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Y Part B Menthol, the substance we can smell in mentholated cough drops, is composed of C. H. and O. A 0.1005-mg sample of menthol is combusted, producing 0.2829 mg of CO₂ and 0.1159 mg of H₂O. What Is the empirical formula for menthol? Express your answer as a chemical formula. C10H200 ✓ Previous Answers Correct Since both CO₂ and H₂O contain oxygen, there is an extra step to calculate the number of moles of oxygen in the sample. The numbers of moles of C and H calculated from the collected masses of CO₂ and H₂O, respectively, must be converted to the masses of C and H. Once you have the mass of each, the mass contribution of C and H can be subtracted from the mass of the menthol sample. This will give you the mass of oxygen, which can be converted to moles using its atomic mass. Part C If the compound has a molar mass of 156 g/mol, what is its molecular formula? Express your answer as a chemical formula. ΕΞΑΣΦΑ 4

Y Part B Menthol, the substance we can smell in mentholated cough drops, is composed of C. H. and O. A 0.1005-mg sample of menthol is combusted, producing 0.2829 mg of CO₂ and 0.1159 mg of H₂O. What Is the empirical formula for menthol? Express your answer as a chemical formula. C10H200 ✓ Previous Answers Correct Since both CO₂ and H₂O contain oxygen, there is an extra step to calculate the number of moles of oxygen in the sample. The numbers of moles of C and H calculated from the collected masses of CO₂ and H₂O, respectively, must be converted to the masses of C and H. Once you have the mass of each, the mass contribution of C and H can be subtracted from the mass of the menthol sample. This will give you the mass of oxygen, which can be converted to moles using its atomic mass. Part C If the compound has a molar mass of 156 g/mol, what is its molecular formula? Express your answer as a chemical formula. ΕΞΑΣΦΑ 4

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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▼ Part A Combustion analysis of toluene, a common organic solvent, gives 6.45 mg of CO₂ and 1.51 mg of H₂O. It the compound contains only carbon and hydrogen, what is its empirical formula? Express your answer as a chemical formula. C7Hs ▼ ✓ Correct Combustion analysis can be used for determining the empirical formulas of compounds containing only carbon, hydrogen, and oxygen. Combustion reactions, which occur in the presence of oxygen (O₂), form CO₂ and H₂O. Because all of the carbon in the sample is converted to CO₂ and all of the hydrogen in the sample is converted to H₂, O we can use dimensional analysis to determine the numbers of moles of C and H: Previous Answers Part B Y C10H200 BLEINE Dividing both values by 1.33 x 10-4 gives C:H of 1:1.14. This is not close enough to be considered 1:1. No obvious multipliers (2, 3, 4, etc.) produce an integer ratio. By trial and error, the correct multiplier seems to be 7. This makes the empirical formula CHs. Menthol, the substance we can smell in mentholated cough drops, is composed of C. H. and O. A 0.1005-mg sample of menthol is combusted, producing 0.2829 mg of CO₂ and 0.1159 mg of H₂0. What Is the empirical formula for menthol? Express your answer as a chemical formula. Previous Answers Part C moles C 5.86 x 10³ g CO₂ x moles H 1.37 x 103 g H₂O x = If the compound has a molar mass of 156 g/mol, what is its molecular formula? Express your answer as a chemical formula. | ΑΣΦ À chemical GE Correct Since both CO₂ and H₂O contain oxygen, there is an extra step to calculate the number of moles of oxygen in the sample. The numbers of moles of C and H calculated from the collected masses of CO2 and H₂O, respectively, must be converted to the masses of C and H. Once you have the mass of each, the mass contribution of C and H can be subtracted from the mass of the menthol sample. This will give you the mass of oxygen, which can be converted to moles using its atomic mass. 1 mol CO₂ X 44.01 g CO₂ 1 mol H₂O X 18.02 g H₂O > 1 mol C 1 mol CO₂ 2 mol H 1 mol H₂O does not occur for this question = 1.33 x 10 - 1.52 x 10 ► mol C mol H
Transcribed Image Text:▼ Part A Combustion analysis of toluene, a common organic solvent, gives 6.45 mg of CO₂ and 1.51 mg of H₂O. It the compound contains only carbon and hydrogen, what is its empirical formula? Express your answer as a chemical formula. C7Hs ▼ ✓ Correct Combustion analysis can be used for determining the empirical formulas of compounds containing only carbon, hydrogen, and oxygen. Combustion reactions, which occur in the presence of oxygen (O₂), form CO₂ and H₂O. Because all of the carbon in the sample is converted to CO₂ and all of the hydrogen in the sample is converted to H₂, O we can use dimensional analysis to determine the numbers of moles of C and H: Previous Answers Part B Y C10H200 BLEINE Dividing both values by 1.33 x 10-4 gives C:H of 1:1.14. This is not close enough to be considered 1:1. No obvious multipliers (2, 3, 4, etc.) produce an integer ratio. By trial and error, the correct multiplier seems to be 7. This makes the empirical formula CHs. Menthol, the substance we can smell in mentholated cough drops, is composed of C. H. and O. A 0.1005-mg sample of menthol is combusted, producing 0.2829 mg of CO₂ and 0.1159 mg of H₂0. What Is the empirical formula for menthol? Express your answer as a chemical formula. Previous Answers Part C moles C 5.86 x 10³ g CO₂ x moles H 1.37 x 103 g H₂O x = If the compound has a molar mass of 156 g/mol, what is its molecular formula? Express your answer as a chemical formula. | ΑΣΦ À chemical GE Correct Since both CO₂ and H₂O contain oxygen, there is an extra step to calculate the number of moles of oxygen in the sample. The numbers of moles of C and H calculated from the collected masses of CO2 and H₂O, respectively, must be converted to the masses of C and H. Once you have the mass of each, the mass contribution of C and H can be subtracted from the mass of the menthol sample. This will give you the mass of oxygen, which can be converted to moles using its atomic mass. 1 mol CO₂ X 44.01 g CO₂ 1 mol H₂O X 18.02 g H₂O > 1 mol C 1 mol CO₂ 2 mol H 1 mol H₂O does not occur for this question = 1.33 x 10 - 1.52 x 10 ► mol C mol H
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