Complete the table below for calculating the formula weight of the ionic compound aluminum oxide, Al,O3. (Enter atomic and formula weights to two decimal places.)

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 =

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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)

Write the empirical formula for at least four ionic compounds that could be formed from the following ions:

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.

Given the following average atomic masses (in atomic mass unit, u),Hydrogen: 1.008 u, Oxygen: 15.999 u, and sulfur: 32.06 u.What percentage of sulfuric acid’s (H2SO4) mass is oxygen? Express your answer to 2 decimal places.

A chemist decomposes samples of several compounds; the masses of their constituent elements are listed. Calculate the empirical formula for each compound. Express your answer as a chemical formula   0.2907 g F, 0.1224 g O 0.524 g Na, 0.569 g As, 0.486 g O  1.443 g Se, 2.591 g Cl

When 2.013 grams of a hydrocarbon, CxHy, were burned in a combustion analysis apparatus, 6.315 grams of CO2 and 2.586 grams of H2O 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 =