#1
Vitamin C (Molar mass=176.12 g/mol) contains C,H and O. When a 1.00g sample of vitamin C is burned, 1.50 g of carbon dioxide and 0.41 g of water are produced. Determine EF and MF for vitamin C

EF= Empirical Formula
MF= Molecular Formula

I can do MF but I can't figure out the Empirical Formula.
GREAT ODIN'S RAVEN
#2
Empirical Formula:

Divide all the given masses by their relative atomic masses, then divide those by the lowest number you've calculated. Adjust into whole numbers.

How do you get 1.5 grams of CO2 from 1 gram of ascorbic acid?
#3
Quote by Shred Head
Empirical Formula:

Divide all the given masses by their relative atomic masses, then divide those by the lowest number you've calculated. Adjust into whole numbers.

How do you get 1.5 grams of CO2 from 1 gram of ascorbic acid?


Don't ask me that's what my paper says
GREAT ODIN'S RAVEN
#4
because it's combining with the oxygen from the atmosphere around it. I guess there's quite alot of carbon in vitamin C. but yea, for empirical formula, find out how many moles of each element you have, then divide that by the lowest, and you'll get the empirical formula. to get molecular formula, find the atomic mass of the empirical formula, and divide the molar mass (176.12) by that, and adjust to whole numbers, and voila. in theory, you shouldn't be able to do the MF without already having the EF.
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#5
Aah, i hated these kind of questions.


Its been 3 years since i've done these kind of questions.


So all i'll say is...


DO YOUR HOMEWORK YOURSELF!!!!!!!