C H O Mass of element (in g) (assuming 100 g of compound) 1._38.6_ 2._9.76__ 3._51.56_ Moles of element 4.______ 5.______ 6.______ Moles of element/Smallest moles 7.______ 8.______ 9.______ Multiplier 10._____ 10._____ 10.______ Empirical formula 11._____ Molecular weight of empirical formula 12._____ Molecular weight of compound / Molecular weight of empirical formula 13._____ True formula = C12H36O12
C H O Mass of element (in g) (assuming 100 g of compound) 1._38.6_ 2._9.76__ 3._51.56_ Moles of element 4.______ 5.______ 6.______ Moles of element/Smallest moles 7.______ 8.______ 9.______ Multiplier 10._____ 10._____ 10.______ Empirical formula 11._____ Molecular weight of empirical formula 12._____ Molecular weight of compound / Molecular weight of empirical formula 13._____ True formula = C12H36O12
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
Chapter3: Stoichiometry
Section: Chapter Questions
Problem 196MP: Consider the following balanced chemical equation: A+5B3C+4D a. Equal masses of A and B are reacted....
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Question
An organic compound has a gram molecular weight of 372 g/mol, and its composition is 38.6% carbon, 9.76% hydrogen, and 51.56% oxygen. Determine (a) the empirical formula (b) the molecular formula.
C | H | O | |
Mass of element (in g) (assuming 100 g of compound) | 1._38.6_ | 2._9.76__ | 3._51.56_ |
Moles of element | 4.______ | 5.______ | 6.______ |
Moles of element/Smallest moles | 7.______ | 8.______ | 9.______ |
Multiplier | 10._____ | 10._____ | 10.______ |
Empirical formula | 11._____ | ||
Molecular weight of empirical formula | 12._____ | ||
Molecular weight of compound / Molecular weight of empirical formula |
13._____ |
True formula = C12H36O12
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