Recent content by cobaltcalcium

This is what's on my scratch paper so far: 054 moles at 1.51atm/375k yields 1 liter now molar wt for water is 18 g/m and CO2 is 44 g/m say x is number of moles hydrogen needed and y is number of moles carbon needed from above we build a formula total moles equal to .054 so x + y= .054...

I know the ideal gas law, how to find moles etc. Density = mass/volume. But I'm still getting confused with what to do with all the data.

This problem was proposed to us by our Chemistry professor. Consider a sample of a hydrocarbon at 0.959atm and 298K. Upon combusting the entire sample in oxygen, you collect a mixture of gaseous carbon dioxide and water vapor at 1.51atm and 375K. This mixture has a density of 1.391 g/L and...