# Chemistry

A compound contains only carbon, hydrogen, nitrogen, and oxygen. Combustion of 0.157 of the compound produced 0.213g CO2 and 0.0310 g H20. In another experiment, it is found that 0.103g of the compound produces 0.0230 g NH3. What is the empirical formula of the compound?

this is what i tried....
Compound (0.157g) + O2--> CO2(.213g) +H2O(.0310g)

1. 👍 0
2. 👎 0
3. 👁 159
1. I would convert 0.213g CO2 to g C, then to %C. Convert 0.0310 g H2O to grams H, then top %H. Add g H to g C and subtract from 0.157 to obtain g O, and convert to %O. Then for the separate run on N, convert g NH3 to g N and to %N.
Take a 100 g sample and that will provide you with those percentages C, H, N, O. (For example, 60% C will become 60.0 g C).
Convert g C to moles.
Convert g H to moles.
Convert g O to moles.
Convert g N to moles.

Finally, you want to find the ratio of each of these elements to each other in small whole numbers. The easy way to do that is to divide the smallest number by itself which assures of 1.000 for that number. Divide all of the other numbers by that same small number, then round to whole numbers. That should be the empirical formula. [Note: in rounding the numbers, don't round numbers that are between xx.25 and xx.75--for example 1:1.5 would become 2:3 and not 1 to 1 or 1 to 2.]
Check my thinking.

1. 👍 0
2. 👎 0
2. C18 H13 N5 O22?

1. 👍 0
2. 👎 0
posted by alex

## Similar Questions

1. ### smk lutong

A compound consists only of carbon, hydrogen, nitrogen, and oxygen.  Combustion of 10.68 g of the compound  produced 16.01 g carbon dioxide and 4.37 g of water.  the molsr mass of the compound is 176.1

asked by nadeen on September 16, 2013
2. ### chemestry

A compound contains only carbon, hydrogen, nitrogen, and oxygen. Combustion of 0.157g of the compound produced 0.123g carbon dioxide and 0.0310g water. In another experiment, it is found that 0.103g of the compound produces

asked by salz on March 11, 2016
3. ### 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
4. ### Chemistry

Hi, I posted a question yesterday : A compound contains only carbon, hydrogen, nitrogen, and oxygen. Combustion of 0.157 of the compound produced 0.213g CO2 and 0.0310 g H20. In another experiment, it is found that 0.103g of the

asked by Anonymous on April 15, 2010
5. ### chemistry

2.4g of a compound of carbon, hydrogen and oxygen gave on combustion, 3.52g of CO2 and 1.44g of H2O. The relative molecular mass of the compound was found to be 60. a)What are the masses of carbon, hydrogen and oxygen in 2.4g of

asked by Bria on October 20, 2013
6. ### chemistry

2.4g of a compound of carbon, hydrogen and oxygen gave on combustion, 3.52g of CO2 and 1.44g of H2O. The relative molecular mass of the compound was found to be 60. a)What are the masses of carbon, hydrogen and oxygen in 2.4g of

asked by Bria on October 20, 2013
7. ### 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

asked by Brian on March 14, 2013
8. ### C hemistry

An unknown compound contains only carbon, hydrogen, and oxygen . Combustion of 2.50 g of this compound produced 3.67 g of carbon dioxide and 1.50 g of water. What is the empirical formula of a substance that contains 8.33×10−2

asked by isoka on September 26, 2010
9. ### Chemistry

The molecular formula of a compound containg only carbon and hydrogen is to be determined. When a sample of the compound is burned on oxygen gas, 7.2 grams of water and 7.2 liters of carbon dioxide gas are produced(measured at

asked by Patrick on January 9, 2011
10. ### chemistry

Upon combustion, 4.30 grams sample of a compound containing only carbon, hydrogen, and oxygen produced 8.59 g of CO2 and 3.52g of H2o. what is empirical formula of the compound ?

asked by Ayesha on February 25, 2015

More Similar Questions