Alcohols can be used as fuels. The table below shows the energy released when 1.00 g of different alcohols is completely burned.
| Alcohol | Formula of one molecule of the alcohol | Energy released in kJ/g\text{kJ/g}kJ/g |
|---|---|---|
| Ethanol | C2H5OH\text{C}_2\text{H}_5\text{OH}C2H5OH | 29.6 |
| Propanol | C3H7OH\text{C}_3\text{H}_7\text{OH}C3H7OH | 33.6 |
| Butanol | C4H9OH\text{C}_4\text{H}_9\text{OH}C4H9OH | 36.1 |
| Pentanol | C5H11OH\text{C}_5\text{H}_{11}\text{OH}C5H11OH | 37.7 |
| Hexanol | C6H13OH\text{C}_6\text{H}_{13}\text{OH}C6H13OH | 38.9 |
| Heptanol | C7H15OH\text{C}_7\text{H}_{15\text{OH}}C7H15OH | 39.8 |
Calculate the mass of propanol that must be burned to release the same amount of energy as burning 1.00 g of hexanol.
Give your answer to 3 significant figures.
12 exam-style questions on AQA GCSE Chemistry 7.2 Reactions of alkenes and alcohols, covering 7.2.1 Structure and formulae of alkenes, 7.2.2 Reactions of alkenes, 7.2.3 Alcohols, and 7.2.4 Carboxylic acids. Each one has a worked solution and a mark scheme showing where the marks go.