Question

Match List-I with list-II

Column 1	Column 2
Haber process	${\mathrm{HNO}}_3$ synthesis
Ostwald process	Aluminum extraction
Contact process	${\mathrm{NH}}_3$ synthesis
Hall-Heroult process	${\mathrm{H}}_2{\mathrm{SO}}_4$ synthesis

Answer 1

(A) Haber process- (III) ${\mathrm{NH}}_3$

1. The Haber-Bosch process, sometimes known as the Haber process, is one of the most effective and successful industrial processes used to produce ammonia.
2. By interacting with hydrogen (${\mathrm{H}}_2$) and a metal catalyst, atmospheric nitrogen (${\mathrm{N}}_2$) is transformed into ammonia (${\mathrm{NH}}_3$)
3. .$\underset{\mathrm{Nitrogen}\mathrm{gas}}{2{\mathrm{N}}_2\left(\mathrm{g}\right)}+\underset{\mathrm{Hydrogen}\mathrm{gas}}{{\mathrm{H}}_2\left(\mathrm{g}\right)}\to \underset{\mathrm{Ammonia}\mathrm{gas}}{2{\mathrm{NH}}_3\left(\mathrm{g}\right)}$
4. Through pipes, hydrogen, and nitrogen that have been extracted from natural gas and the air respectively are pumped.
5. the pressure of the mixture of gases is increased upto $200$atmospheres
6. The pressurized gases are heated to ${450}^{°}\mathrm{C}$ and then passed through an iron catalyst in a tank.
7. The reaction mixture is cooled in order to allow the ammonia to liquefy and remove it.

(B) Ostwald process- (I) ${\mathrm{HNO}}_3$ synthesis

1. The Ostwald process is one of the chemical processes often used for producing nitric acid.
2. The process includes two steps: Catalytic oxidation reaction and absorption of ${\mathrm{NO}}_2$
3. Ammonia is subjected to oxidation, which produces nitric oxide ($\mathrm{NO}$). The reaction is exothermic and reversible. $\underset{\mathrm{Ammonia}}{4{\mathrm{NH}}_3\left(\mathrm{g}\right)}+\underset{\mathrm{Oxygen}}{5{\mathrm{O}}_2\left(\mathrm{g}\right)}\rightleftharpoons \underset{\mathrm{Nitric}\mathrm{oxide}}{4\mathrm{NO}\left(\mathrm{g}\right)}+\underset{\mathrm{water}}{6{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)}$
4. Ammonia oxidation results in the production of extremely hot nitric oxide gas. Nitric oxide is cooled to ${1500}^{°}\mathrm{C}$ in a heat exchanger before being passed through.
5. Nitric oxide is moved to another oxidizing tower after cooling, where nitrogen dioxide (${\mathrm{NO}}_2$) is oxidized at a temperature of roughly$500°\mathrm{C}$.$\underset{\mathrm{Nitric}\mathrm{oxide}}{2\mathrm{NO}\left(\mathrm{g}\right)}+\underset{\mathrm{oxygen}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\rightleftharpoons \underset{\mathrm{nitrogen}\mathrm{dioxide}}{2{\mathrm{NO}}_2\left(\mathrm{g}\right)}$
6. The nitrogen dioxide from the secondary oxidation chamber is fed to an exclusive water absorption tower. The water is absorbed by ${\mathrm{NO}}_2$ gas as it passes through a tower. Through this procedure, nitric acid is then produced. $\underset{\mathrm{Nitrogen}\mathrm{dioxide}}{3{\mathrm{NO}}_2\left(\mathrm{g}\right)}+\underset{\mathrm{water}}{{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)}\to \underset{\mathrm{Nitric}\mathrm{acid}}{{\mathrm{HNO}}_3\left(\mathrm{l}\right)}+\underset{\mathrm{Nitric}\mathrm{oxide}}{\mathrm{NO}\left(\mathrm{g}\right)}$

