Oxides of Carbon: Methods of preparation

Carbon is a chemical element, one of the most important building blocks of our world and the foundation of life as we know it. Without carbon, we would not exist. It’s the basis of all life on our planet, and without it, there would be no humans, plants, animals, or even other forms of life as we know it. One of the most important uses of carbon is to make things, such as medicines, plastics, computers, cars, and the thousands of other products we use every day. Without carbon, our economy would not be able to function, and it’s the fourth most abundant element in the universe.

Carbon’s two important gaseous compounds with oxygen, carbon monoxide (CO) and carbon dioxide (CO2), are released into the atmosphere through natural processes, such as animal respiration and volcanoes, and through human activities, such as the burning of fossil fuels. 

Oxides of Carbon

Oxides of carbon are solid forms of carbon. 

Oxides of carbon are inorganic compounds that contain one or more carbon atoms covalently bonded to one or more oxygen atoms. Oxides of carbon are also known as carbonates. The most common carbonate is limestone, which is made of the mineral calcite. Calcite is a salt that crystallises from water. The chemical formula for calcite is CaCO3. Oxides of carbon are also important components of catalysts used in chemical reactions. 

The most common oxide of carbon is known as graphite, which is used to line pencils and as a coating on steel. Other common oxides of carbon include diamond, which is used as a gemstone, to make glass, and diamond-like carbon, which is used in touch screens, DVDs, and paper. It is a building block of life and is the basis of many important compounds, such as proteins and DNA. Many other compounds are also known as carbonates, such as calcium carbonate (limestone), which is a major constituent of soils and is vital for the survival of many plants. 

Properties of Oxides of Carbon

1. They are crystalline in shape and can be very hard.

2. They are also relatively stable and do not easily react with other substances. This makes them great for use in the industry!

3. All oxides of carbon are colourless, odourless, tasteless solids.

4. They are typically solid at room temperature and pressure, but can also exist in liquid form. 

5. They have a metallic lustre.

6. They are very reactant and will ignite easily. They burn with a white, blue, or purple flame.  

Preparation of some common oxides of Carbon

CO2 (Carbon Dioxide):

The most common oxide is carbon dioxide, which is a gas at room temperature and pressure. It is a colourless gas that is easy to measure and has a mild odour. It is an important ingredient in fizzy drinks and as a building material for concrete, and as a feedstock for the chemical industry. It is the main greenhouse gas that is released from the burning of fossil fuels. It is also the gas that is responsible for the greenhouse effect. CO2 is produced by all living things, including animals, plants, and bacteria. 

Preparation of CO2:

The most common oxide of carbon is calcium carbonate or limestone. Calcium carbonate is used in the construction industry, as a filler in cement and the making of toothpaste and egg whites. The oxide of carbon calcium carbonate is also used as a reactant in the preparation of CO2. 

The chemical equation for the preparation of CO2 using calcium carbonate is 

CaCO3 + H2O → Ca2(HCO3)2 + CO2. 

CO (Carbon Monoxide):

Carbon monoxide is a gas at room temperature. It is released when you burn coal or gasoline. CO is a colourless and odourless gas that is lethal if you breathe it in large amounts. CO is a deadly poison because it blocks the action of the hormone carbon dioxide, which is necessary for cells to function. It is released from motor vehicle exhaust and from fires, such as those in coal mines, that burn organic material. CO is a gas that can be inhaled and can cause deadly poisoning. CO is used to make charcoal and blackened foods. 

CO is the main ingredient in car exhaust and is also a by-product of incomplete combustion in engines, furnaces, and fires. CO is also used in the manufacture of paper and is an active ingredient in some pesticides.CO is the main ingredient in carbon dioxide pipes and carbon monoxide incense. 

Preparation of CO:

Chemical reactions used in the preparation of CO include burning wood, coal, charcoal, and other organic materials; burning fossil fuels; burning trash and garbage; and the combustion of energy-releasing materials, such as sugar, fat, and cellulose. All of these processes release oxygen and generate CO and other gases. CO is a by-product of many of these processes, but it is also a raw material used to make other oxides of carbon and other chemicals, such as plastics and pharmaceuticals.

Conclusion

The carbon in oxides of carbon is in the form of a C-O-C structure. The general formula of an oxide of carbon is CxOy. Oxides of carbon are classified as follows: carbonates, oxides, hydroxides, and halides. The most common oxides of carbon on Earth are carbonates, oxides, and carbon dioxide, which are all inorganic compounds.