The equation below represents a reaction that takes place in an industrial process.
[tex]4NH_3 + 5O_2 \rightarrow 6H_2O + 4NO[/tex]
a. Name the catalyst used.
b. What are the other conditions for the reaction?
c. Why are the products cooled before being oxidized?
Answer (2)
The catalyst used for the reaction is typically platinum or rhodium. Conditions for the reaction include high temperatures and sometimes pressures. Cooling the products before further oxidation helps prevent unwanted side reactions and equipment damage.
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The reaction given in the equation 4 N H 3 + 5 O 2 → 6 H 2 O + 4 NO is commonly known as the Ostwald process, which is used in the industrial production of nitric acid from ammonia.
Here’s how it breaks down:
Catalyst Used: The catalyst commonly used for this reaction is platinum (Pt), often with small amounts of rhodium. The catalyst helps to increase the rate of reaction without being consumed in the process.
Other Conditions for the Reaction:
Temperature: The reaction is typically carried out at high temperatures, around 800-900°C.
Pressure: Pressure conditions are usually around 4-10 atmospheres.
Excess Oxygen: An excess of oxygen is required to drive the reaction towards the formation of nitric oxide ( NO ).
Why the Products are Cooled Before Being Oxidized: Once the reaction has formed nitric oxide ( NO ), the products are cooled before further oxidation. Cooling is important because it allows the NO to be more efficiently absorbed in subsequent steps to form nitrogen dioxide ( N O 2 ), which then reacts with water to produce nitric acid ( H N O 3 ). Cooling also reduces the chances of undesirable side reactions that may occur at high temperatures. Additionally, cooling helps in the conversion of gaseous products into liquids or solids which are easier to handle and separate in industrial settings.
This Ostwald process is a crucial step in producing nitric acid, which is an important chemical used in fertilizers, explosives, and many other industrial applications.
