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The Mole

The Mole. Too small to see. Because atoms are so small , it makes more sense to measure large amounts of atoms in reactions . One mole of a substance contains the same number of particles as atoms in 12 grams of Carbon-12. The Avagadro Constant.

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The Mole

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  1. The Mole

  2. Toosmalltosee • Becauseatoms are so small, itmakes more sensetomeasurelargeamounts of atoms in reactions. • One mole of a substancecontainsthesamenumber of particles as atoms in 12 grams of Carbon-12

  3. TheAvagadroConstant • 1 mole of a substancecontains 6.022 x 1023particles • Thats 602 200 000 000 000 000 000 000 particles!!!

  4. Equation • Tocalculatethe moles in a substancewe use thefollowingequation: • Moles of Atoms = Mass/RelativeAtomicMass

  5. R.A.M. • RelativeAtomicMassisthe Ar valuefromthePeriodicTable

  6. Question • Howmany moles of atoms are there in 2.4 g of carbon?

  7. Answer • Moles of atoms = mass/R.A.M. • = 2.4/12 = 0.2 moles

  8. TheMagicTriangle • Usingthemagictrianglewe can rearrangetheequationtofindmassinstead of moles

  9. Question • Whatisthemass of 0.1 moles of CarbonAtoms?

  10. For a compound • A compound has more thanonetype of atom, so wehavetofindtheRelative Formula Mass (R.F.M.) • We do thisbyaddingthe Ar of theelements in themolecule. • So theequationthenbecomes: • Moles = Mass/R.F.M.

  11. Question • Howmany moles are there in 8 g of copper(II) oxide (formula CuO)? • 1. Findthe RFM Cu = 64 O = 16 So the RFM of CuOis 80 ….thenjustfollowtheequation…

  12. Questions • Howmany moles of atoms are there in: • 2 g of hydrogen • 36 g of carbon • 160 g of oxygen • 14 g of nitrogen • 0.19 g of flourine

  13. Questions • Howmany moles of molecules are there in: • 26 g of H2O • 170 g of NH3 • 1.6 g of CH4 • O.2 g of C2H6 • 16 g of NH4NO3

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