What are the functions of potassium hydroxide and tetraoxosulphate 6 acid and heated iron filing in the preparation of nitrogen from air.
Describe the commercial preparation of nitrogen.
Both hydrogen sulphide and sulphur 4 oxide decolourise acidified potassium tetraoxomanganate 7 solution.
A.write the chemical equation for these reaction.
B.state the main difference in the action of these gases on acidified KMNO4 solution
A. To understand the functions of potassium hydroxide (KOH), tetraoxosulphate 6 acid (H2SO4), and heated iron filings in the preparation of nitrogen from air, we need to break down the process:
1. KOH: In this reaction, potassium hydroxide acts as a drying agent. It removes any water vapor that may be present in the air. Since nitrogen gas is the desired product, it is crucial to remove any moisture because water can interfere with the reaction.
2. H2SO4: Tetraoxosulphate 6 acid, also known as sulfuric acid, plays a dual role in this process. It acts as a catalyst to speed up the reaction between atmospheric oxygen and iron filings. It also absorbs any water produced during the reaction to prevent it from interfering with the formation of nitrogen gas.
3. Heated Iron Filings: When iron filings are heated in the presence of air and H2SO4, they react with oxygen to form iron(II) oxide (FeO). This reaction is known as the reduction of iron oxide. The iron filings provide a source of oxygen for the reaction, and as a result, nitrogen gas (N2) is produced.
So, to summarize, potassium hydroxide removes moisture, tetraoxosulphate 6 acid acts as a catalyst and absorbs water, and heated iron filings provide oxygen for the reaction, leading to the production of nitrogen gas.
B. Commercial preparation of nitrogen:
The most common method for commercial nitrogen preparation is through fractional distillation of liquefied air. Here are the steps involved:
1. Compression: The air is compressed using a compressor to increase its pressure. This helps in liquefying the air at low temperatures.
2. Cooling: The compressed air is then cooled to very low temperatures using a series of heat exchangers. As the temperature decreases, the components of air liquefy at different temperatures, allowing for separation.
3. Fractional Distillation: The cooled and liquefied air is fed into a fractional distillation column. This column has multiple trays, each at different temperatures. As the air rises through the column, it gradually warms up, causing the components to vaporize at their respective boiling points.
4. Separation: Nitrogen, having a lower boiling point (-196°C), vaporizes first and is collected as a gas at the top of the column. Oxygen and other trace gases are collected at different trays based on their boiling points.
5. Purification: The collected nitrogen gas may go through further purification processes to remove any impurities, such as trace amounts of oxygen or other gases, to obtain high-purity nitrogen.
Overall, through compression, cooling, fractional distillation, and purification, nitrogen gas is commercially prepared from air.
Now let's move on to the next question:
Both hydrogen sulfide (H2S) and sulfur 4 oxide (SO2) decolourize acidified potassium tetraoxomanganate 7 solution (KMnO4).
A. Chemical equations for these reactions:
1. Hydrogen sulfide (H2S):
H2S + KMnO4 + H2SO4 → MnSO4 + K2SO4 + S + 2H2O
2. Sulfur 4 oxide (SO2):
SO2 + 2KMnO4 + 2H2SO4 → K2SO4 + 2MnSO4 + 2H2O
B. The main difference in the action of these gases on acidified KMnO4 solution:
Both hydrogen sulfide and sulfur 4 oxide are reducing agents that react with KMnO4. However, the main difference lies in the products formed during the reaction.
When hydrogen sulfide reacts with acidified KMnO4, sulfur (S) is formed as a solid precipitate. On the other hand, when sulfur 4 oxide reacts with acidified KMnO4, the products are potassium sulfate (K2SO4), manganese sulfate (MnSO4), and water (H2O).