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Unformatted text preview: iii. Molecular formula will be a multiple of the empirical formula. Therefore, the molar mass will be a multiple of the empirical mass 1. Example 2. C3H4O3 is the empirical formula of vitamin c a. Empirical mass = 88.06 g/ mol b. Molar Mass = 176.14 g c. 176.14/88.06 = 2 d. (C 3 H 4 O 3 )2 = C 6 H 8 O 6 b. Molecular formula is the actual numbers of atoms in a molecular compound c. Mass percentage is another way to express the ratio IV)Combustion Analysis a. Masses used from empirical formula come from combustion analysis b. Mainly used for organic compounds i. Study how much CO 2 , H 2 0, N 2 is released in the exhaust ii. Will mainly ignore N2 iii. Find the moles of Carbon and Hydrogen and Oxygen iv. Divide by the smallest number of moles found k...
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This note was uploaded on 07/17/2010 for the course 160 161 taught by Professor Kim during the Spring '08 term at Rutgers.
- Spring '08