13. Empirical Formula and Combustion Analysis Calculations. i.) A compound containing only carbon and hydrogen was...

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13. Empirical Formula and Combustion Analysis Calculations. i.) A compound containing only carbon and hydrogen was found to be 81.80% carbon. What is the empirical formula? The molar mass of the compound is 132.6 g/mol. Determine the molecular formula? i.) E.Formula = C3H8 M. Formula = C9H24 ii.) A 20-g sample containing 12.974 g carbon,0.540 g hydrogen, and 6.486 g oxygen was analyzed. Determine the empirical and molecular formulas (molar mass = 296.236 g/mol). ii.) E.Formula = C8H403 M. Formula = C16H8O6 iii.) A compound with a known molecular weight (146.99 g/mol) that contains only C, H, and Cl was studied by combustion analysis. When a 0.367 g sample was combusted, 0.659 g of CO2 and 0.0892 g of H₂O formed. What are the empirical and molecular formulas? iii.) E.Formula = C3H₂Cl M. Formula = C6H4Cl₂ iv.) When a 1.000 g of vitamin C (molar mass= 176.12 g/mol) is placed in a combustion chamber and burned, the following data are obtained: mass of CO2 detected: 1.50 g, mass of H₂O detected 0.41 g. Use it to determine the empirical and molar formulas for vitamin C. *vitamin C contains C, H, and O iv.) E.Form = C3H403 M. Forma = C6H806 14.Hydrates. i.) A 3.592-g sample of hydrated magnesium bromide, MgBr₂ nH₂O, is dried in an oven. When the anhydrous salt is removed from the oven, its mass is 2.263 g. What is the value of n? i.) n = 6 ii.) A hydrate is determined to be 45.43% water, 24.78% cobalt, and 29.79 % chlorine. Find the chemical formula and name for this hydrate. ii.) CoCl₂ 6H₂0 cobalt (II) chloride hexahydrate 13. Empirical Formula and Combustion Analysis Calculations. i.) A compound containing only carbon and hydrogen was found to be 81.80% carbon. What is the empirical formula? The molar mass of the compound is 132.6 g/mol. Determine the molecular formula? i.) E.Formula = C3H8 M. Formula = C9H24 ii.) A 20-g sample containing 12.974 g carbon,0.540 g hydrogen, and 6.486 g oxygen was analyzed. Determine the empirical and molecular formulas (molar mass = 296.236 g/mol). ii.) E.Formula = C8H403 M. Formula = C16H8O6 iii.) A compound with a known molecular weight (146.99 g/mol) that contains only C, H, and Cl was studied by combustion analysis. When a 0.367 g sample was combusted, 0.659 g of CO2 and 0.0892 g of H₂O formed. What are the empirical and molecular formulas? iii.) E.Formula = C3H₂Cl M. Formula = C6H4Cl₂ iv.) When a 1.000 g of vitamin C (molar mass= 176.12 g/mol) is placed in a combustion chamber and burned, the following data are obtained: mass of CO2 detected: 1.50 g, mass of H₂O detected 0.41 g. Use it to determine the empirical and molar formulas for vitamin C. *vitamin C contains C, H, and O iv.) E.Form = C3H403 M. Forma = C6H806 14.Hydrates. i.) A 3.592-g sample of hydrated magnesium bromide, MgBr₂ nH₂O, is dried in an oven. When the anhydrous salt is removed from the oven, its mass is 2.263 g. What is the value of n? i.) n = 6 ii.) A hydrate is determined to be 45.43% water, 24.78% cobalt, and 29.79 % chlorine. Find the chemical formula and name for this hydrate. ii.) CoCl₂ 6H₂0 cobalt (II) chloride hexahydrate

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13 i Atomic Element percentage mass C H ii C Element amount H O So empirical formula is C3H8 Empiric... View the full answer