chemistry

When 1.24g of an organic compound with the formula CxHyOz is burned in excess oxygen, 1.76g of carbon dioxide and 1.08g of water vapor are obtained. What is the empirical formula of the compound?

Determine the moles of CO2 in 1.76grams, that will give you the moles of C in the original compound.

Determine the moles of H2O in 1.08 grams, that will give you the moles of H2, double it, and you have the number of moles in the original compound.

Add the weight of the moles of C in the original compouond to the weight of moles of H in the orig compound, then subtract that weight from 1.24g. The remainder is the weight of O in the compound, now calculate the moles of O in that.

You have the moles of C, H, and O in the original compound.

Take the smaller of those three numbers, and divide into all three. The numbers you get will be the mole ratio.

For instance, assume you had these numbers....C .0024 moles, H .0050 moles, and O .0025 moles.

C is the lower number, dividing, we get
CH2O

1. 👍 0
2. 👎 0
3. 👁 269
1. Ghhhh

1. 👍 0
2. 👎 0

Similar Questions

1. general chemistry

A 1.24g sample of a hydrocarbon, when completely burned in excess of O2(g), yields 4.04g CO2 and 1.24g H20. Determine the empirical formula.

asked by StressedStudent on February 6, 2013
2. 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

asked by Clive Lodnyx on July 18, 2016
3. Chemistry

When 1.5173g of an a organic iron compound contains Fe,C,HH and O was burned in oxygen 2.838g CO2 and 0.8122g H2O wereproduce.in a separate experiment to determine mass % of iron, 0.3355g of the compound yield 0.0758g Fe2O3.What

asked by Mkubwa Ali Ismail on November 21, 2018
4. chemistry

one moles of a compound containing only carbon, hydrogen, and nitrogen was burned in the presence of excess oxygen to give 264g of CO2, 63 g of H20, and 46 g of NO2. Calculate the molecular formula of the compound.

asked by julie on September 16, 2007
5. Chemistry

5.6g of an organic compound on burning with excess oxygen gave 17.6g of carbon dioxide nd 7.2g of water what is the organic compound

asked by Abira on April 25, 2019
6. General Chemistry

An unknown compound has a formula of CxHyOz. You burn 0.1523 g of the compound and isolate 0.3718 g of CO2, and 0.1522 g of H2O. What is the empirical formula of the compound? If the molar mass is 72.1 g/mol what is the molecular

asked by Jashmid on December 8, 2010
7. Chemistry

A 2.52g sample of a compound containing only carbon, hydrogen, nitrogen, oxygen, and sulfur was burned in excess O to yield 4.36g of CO2 and 0.892g of H20. Another sample of the same compound of mass 4.14g, yielded g of SO3. A

asked by Christina on September 6, 2010
8. Chemistry

A compound of carbon, hydrogen, and oxygen was burned in oxygen, and 2.00g of the compound produced 2.868 g CO2 and 1.567 g H2O. In another experiment, 0.1107 g of the compound was dissolved in 25.0 g of water. This solution had a

asked by sevag on December 9, 2012
9. skyiline college

A compound of carbon, hydrogen, and oxygen was burned in oxygen, and 2.00g of the compound produced 2.868 g CO2 and 1.567 g H2O. In another experiment, 0.1107 g of the compound was dissolved in 25.0 g of water. This solution had a

asked by sevag on December 8, 2012
10. Chemistry

A compound of carbon, hydrogen, and oxygen was burned in oxygen, and 2.00g of the compound produced 2.868 g CO2 and 1.567 g H2O. In another experiment, 0.1107 g of the compound was dissolved in 25.0 g of water. This solution had a

asked by Desz on August 6, 2013

More Similar Questions