Name two oxides of carbon. Discuss briefly their
preparation, properties and uses.
Please give answer completely!
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Answer:
Carbon dioxide, (CO2), a colourless gas having a faint sharp odour and a sour taste. It is one of the most important greenhouse gases linked to global warming, but it is a minor component of Earth’s atmosphere (about 3 volumes in 10,000), formed in combustion of carbon-containing materials, in fermentation, and in respiration of animals and employed by plants in the photosynthesis of carbohydrates. The presence of the gas in the atmosphere keeps some of the radiant energy received by Earth from being returned to space, thus producing the so-called greenhouse effect. Industrially, it is recovered for numerous diverse applications from flue gases, as a by-product of the preparation of hydrogen for synthesis of ammonia, from limekilns, and from other sources.
photosynthesis
photosynthesis
Diagram of photosynthesis showing how water, light, and carbon dioxide are absorbed by a plant to produce oxygen, sugars, and more carbon dioxide.
Encyclopædia Britannica, Inc.
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Carbon dioxide
QUICK FACTS
KEY PEOPLE
Joseph Black
Jan Baptista van Helmont
Gerard Peter Kuiper
Charles Keeling
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Greenhouse gas
Carbon footprint
Keeling Curve
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Air
Biogenic gas
Dry ice
Carbonation
Carbon dioxide was recognized as a gas different from others early in the 17th century by a Belgian chemist, Jan Baptista van Helmont, who observed it as a product of both fermentation and combustion. It liquefies upon compression to 75 kg per square centimetre (1,071 pounds per square inch) at 31 °C (87.4 °F) or to 16–24 kg per sq cm (230–345 lb per sq in.) at −23 to −12 °C (−10 to 10 °F). By the mid-20th century, most carbon dioxide was sold as the liquid. If the liquid is allowed to expand to atmospheric pressure, it cools and partially freezes to a snowlike solid called dry ice that sublimes (passes directly into vapour without melting) at −78.5 °C (−109.3 °F) at the pressure of the normal atmosphere.
Carbon dioxide is used as a refrigerant, in fire extinguishers, for inflating life rafts and life jackets, blasting coal, foaming rubber and plastics, promoting the growth of plants in greenhouses, immobilizing animals before slaughter, and in carbonated beverages.
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Oxides of phosphorus
Phosphorus forms two common oxides, phosphorus(III) oxide (or tetraphosphorus hexoxide), P4O6, and phosphorus(V) oxide (or tetraphosphorus decaoxide), P4O10. Both oxides have a structure based on the tetrahedral structure of elemental white phosphorus. Phosphorus(III) oxide is a white crystalline solid that smells like garlic and has a poisonous vapour. It oxidizes slowly in air and inflames when heated to 70 °C (158 °F), forming P4O10. It is the acid anhydride of phosphorous acid, H3PO3, that is produced as P4O6 dissolves slowly in cold water. Phosphorus(V) oxide is a white flocculent powder that can be prepared by heating elemental phosphorus in excess oxygen. It is very stable and is a poor oxidizing agent. The P4O10 molecule is the acid anhydride of orthophosphoric acid, H3PO4. When P4O10 is dropped into water, it makes a hissing sound, heat is liberated, and the acid is formed. Because of its great affinity for water, P4O10 is used extensively as a drying agent for gases and for removing water from many compounds
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