Assume that 3.57 x 106 kJ are needed to heat a swimming pool. If this energy is derived from the combustion of liquid ethanol (CH3CH2OH) at standard conditions (25 oC and 1 atm) what volume in liters of ethanol must be burned?
The heat of combustion of ethanol is 1366.818 kJ/mol. The density of ethanol is 0.789 g/cm3
Enter a numeric answer only. Do not enter units.
2007-01-31 01:50:14 · 1 answers · asked by sunyrob 1 in Science & Mathematics ➔ Chemistry
Divide the total energy required by the heat of combustion. The result M is the number of moles required.
Calculate the MW of ethanol.
Multiply M * MW. This is ME the mass of ethanol required in g.
Multiply density by 1000. This is D1000, density in g/liter.
Divide ME by D1000. That's the answer.
I hope you can do this easy math yourself, and some point-hungry weed doesn't come and do it for you..
2007-02-02 06:24:48 · answer #1 · answered by kirchwey 7 · 0⤊ 0⤋