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Lecture 6

CHEM 131 Lecture Notes - Lecture 6: Unified Atomic Mass Unit, Molecular Mass, Atomic Mass


Department
Chemistry
Course Code
CHEM 131
Professor
Shuhua Ma
Lecture
6

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Chem 131 - 9/15
Molar Mass
1. The mass of 1 mole of a substance
a. 1 mole 12C atoms = 6.022 x 1023 atoms = 12.00 g
b. 1 12C atom = 12.00 amu
2. For any element
a. Atomic mass (amu) = molar mass (g/mol)
3. 1 amu = 1.6606 x 10-24g or 1 g = 6.022 x 1023 amu
Molecular Mass (or molecular weight)
4. The sum of the atomic masses (in amu) in a molecule
5. For any molecule
a. Molecular mass (amu) = molar mass (g/mol)
Formula Mass
6. The sum of the atomic masses (in amu) in an empirical formula)
7. Example:
a. Find the sum of NaCl (Na = 23; Cl = 35; 23 + 35 = 58 amu)
8. For any ionic compound or empirical formula
a. Formla mass (amu) = molar mass (g/mol)
Calculate
9. Calculate the mass in grams of 0.254 mol. C14H12O6
a. C14 = 168.154
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