(C) Contact process- (IV) ${\mathrm{H}}_2{\mathrm{SO}}_4$ synthesis

1. One of the most common or widely used processes for producing sulfuric acid is the contact process.
2. There are four steps in the contact process for making sulfuric acid. These processes include sulfur extraction, sulfur dioxide preparation, sulfur dioxide conversion to sulfur trioxide, and sulfur trioxide conversion to sulfuric acid.
3. From natural gas and oil, sulfur is extracted.
4. The stationary atomizer is pumped with molten sulfur. Sulfur atoms are created as a result of this. The hot furnace is treated with atomized sulfur. A sulfuric acid dehydrator is used to pre-heat and dry the air and is also applied to the hot furnace.
5. At one end of the heated furnace, air and molten sulfur that have been atomized are retained. Sulfur dioxide is created at the other end of a process.$\underset{\mathrm{Sulfur}}{\mathrm{S}}+\underset{\mathrm{oxygen}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\to \underset{\mathrm{Sulfur}\mathrm{dioxide}}{{\mathrm{SO}}_2\left(\mathrm{g}\right)}$
6. In a lead chamber, sulfur dioxide and oxygen are mixed at a $1:1$ ratio. With one to two atm, the temperature is set to $400$ to ${450}^{°}\mathrm{C}$ degrees Celsius. Vanadium pentoxide catalyzes the reaction, which results in sulfur trioxide. $\underset{\mathrm{Sulfur}\mathrm{dioxide}}{2{\mathrm{SO}}_2\left(\mathrm{g}\right)}+\underset{\mathrm{oxygen}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\rightleftharpoons \underset{\mathrm{sulfur}\mathrm{trioxide}}{{\mathrm{SO}}_3\left(\mathrm{g}\right)}$
7. Now, sulfuric acid is used to dilute sulfur trioxide. This results in oleum. $\underset{\mathrm{sulfur}\mathrm{trioxide}}{{\mathrm{SO}}_3\left(\mathrm{g}\right)}+\underset{\mathrm{sulfuric}\mathrm{acid}}{{\mathrm{H}}_2{\mathrm{SO}}_4\left(\mathrm{l}\right)}\to \underset{\mathrm{oleum}}{{\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_7}$
8. To make concentrated sulfuric acid, oleum can be further diluted with water. $\underset{\mathrm{oleum}}{{\mathrm{H}}_2{\mathrm{S}}_2{\mathrm{O}}_7}+\underset{\mathrm{water}}{{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)}\to \underset{\mathrm{Sulfuric}\mathrm{acid}}{2{\mathrm{H}}_2{\mathrm{SO}}_4\left(\mathrm{l}\right)}$

(D) Hall-Heroult process- (II) Aluminum extraction

1. The complex electrolysis process known as the Hall-Heroult process is used to generate aluminum.
2. In the Hall-Heroults method, ${\mathrm{CaF}}_2$ or ${\mathrm{Na}}_3{\mathrm{AlF}}_6$is combined with pure ${\mathrm{Al}}_2{\mathrm{O}}_3$. As a result, the mixture's melting point is lowered and its capacity to conduct electricity is raised. It uses a steel vessel lined with carbon and graphite rods.
3. Graphite serves as an anode, and the carbon lining serves as a cathode. At the anode of the electrolytic cell, which has carbon electrodes, oxygen is created when electricity is applied.
4. As a result of this oxygen's reaction with the anode's carbon, carbon monoxide, and carbon dioxide are created.$$\begin{gathered} \underset{\mathrm{carbon}}{\mathrm{C}\left(\mathrm{s}\right)}+\underset{\mathrm{oxygen}\mathrm{ion}}{{{\mathrm{O}}_2}^{-}}\to \underset{\mathrm{carbon}\mathrm{monoxide}}{\mathrm{CO}\left(\mathrm{g}\right)}+2{\mathrm{e}}^{-} \\ \underset{\mathrm{carbon}}{\mathrm{C}\left(\mathrm{s}\right)}+\underset{\mathrm{oxygen}\mathrm{ion}}{2{{\mathrm{O}}_2}^{-}}\to \underset{\mathrm{carbon}\mathrm{dioxide}}{{\mathrm{CO}}_2\left(\mathrm{g}\right)}+4{\mathrm{e}}^{-} \end{gathered}$$
5. Aluminum ions are produced at the adverse cathode from the aluminum oxide, and because they are heavier than the cryolite solution, they sink to the bottom. ${\mathrm{Al}}^{3+}+3{\mathrm{e}}^{-}\to \mathrm{Al}$
6. The aluminum then took on a liquid shape after sinking to the bottom. At the positive anode on the opposite side, oxygen from aluminum oxide develops and reacts with graphite carbon.
7. Overall reaction is $\underset{\mathrm{Aluminum}\mathrm{oxide}}{2{\mathrm{Al}}_2{\mathrm{O}}_3}+\underset{\mathrm{carbon}}{3\mathrm{C}}\to \underset{\mathrm{Aluminum}}{4\mathrm{Al}\left(\mathrm{s}\right)}+\underset{\mathrm{carbon}\mathrm{dioxide}}{3{\mathrm{CO}}_2\left(\mathrm{g}\right)}$

Final answer:

List-I	List-II
A. Haber process	${\mathrm{NH}}_3$ synthesis
B. Ostwald process	${\mathrm{HNO}}_3$ synthesis
C. Contact process	${\mathrm{H}}_2{\mathrm{SO}}_4$ synthesis
D. Hall-heroult process	Aluminum extraction