Posted by **manny** on Wednesday, September 26, 2007 at 5:40pm.

Hi the following comes from my first homework assignment in AP Chemistry. I am totally lost on this question and don't know where to start. Thanks a lot in advance!!!!!

A 0.1247 g sample of ascorbic acid, Vitamin C, was burned in a carbon-hydrogen combustion apparatus to produce 0.1869 g of carbon dioxide, and 0.0510 g of water. Ascorbic acid contains only carbon, hydrogen, and oxygen. Determine the masses of C,H, and O in the sample and then determine the simplest formula.

- chem -
**DrBob222**, Wednesday, September 26, 2007 at 8:41pm
Convert 0.1869 g CO2 to g C.

0.1869 g CO2 x (1 mol C/1 mol CO2) = ?? g C.

Convert 0.0510 g H2O to g H.

0.0510 g H2O x (2 mols H/1 mol H2O) = ?? g H

Determine g oxygen by adding g C and g H and subtracting from the 0.1247 g sample initially taken.

Then the simplest (empirical formula) is determined by converting g C, H, and O to mols

mols C = g C/atomic mass C = xx mols C.

mols H = g H/atomic mass H = xx mols H.

mols O = g O/atomic mass O = xx mols O.

Now find the ratio of the three in simplest numbers; i.e., divide the smallest number by itself (thereby making it 1.00) and divide the other two numbers by the smallest number. Post your work if you get stuck.

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