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.