Sulfur dioxide reacts with oxygen in a reversible reaction to produce sulfur trioxide.
2SO2+O2⇌2SO3\mathrm{2SO_2 + O_2 \rightleftharpoons 2SO_3}2SO2+O2⇌2SO3
| Relative atomic mass (ArA_rAr) | Value |
|---|---|
| S | 32 |
| O | 16 |
| Experimental information | Value |
|---|---|
| Mass of sulfur dioxide used | 16.0 g |
| Oxygen | Excess |
| Mass of sulfur trioxide collected | 17.0 g |
Calculate the percentage yield of sulfur trioxide.
Explain why the reversible nature of the reaction may reduce the percentage yield of sulfur trioxide.
104 exam-style questions on AQA GCSE Chemistry 3.3 Yield and atom economy of chemical reactions, covering 3.3.1a Percentage yield, 3.3.1b Theoretical mass of a product, 3.3.2a Atom economy, and 3.3.2b Choosing a reaction pathway. Each one has a worked solution and a mark scheme showing where the marks go.