A 6.300 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 8.934 grams of CO, and 5.487 grams of H,O are produced. In a separate experiment, the molecular weight is found to be 62.07 amu. Determine the empirical formula and the molecular formula of the organic compound. Enter the elements in the order C, H, O empirical formula = molecular formula=

A 6.300 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 8.934 grams of CO, and 5.487 grams of H,O are produced. In a separate experiment, the molecular weight is found to be 62.07 amu. Determine the empirical formula and the molecular formula of the organic compound. Enter the elements in the order C, H, O empirical formula = molecular formula=

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

When 6.165 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 18.67 grams of CO₂ and 9.557 grams of H₂O were produced. In a separate experiment, the molar mass of the compound was found to be 58.12 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question. empirical formula = molecular formula =
A certain chemical substance has the following percent composition by mass. Element Mass Percent carbon 25.29% hydrogen 3.891% bromine 56.08% nitrogen 14.75% Determine the empirical formula for the compound.Enter your answer without subscripts. C12H21Cl3 should be entered as C12H21Cl3. Enter elements in the order C, H, followed by the remaining elements alphabetically. Single elements do not need to have a subscript. CH4 should be entered as CH4, not C1H4.Empirical Formula: Answer
Use percent composition and molar mass to determine molecular formula. Analysis of a compound of carbon, hydrogen and oxygen showed that it is 52.13% C and 13.15% H, with O accounting for the remainder. In a separate experiment, the molar mass of the compound was found to be 46.08 g/mol. Determine the molecular formula of the compound. Enter the elements in the order C, H, O.
A 1.746 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 4.405 grams of Co, and 0.7731 grams of H20 are produced. In a separate experiment, the molar mass is found to be 122.1 g/mol. Determine the empirical formula and the molecular formula of the organic compound. Enter the elements in the order C, H, O empirical formula = molecular formula =
Sample A 8.074 gram sample of an organic compound containing C, H and O is analyzed by combustion analysis and 20.88 grams of CO₂ and 4.274 grams of H₂O are produced. In a separate experiment, the molar mass is found to be 136.2 g/mol. Determine the empirical formula and the molecular formula of the organic compound. (Enter the elements in the order C, H, O.) Empirical formula: Molecular formula:
An unknown compound contains only CC , HH , and OO . Combustion of 8.60 g8.60 g of this compound produced 17.2 g17.2 g CO2CO2 and 7.03 g7.03 g H2OH2O . What is the empirical formula of the unknown compound? Insert subscripts as needed.
One form of asbestos called chrysotile is considered to be a human carcinogen. Mass analysis shows that the composition of chrysotile is 26.3% Mg, 20.2% Si, 1.45% H, and the remainder of the mass is oxygen. Determine the empirical formula of chrysotile. ( Type in the formula without spaces or subscripts in the order it appears in the problem. As in Mg1Si2H3O4)
When 6.961 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 21.84 grams of CO₂ and 8.943 grams of H₂O were produced. In a separate experiment, the molar mass of the compound was found to be 28.05 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question. empirical formula = molecular formula = =
A 3.000 g sample of a gaseous compound was found to contain 2.560 g of carbon and 0.440 g of hydrogen. A) What is the simplest formula of the compound (Write C first and then H)? You won't be able to make the numbers a subscript. For instance, for MgCl2 enter MgCl2. B) The molar mass of the compound was found to be 42.08 g/mol. What is the molecular formula of the compound? You won't be able to make the numbers a subscript. For instance, for MgCl2 enter MgCl2.
When 4.007 grams of a hydrocarbon, C,Hy, were burned in a combustion analysis apparatus, 12.14 grams of CO, and 6.212 grams of H20 were produced. In a separate experiment, the molar mass of the compound was found to be 58.12 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question. empirical formula = molecular formula =
When 6.608 grams of a hydrocarbon, C,Hy, were burned in a combustion analysis apparatus, 20.73 grams of CO2 and 8.489 grams of H,O were produced. In a separate experiment, the molar mass of the compound was found to be 70.13 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question. empirical formula molecular formula
When 5.095 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 15.61 grams of CO₂ and 7.457 grams of H₂O were produced. In a separate experiment, the molar mass of the compound was found to be 86.18 g/mol. Determine the empirical formula and the molecular formula of the hydrocarbon. Enter the elements in the order presented in the question. empirical formula molecular formula = = Previous Next