A 9.107 g sample of an amino acid containing the atoms C, H, N, and O, was subjected to combustion analysis and yielded 8.802 g of carbon dioxide, 4.505 g of water, and 4.600 g of nitrogen dioxide. Its molar mass was measured to be 91.07 g/mole. Determine the empirical formula using the following steps. A. (12) Calculate the number of moles of CO, H,0, and NO,. B. (24) Calculate the masses and moles of carbon, hydrogen, and nitrogen from the appropriate products. C. (8) Determine the mass and moles of oxygen in the original sample. D. (6) Use the data to derive the empirical formula and the molecular formula.
A 9.107 g sample of an amino acid containing the atoms C, H, N, and O, was subjected to combustion analysis and yielded 8.802 g of carbon dioxide, 4.505 g of water, and 4.600 g of nitrogen dioxide. Its molar mass was measured to be 91.07 g/mole. Determine the empirical formula using the following steps. A. (12) Calculate the number of moles of CO, H,0, and NO,. B. (24) Calculate the masses and moles of carbon, hydrogen, and nitrogen from the appropriate products. C. (8) Determine the mass and moles of oxygen in the original sample. D. (6) Use the data to derive the empirical formula and the molecular formula.
Chemistry by OpenStax (2015-05-04)
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Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
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Chapter18: Representative Metals, Metalloids, And Nonmetals
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Problem 78E: Phosphoric acid, one of the acids used in some cola drinks, is produced by the reaction of...
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Transcribed Image Text:A 9.107 g sample of an amino acid containing the atoms C, H, N, and O, was
subjected to combustion analysis and yielded 8.802 g of carbon dioxide, 4.505
g of water, and 4.600 g of nitrogen dioxide. Its molar mass was measured to
be 91.07 g/mole. Determine the empirical formula using the following steps.
A. (12) Calculate the number of moles of CO, H,0, and NO,.
B. (24) Calculate the masses and moles of carbon, hydrogen, and nitrogen
from the appropriate products.
C. (8) Determine the mass and moles of oxygen in the original sample.
D. (6) Use the data to derive the empirical formula and the molecular
formula.
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