# Chemistry

2) What is the empirical formula of a compound containing C, H, O if combustion of 1.23g of the compound yields 1.8g CO2 and .74g of H2O

3) What are the empirical and molecular formulas of a hydrocarbon if combustion of 2.10g of the compound yields 6.59g CO2 and 2.7g H20 and its molar mass is about 84g/mol

I really do not understand the steps to do this. I understand the standard way going from grams to moles then I do not know what to do with the values I calculate.

1. 👍 0
2. 👎 0
3. 👁 1,112
1. OK. Step by step #2 and I'll assume you know how to get from grams to mols.
6.59g CO2 = 0.150 mols CO2 = 0.150 mols C.
2.7 g H2O = 0.150 mols H2O = 0.300 mols H(atoms)
So now we have
0.150 g C
0.300 g H

We want to find the ratio, in small whole numbers, with no number being smaller than 1.00. The easy way to do that is to divide the smaller number by itself.
C = 0.150/0.150 = 1.00. That way assures us of getting 1.00 for the smaller number.
Then divide all of the other numbers (just one other one in this problem but many will have more than one).
0.300/0.150 = 2.00
So the ratio is C1.00H2.00 but we don't right the 1.00 and we would show CH2 for the empirical formula.

#1 you must convert mols CO2 and mols H2O to grams C, grams H and find O by total mass -mass C - mass H = mass O.

Then launch into the above to find the ratio. If you get stuck show your work and explain what you don't understand about the next step.

1. 👍 0
2. 👎 0

## Similar Questions

1. ### Chemistry

An unknown compound contains only C, H, and O. Combustion of 4.50 g of this compound produced 10.2 g of CO2 and 4.19 g of H2O. What is this empirical formula of the unknown compound?

2. ### Chemistry

A certain compound containing only carbon and hydrogen was found to have a vapor density of 2.550 g/L at 100 degrees C and 760 mm Hg. If the empirical formula of this compound is CH, what is the molecular formula of this compound?

3. ### Chemistry

Combustion analysis of an unknown compound containing only carbon and hydrogen produced 2.277 g of CO2 and 1.161 g of H2O. What is the empirical formula of the compound? How do I go about solving this?

4. ### Chemistry

A compound containing only carbon, hydrogen and oxygen is subjected to elemental analysis. Upon complete combustion, a .1804g sample of the compound produced .3051g of CO2 and .1249g of H2O. What is the empirical formula of the

1. ### Chemistry- Empirical Formula

Aniline, consists of C, H, and N. Combustion of such compounds yields CO2, H2O, and N2. If the combustion of 9.71 mg of aniline yields 6.63 mg H2O and 1.46 mb N2, what is the empirical formula? What is the molecular formula of a

2. ### Chemistry

combustion analysis of 63.8 mg of C,H, and O containing compound produced 145.0 mg of CO2 and 59.38 mg of H2O. What is the empirical formula for the compound?

3. ### Chemistry

1) A compound has the following percentages by mass: barium, 58.84%; sulfur, 13.74%; oxygen, 27.43%. Determine the empirical formula of the compound. 2) If a 1.271-g sample of aluminum metal is heated on a chlorine gas atmosphere,

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

1. ### Chemistry

A compound containing only C, H, and O was extracted from the bark of the sassafras tree. The combustion of 36.3mg produced 98.6 of CO2 and 20.2mg of H2O. The molar mass of the compound was 162 g/mol. Determine its empirical and

2. ### chemistry

A compound is found to be 51.39% carbon, 8.64% hydrogen, and 39.97% nitrogen. It has a molecular molar mass of 140.22 g/mol. (This question requires one to find the empirical formula to end up with the final answer in molecular

3. ### Chemistry

Combustion analysis of 0.300 g of an unknown compound containing carbon, hydrogen, and oxygen produced 0.5213 g of CO2 and 0.2835 g of H2O. What is the empirical formula of the compound? C2H5O C3H8O2 C2H10O3 C2H5O2

4. ### Chemistry

A student calculates the empirical formula of a compound to be C1.5H3.5. Express this as a correct empirical formula.