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• Ammonia (NH3) is a colourless, odourless gas that is made up of nitrogen and hydrogen.
• It's the simplest stable compound of these elements, and it's used to make a variety of commercially relevant nitrogen compounds.
• In chemical analysis, nitrogen is frequently utilised during sample preparation. It is used to concentrate liquid samples and reduce their volume.
• Hydrogen can be utilised to generate electricity, power, and heat in fuel cells. The most prevalent applications for hydrogen today are petroleum refining and fertiliser production, with transportation and utilities as new areas.

Calculate the amount of ammonia gas created when 3.0g of hydrogen and nitrogen are combined.

The reaction stoichiometry can be used to calculate the amount of reactants consumed or the amount of products created.

Given:

Mass of hydrogen =3.0g

Mass of nitrogen =3.0g

The response of \({N_2}\) with \({H_2}\) to take shape\(N{H_3}\) can be expressed as follows:

\({N_2} + 3{H_2} \to 2N{H_3}\)

Based on the stoichiometry of the reaction:

1 mole of the \({N_2}\) mixes with three moles \({H_2}\) to make two moles of \(N{H_3}\)

Moles of \({H_2}\)reacted \( = \frac{{3.0\;g}}{{1.0\;g.mo{l^{ - 1}}}} = 3.0\) moles

Moles of \({N_2}\)reacted \( = \frac{{3.0\;g}}{{28.0\;g.mo{l^1}}} = 0.1071\)moles

The reactant that is being limited is \({N_2}\)

Based on the stoichiometry of the reaction

1 mole of \({N_2}\) makes two moles of \(N{H_3}\)

Moles of \(N{H_3}\) created from the \({N_2}\) right now is: \( = \frac{{0.1071 moles {N_2} \times 2 mole N{H_3}}}{{1 mole{ _2}}} = 0.2142\) moles \(N{H_3}\)

Mass of \(N{H_3}\)produced \( = 0.2142moles \times 17\;{g^{mol}}mo{l^{ - 1}} = 3.641\;g\)

Around a pound of ammonia is produced \(3.64\;g\).