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


  • *The mole was invented as a way to describe number of atoms.


  • *1 mole = 6.02 x 1023 things.

  • 602,000,000,000,000,000,000,000 things.


What if you had a mole of $1 bills?


  • In a mole of water, there are 6.02 x 1023 molecules of H2O.

  • Pass around 1 mole of water.


*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

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


*Convert moles to grams

  • Mg. 1 mole  ? grams

  • 6.94 grams


  • 3 moles Be  ? grams

  • 27 grams.


  • 2.5 x 1022 atoms of Na  grams Na?

  • .96 grams


  • 3 moles of CH4 to grams?

  • 48 grams.


  • 4 moles of HF to grams?

  • 80 grams


Try it:

  • 6 moles of H2O to grams.

  • 126 g of NaF to moles.

  • 108 grams, 3 moles


  • Molar mass of Uranium a ball of uranium with a radius of 1.3 inches weighs a pound.


  • *A mole of any gas takes up 22.4 L (at STP). This is Avogadro’s Hypothesis.

  • This is like a cube with sides of 28.2 cm.


  • One mole of He, H, O, N, etc. will all take up 22.4 L.

  • Question: How many He atoms are there in 22.4 L?

  • Question: How many H2 molecules are there in 22.4 L?


  • How many moles of O2 in 44.8 liters of O2?


  • How many L in 4 moles of N2?

  • 89.6 L


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


Gas Density:

  • Often is measured in g/L.

  • What is the density of H2 gas at STP?

  • .089 g/L


  • Gas density


  • Page 303, roadmap.

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


  • Be able to solve mole problems.

  • Compare a mole of eggs to a dozen eggs.

  • What is a mole useful for?


  • *Gas density to molar mass.

  • Exp: 2.86 g/L.


Percent Composition

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


  • *Percent Composition from mass data:

  • 5.4 g of oxygen and 8.2 g of magnesium in a 13.6 gram compound.

  • 60.3% Mg, 39.7% O


  • *Percent composition from the chemical formula Find the amount of grams of each element in 1 mole of the compound, then find the %.

  • C3H8

  • 81.8% C, 18% H


  • How many grams of O are present in 36 grams of H2O?

  • 32 grams O


  • *Empirical formula: Expresses the atoms in their lowest ratio.

  • *Molecular formula: Expresses the atoms in their actual abundance.

  • Exp: H2O2 HO


*Determining Empirical Formula:

  • 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


  • The molecular formula is always a whole number multiple of the empirical formula.


  • Empirical formula to Molecular formula If the empirical formula is CH4N and the molecular molar mass is 60 g/mol, what is the molecular formula?

  • C2H8N2


Gas Chromotography


Uses for Gas Chromotography


The end


Assignment

  • 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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