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Chemical Composition

Chemical Composition. Mole (mol) – The number equal to the number of carbon atoms in 12.01 grams of carbon. Avogadro’s number – The number of atoms in exactly 12 grams of pure 12 C; 6.022 x 10 23 . One mole of anything contains 6.022 x 10 23 units of that substance.

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Chemical Composition

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  1. Chemical Composition Mole (mol) – The number equal to the number of carbon atoms in 12.01 grams of carbon. Avogadro’s number – The number of atoms in exactly 12 grams of pure 12C; 6.022 x 1023. One mole of anything contains 6.022 x 1023 units of that substance.

  2. Molar mass – The mass in grams of 1 mol of the substance. • Molar Mass of an element is the mass in grams of 6.022 x 1023 atoms. • Molar Mass of an compound is the mass in grams of 6.022 x 1023 molecules or units.

  3. % Composition = grams of element of element by mass grams of compound X 100 % Composition = molar mass of element__ of element by molar mass ofcompound X 100 molar mass

  4. Hydrate – Molecule with water attached to crystalline structure. Ex. CuSO4 * 5H2O molar mass of H2O % Comp. H2O = molar mass of X 100 hydrate compound

  5. Empirical Formula – Expressed the smallest whole-number ratio of the atoms present in a compound. Percent to massMass to moleDivide by smallMultiply 'til whole

  6. Molecular Formula – The exact formula of a molecule, giving the types of atoms and the number of each. Compare empirical formula mass to known molar mass. Molecular formula = (empirical formula)n n = molar mass empirical formula mass

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