Ammonium nitrate, NH4NO3\text{NH}_4\text{NO}_3NH4NO3, is a very common nitrogen-based fertiliser.
Explain why fertilisers are important in the agricultural production of crops.
Ammonium nitrate is produced by reacting ammonia with nitric acid:
NH3+HNO3→NH4NO3 \text{NH}_3 + \text{HNO}_3 \rightarrow \text{NH}_4\text{NO}_3 NH3+HNO3→NH4NO3Calculate the mass of ammonium nitrate that could be made from 5.1 tonnes5.1\text{ tonnes}5.1 tonnes of ammonia.
Relative atomic masses (ArA_rAr): H=1.0\text{H} = 1.0H=1.0, N=14.0\text{N} = 14.0N=14.0, O=16.0\text{O} = 16.0O=16.0.
A student prepares some ammonium nitrate in the laboratory.
She predicts that she should make 16.0 g16.0\text{ g}16.0 g of ammonium nitrate.
Her percentage yield is 75%75\%75%.
Calculate the actual mass of ammonium nitrate that the student makes.
91 exam-style questions on OCR GCSE Chemistry Monitoring chemical reactions. Each one has a worked solution and a mark scheme showing where the marks go.