A research chemist is investigating the thermal efficiency of various liquid biofuels. The chemist combusts samples of different straight-chain alcohols under standard laboratory conditions to determine the energy released per gram.
| Alcohol | Chemical formula of alcohol molecule | Energy released in kJ/g\text{kJ/g}kJ/g |
|---|---|---|
| Ethanol | C2H5OH\text{C}_2\text{H}_5\text{OH}C2H5OH | 29.8 |
| Propanol | C3H7OH\text{C}_3\text{H}_7\text{OH}C3H7OH | 33.5 |
| Butanol | C4H9OH\text{C}_4\text{H}_9\text{OH}C4H9OH | 36.0 |
| Pentanol | C5H11OH\text{C}_5\text{H}_{11}\text{OH}C5H11OH | 37.8 |
| Hexanol | C6H13OH\text{C}_6\text{H}_{13}\text{OH}C6H13OH | 39.0 |
| Heptanol | C7H15OH\text{C}_7\text{H}_{15}\text{OH}C7H15OH | 40.2 |
Calculate the mass of ethanol that must be completely burned to release the same amount of thermal energy as burning 4.80 g4.80\text{ g}4.80 g of hexanol. Give your answer to 3 significant figures.