Sulfur trioxide is produced in a pilot reactor using this reaction.
2SO2+O2⇌2SO3 \mathrm{2SO_{2} + O_{2} \rightleftharpoons 2SO_{3}} 2SO2+O2⇌2SO3Oxygen is in excess. The production record for one run is shown in the table.
| Mass of sulfur dioxide supplied (tonnes) | Mass of sulfur trioxide obtained (tonnes) |
|---|---|
| 1.60 | 1.70 |
Relative atomic mass (ArA_rAr): O = 16.0 S = 32.0
Calculate the percentage yield of sulfur trioxide in this run.
A larger run is required to produce 25.5 tonnes of sulfur trioxide. The percentage yield is the same as in the pilot run.
Calculate the mass of sulfur dioxide that must be supplied. Oxygen is in excess.
152 exam-style questions on OCR GCSE Chemistry 5.1 Monitoring chemical reactions, covering 5.1.1 The technique of titration, 5.1.2 Theoretical mass, percentage yield and atom economy, 5.1.3 Concentration of a solution in mol/dm3, 5.1.4 Concentration calculations and titration results, 5.1.5 Molar gas volume and volumes of gases in reactions, and 5.1.6 Choosing a reaction pathway. Each one has a worked solution and a mark scheme showing where the marks go.