Question

Under what conditions can hydrogen be made to combine with oxygen? Name the product in the following case and write the equation for it.

Answer 1

Ammonia is a nitrogen-hydrogen chemical with the formula $N{H_3}$. Ammonia is a colourless gas with a strong odour. It is a stable binary hydride and the simplest pnictogen hydride. It's a frequent nitrogenous waste, especially among aquatic creatures, and it helps terrestrial creatures meet their nutritional demands by acting as a precursor to food and fertilisers.

Complete answer: The Haber process is an excellent example of how industrial chemists utilise their understanding of the variables that govern chemical equilibria to determine the ideal conditions for producing a high yield of products at an acceptable rate.
“Atmospheric nitrogen ($N_2$) is transformed to ammonia (NH3) by reacting it with hydrogen (H2)” in the Haber process. A metal catalyst is utilised in this process, which is carried out at high temperatures and pressures.
The process's raw ingredients are as follows.
The nitrogen is supplied via air.
Natural gas and water provide hydrogen as well as the energy required to heat the reactants.
The catalyst, iron, is a non-renewable resource.
We blend nitrogen gas from the air with hydrogen atoms derived from natural gas in a 1:3 volume ratio. The gases are circulated over four catalyst beds, with each pass cooling the gases. This is done in order to keep the equilibrium steady. In each pass, varying amounts of conversion occur, and unreacted gases are recycled. Normally, an iron catalyst is utilised in the process, and the entire method is carried out at a temperature of $400-{450^o}C$ and a pressure of 150–200 atm. Shift conversion, carbon dioxide removal, steam reforming, and methanation are all part of the process.
${{\text{N}}_2} + 3{{\text{H}}_2} \to 2{\text{N}}{{\text{H}}_3}\quad \Delta {H^\circ } = - 91.8\;{\text{kJ}}/{\text{mol}}$

Note:
Ammonia production on a large scale has been difficult prior to the creation of the Haber process, with early approaches such as the Birkeland–Eyde and Frank–Caro processes all being inefficient. Despite the fact that the Haber process is now mostly used to make fertiliser, it provided Germany with a source of ammonia for the creation of explosives during World War I, compensating for the Allied Powers' trade ban on Chilean saltpetre.