# chemistry

an organic compound contains C , H and O. in one combustion analysis, 10.71 g of this compound yields 6.41 g of H2O and 15.72 g of CO2. Calculate the number of carbon atoms in this organic compound if the molar mass of the compound is 146 g/mol

1. 👍 0
2. 👎 0
3. 👁 347
1. Find the formula as follows:
g C = g CO2 x atomic mass C/molar mass CO2 = approx 4
g H = g H2O x 2*atomic mass H/molar mass H2O = approx 0.7
g O = g compound - g C - g H = approx 6

mols C = g C/atomic mass C = approx 0.35
mols H = g H/atomic mass H = approx 0.7
mols O = g O/atomic mass O = approx 0.35 so the ratio is
CH2O for the empirical formula and 30 is the empirical mass.
molecular formula is 146/30 = 4.9 so round to 5 and the molecular formula is C5H10O5. My assumption is that the 146 is an approx molar mass but it is 150 from the molecular formula.
mols compound is 10.71/150 = x
C atoms = x*6.02E23*5

1. 👍 0
2. 👎 0

## Similar Questions

1. ### 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?

asked by Emma on December 6, 2012
2. ### 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?

asked by Casey on September 21, 2013
3. ### Cemistry

When a 0.952 g sample of an organic compound containing C, H,and O is burned completely in oxygen, 1.35 g of CO2 and0.826 g of H2O are produced. What is the empiricalformula of the compound?

asked by Eddy on September 29, 2011
4. ### Chemistry

Analysis of a sample of an organic compound showed it contains 39.9%carbon,6.9%hydrogen and 53.2%oxygen. a)calculate the empirical formula b)if the relative molecular mass is 60,what is the molecular formula of the

asked by Angel on December 19, 2015
5. ### chemistry

a compound contains 5.2% by mass Nitrogen. It also contains carbon, hydrogen and oxygen. Combustion of 0.085g of the compound produced 0.224g of carbon dioxide and 0.0372g of water. Calculate the empirical formula of the compound.

asked by martina on October 8, 2013
1. ### 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?

asked by Laura on September 19, 2010
2. ### 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

asked by Annabelle on April 10, 2014
3. ### Chemistry

Assume that the complete combustion of one mole of ethanol to carbon dioxide and water liberates 1370 kJ/mol (?G°\' = –1370 kJ/mol). If the energy generated by the combustion of ethanol is entirely converted to the synthesis of

asked by Royzel on January 27, 2014
4. ### Chemistry

Diethyl ether (also known as “ether”), C4H10O (l), is an organic compound that has long been used as a surgical anesthetic. The complete combustion of 1 mol of C4H10O (l) to CO2 (g) and H2O (l) yields ΔH °=-2723.7 kJ. a)

asked by Feufolia on March 10, 2016
5. ### science(chemistry)

an organic compound contains 49.3 percent carbon,6.84percent hydrogen and its vapour density is 73.molecular formula of compound

asked by akshar on June 5, 2011
6. ### chemistry

Combustion analysis of 1.0g of a compound containing carbon , hydrogen and oxygen gives 2.3 g of carbon dioxide and 0.93g of water . If The relative molecular mass is 58. Calculate The empirical and molecular formula

asked by hiedi on September 20, 2015