# chemistry

I need help with this problem...

A 1.208 g sample of a compound containing C, H, and O was burned to produce 2.561 g CO2 and 0.3930 g H2O. Calculate the empirical formula of the compound.

I always get stuck when it comes to finding the subscript for this compound.

1. Convert 2.561g CO2 to g C. Easiest done by 2.561 x (atomic mass C/molar mass CO2).
Convert 0.3930g H2O to g hydrogen. Easiest done by 0.3930 x (2*atomic mass H/molar mass H2O).
Then g O = 1.208 - g C - g H

Now convert g C, H, and O to moles.
moles = grams/molar mass.

Find the ratio of the elements to each other using whole numbers with the smallest being 1.00. That is easiest done by dividing the smallest number by itself; then divide the other mole amounts by the same small number.
If you have trouble, post your work and I can help guide you through it. Be sure to explain what you don't understand about the next step.

posted by DrBob222
2. I ended up with C_2.809 H_2.106 O_1

so would that be C_3 H_2 O?

posted by mark
3. I would round that way BUT I didn't get those numbers. I ended up with 1.99 for C, 1.496 for H, 1.00 for O which rounds to C2H1.5O but that in small whole numbers is C4H3O2 if I didn't make a math error. Look over your work to see if you can find an error; post your work and I'll look for an error if you wish.

posted by DrBob222

First Name

## Similar Questions

1. ### Chemistry

A 0.7381 g sample of a compound containing C, H, and F was burned to produce 0.6368 g CO2 and 0.1303 g H2O. Calculate the empirical formula of the compound. Do I have to take in account the O atoms?
2. ### chemistry

I got C_4 H_3 O_8 for this question but I'd like someone to check my answer, please. A 1.012 g sample of a compound containing C, H, and O was burned to produce 2.145 g CO2 and 0.3293 g H2O. Calculate the empirical formula of the
3. ### Chemistry

Is this correct? A 0.7473 g sample of a compound containing C, H, and O was burned to produce 1.909 g CO2 and 0.7813 g H2O. Calculate the empirical formula of the compound. I got C5 H10 O1. I'm not sure if that's correct..
4. ### AP Chemistry

An organic compound was synthesized and found to contain only C, H, N, O, and Cl. It was observed that when .150g sample of the compound was burned, it produced .138g of CO2 and .0566g of H2O. All the Nitrogen in a different .200g
5. ### Chemistry

A 2.20 g-sample of a compound containing carbon, hydrogen, and oxygen is burned and it produces 4.61 g CO2 and 0.94 g H2O. What is the empirical formula of this compound?
6. ### Chemistry

a compound was analyzed and found to contain C,H,N,O, and Cl. When o.150g sample of this compound was burned, it produced 0.138 g of CO2 and 0.0566 g of H2O. All of the Nitrogen in another sample of mass 0.200 g was converted to
7. ### Chemistry

A 0.100g sample of a compound containing C, H, and O is burned oxygen producing 0.1783 g of CO2 and 0.0734 g of H2O. Determine the empirical formula of the compound.
8. ### Chemistry

A 0.5438 g sample of a compound contains only C H and O was burned completely in oxygen.the products were 1.0390 g CO2 and 0.6369g H2O. Determine the empirical formula of thr compound
9. ### CHEMISTRY

A compound which contains hydrogen, oxygen, carbon only has molar mass of about 85 g/mol. When 0.43 g of the compound is burned in excess of oxyfen, 1.10 g of CO2 and 0.45 g of H2O are formed. Find the molecular formula and the
10. ### chemistry

a 2.500g sample of an unknown compound containing only C, H and O was burned in O2. The products were 4.776g of CO2 and 2.934g of H2O. a) what is the percent compostion of the original compound? %C- %H- %O and what is empirical

More Similar Questions