When 1.915 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 6.474 grams of CO2 and 1.325 grams of H2O were produced. In a separate experiment, the molar mass of the compound was found to be 78.11 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.

In a first expirement, a compound is analyzed and found to contain 85.63% C and 14.37% hydrogen by mass. Determine the empirical formula of the compound. In a separate expirement, the molar mass of the compound from the first expirement was found to be 42.081 g/mol. What is the molecule formula for the compound?

A 3.06 mg sample of a compound containing carbon, hydrogen, and oxygen underwent combustion producing 6.95 mg of CO2 and 2.84 mg of H2O. What is the empirical formula of the compound?  If the compound has a molar mass of 160 ± 5 g/mol, what is its molecular formula?

a) Elemental analysis of an unknown sample shows its mass composition to be 49.45% carbon (C), 28.84% nitrogen (N), 16.46% oxygen (O) and 5.18% hydrogen (H). Using mass spectrometry, you determine that the molar mass of the compound is equal to 194.19 g/mol. What is the molecular formula of the unknown compound? b) We carry out combustion of C5H10O (molar mass = 86.13 g/mol) (its reaction with O2, to produce CO2 and H2O). What is the maximum mass of products obtained (CO2 (molar mass = 44.01 g/mol) and H2O (molar mass = 18.02g/mol)), if the reaction vessel contains 15.0 g of C5H10O and 1.00 mol of Oz.

When 5.974 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.74 grams of CO2 and 7.675 grams of H2O were produced.In a separate experiment, the molar mass of the compound was found to be 56.11 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon.

Valproic acid, a medication used to treat epilepsy and bipolar mania, contains only C, H, and O. Combustion of 1.000 g of valproic acid produces 2.441 g of CO₂ and 1.000 g of H₂O. Determine the molar mass of the compound if it is between 80.0 and 150.0 g/mol. Provide an answer to four significant figures.

An unknown compound that is composed of C, H and O atoms was submitted to a lab for determination of formula. Combustion in air of 1.230 g of the unknown compound yields 2.162 g CO2 and 1.033 g H2O. What is the empirical formula of the unknown compound?

5. An organic compound containing only C, H, and possibly O was subjected to combustion analysis. A sample weighing 0.7585 g yielded 1.295 g CO₂ and 0.464 g H₂O. What is the empirical formula of the compound?

Upon combustion, a 0.8009 gg sample of a compound containing only carbon, hydrogen, and oxygen produces 1.6004 gg CO2CO2 and 0.6551 gg H2OH2O. Find the empirical formula of the compound.

When a 5.712 g sample of an organic compound containing C, H, and O is burned completely in oxygen, 8.1 g of CO2 and 4.956 g of H2O are produced. What is the empirical formula of the compound?