Ammonium nitrate, NH4NO3\mathrm{NH_{4}NO_{3}}NH4NO3, is a fertiliser made by reacting ammonia with nitric acid.
NH3(aq)+HNO3(aq)→NH4NO3(aq)\mathrm{NH_{3}(aq)} + \mathrm{HNO_{3}(aq)} \rightarrow \mathrm{NH_{4}NO_{3}(aq)}NH3(aq)+HNO3(aq)→NH4NO3(aq)
Relative atomic masses: H = 1, N = 14, O = 16
Ammonia solution is alkaline. Name the type of reaction between ammonia solution and nitric acid.
Calculate the relative formula mass of ammonium nitrate, NH4NO3\mathrm{NH_{4}NO_{3}}NH4NO3.
Calculate the percentage by mass of nitrogen in ammonium nitrate. Use the equation: percentage by mass of nitrogen=total mass of nitrogen atoms in the formularelative formula mass×100\displaystyle \text{percentage by mass of nitrogen} = \frac{\text{total mass of nitrogen atoms in the formula}}{\text{relative formula mass}} \times 100percentage by mass of nitrogen=relative formula masstotal mass of nitrogen atoms in the formula×100
A farmer needs to add 70 kg of nitrogen to a field. Calculate the mass of ammonium nitrate the farmer should use.
The soil in another field lacks potassium. Suggest why ammonium nitrate alone would not be a suitable fertiliser for this field.
43 exam-style questions on Edexcel GCSE Chemistry 6.3 Dynamic equilibria, covering 6.3.1 The Haber process as a reversible reaction, 6.3.2 Conditions and rate in industrial equilibria, and 6.3.3 Fertilisers and the preparation of ammonium sulfate. Each one has a worked solution and a mark scheme showing where the marks go.