Consider a reaction N2+3H2 goes to produce 2NH3
This reaction is known as the Haber-Bosch process and is used to produce ammonia industrially. It involves the combination of nitrogen gas (N2) and hydrogen gas (H2) to produce ammonia gas (NH3).
The balanced chemical equation for the reaction is:
N2 + 3H2 -> 2NH3
In this reaction, one mole of nitrogen gas reacts with three moles of hydrogen gas to produce two moles of ammonia gas.
The reaction is exothermic, meaning it releases energy in the form of heat. It is typically carried out at high pressures of around 200 atmospheres and temperatures of around 400-500 degrees Celsius. Catalysts, such as iron or a mixture of iron and other metal oxides, are used to increase the reaction rate.
The Haber-Bosch process is of great industrial importance because ammonia is a primary component in the production of fertilizers, explosives, and other nitrogen-containing compounds.
The given reaction is: N2 + 3H2 → 2NH3
To understand the reaction, we can break it down step by step:
Step 1: Balancing the equation:
Let's first balance the equation by ensuring that the number of each element is the same on both sides.
N2 + 3H2 → 2NH3
The nitrogen (N) and hydrogen (H) are initially balanced on both sides, with 2 nitrogen atoms and 6 hydrogen atoms on each side.
Now, let's balance the hydrogen atoms by placing a coefficient of 2 in front of H2 on the left side:
N2 + 2H2 → 2NH3
Now we have 4 hydrogen atoms on both sides.
Step 2: Determining the Reactants and Products:
In the given reaction, N2 and H2 are the reactants, while NH3 is the product.
Step 3: Stoichiometry:
The stoichiometry of the reaction indicates the ratio in which the reactants combine and the products are formed.
According to the balanced equation, 1 mole of N2 reacts with 2 moles of H2 to produce 2 moles of NH3.
Step 4: Understanding the Reaction:
The reaction represents the combination of nitrogen gas (N2) and hydrogen gas (H2) to form ammonia (NH3). This reaction is known as the Haber process, which is an important method for producing ammonia.
Step 5: Reaction Conditions:
The reaction is typically carried out under high pressure (around 200 atm) and at a temperature of around 400-500°C. Iron catalysts are often used to increase the reaction rate.
Overall, this reaction is an important industrial process used to produce ammonia, which is a vital component in the production of fertilizers, various chemicals, and even explosives.