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The Mole , Ch. 10 You need a calculator from this chapter on. *The mole was invented as a way to describe number of atoms. *1 mole = 6.02 x 10 23 things. 602,000,000,000,000,000,000,000 things. What if you had a mole of $1 bills?.

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The mole ch 10 you need a calculator from this chapter on

The Mole, Ch. 10You need a calculator from this chapter on.






Converting moles to of particles
*Converting moles to # of particles

  • Convert 3 moles of aluminum to number of atoms of aluminum.

  • Convert 7 moles of methane to molecules of methane.


Molar mass
*Molar Mass

  • One mole of an atom will weigh ___ grams (shown on the periodic table).


Convert moles to grams
*Convert moles to grams

  • Mg. 1 mole  ? grams

  • 6.94 grams



  • 2.5 x 1022 atoms of Na  grams Na?

  • .96 grams




Try it
Try it:

  • 6 moles of H2O to grams.

  • 126 g of NaF to moles.

  • 108 grams, 3 moles







  • STP 0 C, pressure = 1 atm (101.3 kPa)


Gas density
Gas Density:

  • Often is measured in g/L.

  • What is the density of H2 gas at STP?

  • .089 g/L



  • Page 303, roadmap.

  • Try: 55 E23 particles of He to volume of gas. Try: 55 E23 particles of He to grams of gas.




Percent composition
Percent Composition

  • Is the percent by mass of each element in the compound.






Determining empirical formula
*Determining Empirical Formula: ratio.

  • 25.9% N

  • 74.1 % O

  • Assume 100 g of the compound, find the # of moles, then find the whole number ratio.

  • Answer = 2 mol N, 5 mol O




Gas chromotography
Gas Chromotography the empirical formula.


Uses for gas chromotography
Uses for Gas Chromotography the empirical formula.


The end
The end the empirical formula.


Assignment
Assignment the empirical formula.

  • Draw and explain with words:

  • If you could have a mole of anything, what would you want and why?

  • Can be creative and funny.


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