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The Mole 9.3 And 9.4

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• Units for molar mass is g/mol
• Using the relationship of 1 mole of an element = relative atomic mass = molar mass in grams Since 1 mole of an element = molar mass ( mass of 1 mole of an element) Number of moles of an element x relative atomic mass = mass of element in grams
• 1 mole of element â€“Ar 1 mole of molecules â€“ Mr â€“ sum of Ar of the elements that made up that molecules If the compound is covalent we use the term relative molecular mass, if the compound is ionic, we use the term relative formula mass. When doing calculations, can just use the abbreviation M r
• Transcript

• 1. Chapter 9.3 and 9.4 Mole and Molar Mass
• 2.
• You should have completed the worksheet on Mole and Molar Mass.
• You may check your answers by clicking on this document: (Answers to Mole and Molar Mass).
• 3. Summary
• A mole of any substance contains 6 X 10 23 particles.
• 6 X 10 23 is called the Avogadroâ€™s constant or Avogadroâ€™s number.
• Molar mass refers to the mass of one mole of a substance. It has the same value as A r or M r .
• 4. Molar Mass
• 2.Mass of one mole of atoms of the element particles e.g atoms, molecules or ions
• 6 x 10 23 atoms = 1 mole of atoms = _____ g /mol
MOLAR MASS
• 5. Formulae to remember
• 1.
• (a) Number of moles = Number of particles
• 6 x 10 23 (Avogadroâ€™s constant)
• OR
• (b) Number of moles x 6 x 10 23 = Number of particles
• 6. Formulae to Remember
• 2. (a) Relationship between mole and molar mass
• Number of moles of an element
• = mass of element in grams
• relative atomic mass of the element
Moles = Mass A r
• 7. Formulae to Remember
• 2 (b) Mass of one mole of substances
• (covalent compounds)
• = mass of substance in grams
• relative molecular mass
• (c) Mass of one mole of substance
• (ionic compounds)
• = mass of substances in grams
• relative formula mass
Moles = Mass M r