Quote:
Originally Posted by guage
Good grief Charlie Brown... This is a home work assignment my 16 year old daughter brought home from high school, she is a Junior.
I admit this is way beyond any help I can give her.
Anybody care to explain this?
Select a vehicle that can use all three grades of gasoline - unleaded, E-10 and E-85. Compare the carbonic acid that would be produced in the
atmosphere using unleaded gasoline, E-10 and E-85 driving from point A to point B a distance of 90 miles one-way.
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I took chem sophomore year (last year), had a 104 average for most of the year.. Forgot a bit by now.. Is this assuming that all H, C and O in the exhaust forms carbonic acid, or only a certain percentage? Also have to find the chemical composition of gasoline, since its a blend of many different hydrocarbons, unless your assuming its 100% octane. Pick a car and find MPG, calculate how many gallons are required to drive 90 miles, then convert that volume to moles of each fuel (first multiplying .85*gallons, .15*gallons to find amount of ethanol and gaslone in E85 for example). Then solve for mols of H2CO3 that would be formed from that many mols of gas + ethanol + oxygen.