Methods of Preparation of Carbon Dioxide

The scientific formula of carbon dioxide is CO2. Carbon dioxide is widely used in industries, factories, and laboratories for performing various experiments. It is a type of chemical compound that originated in the form of colourless acidic gas. Its density is approximately 53% higher than the other gases present in the atmosphere. 0.04% of the total gas in the atmosphere contains carbon dioxide. Along with the atmosphere, it is extracted manually for industrial and laboratory uses. It is extracted from nature and can be prepared in laboratories. Also, one can prepare carbon dioxide at home, but in a smaller quantity only. 

About Carbon dioxide 

Carbon dioxide is the colourless acidic gas, having a molar mass of 44.009 g·mol−1. The structure of carbon dioxide is Trigonal. The heat capacity of carbon dioxide is 37.135 J/K·mol. Its solubility at the temperature of 25 °C is 1.45 g/L. 

Carbon dioxide is exhaled by human beings in the process of respiration. Then, further, it is absorbed by the plants and utilised by them for synthesising the food through the process of photosynthesis. Along with this, it has various methods of preparation and uses of Carbon Dioxide. 

Methods of preparation 

There are different methods of preparation of carbon dioxide. Let’s understand them separately. 

Natural Method 

Carbon dioxide is found in caves and mines. These caves and mines are found as mineral-like magnesite, dolomite, and limestone. It is extracted from these minerals and stored. 

Along with this, naturally, the carbon dioxide is also prepared by the process of fermentation. In this process, organic sugar-containing food like grapes is stored for many years for preparing alcohol, wines, and beers. Carbon dioxide is also produced and collected for future use during this process. 

Carbon dioxide is also released in the process of decay. 

These are the several natural methods of preparation of carbon dioxide. 

Industrial Method 

Industrially, carbon dioxide is produced by reacting the carbonates with acids. So, for industrial preparation methods, the calcium carbonate reacts with hydrochloric acid. 

When we mix the calcium carbonate with the dilute hydrochloric acid, the calcium chloride forms; along with this, the carbon dioxide and hydrogen gas are also released. Due to the lightweight nature of hydrogen, it goes into the atmosphere fastly, and carbon dioxide gets collected in the funnel. The equation of this reaction is written below. 

CaCO3 + dil 2HCl → CaCl2 + CO2↑ + H2↑

Calcium carbonate + dilute hydrochloric acid → calcium chloride + carbon dioxide + water 

At Home 

Carbon dioxide can easily be prepared at home by baking soda and Vinegar. Firstly, take one teaspoon of baking soda in the glass tube and put ¼ cup vinegar in it. After mixing, you will observe the bubbles in the glass tube, and these bubbles are of carbon dioxide. You can collect carbon dioxide in the balloon or funnel. 

With Methane 

Carbon dioxide can also be prepared using methane by the process of combustion. In the combustion of methane or carbon, the carbon dioxide gets released. When we react to carbon with oxygen, carbon dioxide releases along with this. The released carbon dioxide gets collected for future use. The equation of these reactions is written below. 

C + O2 → CO2 + Heat

Carbon + oxygen → carbon dioxide + Heat 

CH4 + 2O2 → CO2 + 2H2O

Methane + oxygen → carbon dioxide + water 

Decomposition of Calcium Carbonate 

During the decomposition of calcium carbonate, the carbon dioxide gas is released. The equation is written as:

CaCO3 → CaO + CO2 

Calcium carbonate → calcium oxide + carbon dioxide 

Decomposition of magnesium carbonate 

During the decomposition of magnesium carbonate, the carbon dioxide gas is released. The equation is written as:

MgCo3 → MgO + CO2

Magnesium carbonate → magnesium oxide + carbon dioxide 

With Metallic Carbonates 

When metallic carbonates like sodium carbonate react with sulphuric acid, the carbon dioxide gas is released. The equation is written as, 

Na2CO3  + H2SO4 → Na2SO4 + H20 + CO2

Sodium carbonate + sulphuric acid → sodium sulphate + water + carbon dioxide 

With Metallic Bicarbonates 

When metallic bicarbonates like sodium bicarbonate react with sulphuric acid, the carbon dioxide gas is released. The equation is written as:

Na2HCO3  + H2SO4 → Na2SO4 + H20 + CO2 

Sodium bicarbonate + sulphuric acid → sodium sulphate + water + carbon dioxide 

Physical Properties of Carbon dioxide 

Let’s learn some physical properties of carbon dioxide:

• Carbon dioxide is a colourless acidic gas. 
• Carbon dioxide is smelled less (Odourless). 
• It is 53% heavier than the air. Due to this, it finds more near the earth’s surface. 
• The solid carbon dioxide is called dry ice. 
• Carbon dioxide can become solid at room temperature but with the 70 atmospheric pressure. 

Chemical Properties of Carbon dioxide 

Let’s learn some chemical properties of carbon dioxide:

• Water reacts with carbon dioxide to prepare carbonic acid. 

CO2 + H2O → H2CO3

• It reacts with sodium hydroxide to give sodium carbonate as a result. 
• It reacts with calcium hydroxide to give water calcium carbonate as a result. 
• It forms metallic oxides by reacting with metals.

Conclusion 

There are several methods of preparation of carbon dioxide. It can be prepared in laboratories, in industries, at home, and by using different chemical substances like methane, carbonated, bicarbonates, and so forth. Along with this, carbon dioxide is used extensively in preparing cold drinks, soda, and other packet foods. It is also used in fire extinguishers because it stops the supply of oxygen and stops burning fire. It is also used in laboratories for various chemicals like baking soda, urea, washing powder, etc. It is also used in welding metals like iron copper to prevent corrosion.