9. A 0.1342-gram sample of an unknown compound composed of C, H, and O was burned in air, producing 0.240 g of CO2 and 0.0982 g of H2O. If the molar mass of the compound is 222.4 g/mole, determine its empirical and molecular formulas. c Cx Hy Ox + O2 The reston Scrap P
9. A 0.1342-gram sample of an unknown compound composed of C, H, and O was burned in air, producing 0.240 g of CO2 and 0.0982 g of H2O. If the molar mass of the compound is 222.4 g/mole, determine its empirical and molecular formulas. c Cx Hy Ox + O2 The reston Scrap P
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter9: Chemical Quantities
Section: Chapter Questions
Problem 81AP: For each of the following incomplete and unbalanced equations, indicate how many moles of the second...
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My questions is about when we convert to moles in this problem. Why do we convert C and H to moles, then grams, and not say O and H and then find the grams of C from them. Or why can't we just find the moles of O from the given weight of H2O? Basically, why is O excluded in finding moles in the first part of the problem. I understand we need to subtract from the given weight 0.1342 grams but don't know why we can't just subtract g of O and grams of C why must it be C and H.
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