6.02 X 1023 Avogadro’s Number.

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Presentation transcript:

6.02 X 1023 Avogadro’s Number

6.02 X 1023 1 Mole

3.01 X 1023 0.5 Mole

1.50 X 1023 0.25 Mole

12.04 X 1023 Or 1.204 X 1024 2.0 Mole

22.4 Liters 1.0 Mole of any gas at STP

Standard Temperature = 0C Standard Pressure = 1 atm STP

11.2 Liters 0.5 mole of any gas

44.8 Liters 2.0 mole of any gas

67.2 Liters 3.0 mole of any gas

5.6 Liters 0.25 mole of any gas

Sum of the masses of the elements in the compound Formula Mass

Formula Mass of H2O 2 X H = 2 X 1.0 = 2.0 1 X O = 1 X 16.0 = 16.0 Sum = 18.0 Formula Mass of H2O

Formula Mass of NH3 3 X H = 3 X 1.0 = 3.0 1 X N = 1 X 14.0 = 14.0 Sum = 17.0 Formula Mass of NH3

Formula Mass of CO2 1 X C = 1 X 12.0 = 12.0 2 X O = 2 X 16.0 = 32.0 Sum = 44.0 Formula Mass of CO2

Count up the atoms in (NH4)2SO4 For Paren: SubInside X Suboutside N: 2 S: 1 H: 8 O: 4 Count up the atoms in (NH4)2SO4

Count up the atoms in 2Mg3(PO4)2 For Paren: SubInside X Suboutside Coefficients X subs in formula Mg: 6 P: 4 O: 16 Count up the atoms in 2Mg3(PO4)2

MOLE MAP # of Grams # of Moles # of Particles # of Liters (gas)  by formula mass X Formula Mass # of Moles X 22.4 L/mole by 6.02 X 1023  by 22.4 X 6.02 X 1023 # of Particles # of Liters (gas)

Part X 100% Whole Percent

Part X 100% = 2 X 100% Whole 18 Percent H in H2O

Part X 100% = 16 X 100% Whole 18 Percent O in H2O

smallest whole number ratio of the elements in a compound Empirical Formula

Gives exact composition of molecule Molecular Formula

Formula contains all nonmetals Covalent Compound

Formula contains metal plus nonmetal Ionic Compound

CuSO4•5H2O Formula of a hydrated salt. • means “is associated with.” H2O molecules are stuffed in the empty spaces. CuSO4•5H2O

Formula mass of CuSO4•5H2O Mass of CuSO4 plus mass of 5 water molecules. 249.6 grams/mole Formula mass of CuSO4•5H2O

Part X 100% = 90 X 100% Whole 249.6 Percent H2O in CuSO4•5H2O

All elements to the left of the staircase except H Metals

All elements to the right of the staircase plus H Nonmetals

Compound made from 2 elements Binary Compound

Which formulas are empirical? H2O H2O2 CH4 C2H6 C6H12O6 KCl P4O10 CaF2 Which formulas are empirical?

Given empirical formula & Formula Mass, find Molecular Formula Find empirical mass Divide formula mass/empirical mass Multiply subscripts in empirical formula by answer in step 2 Given empirical formula & Formula Mass, find Molecular Formula

Empirical formula = CH & Formula Mass = 78, find Molecular Formula Empirical mass = 13 Divide formula mass/empirical mass = 78/13 = 6 Multiply subscripts: C6H6 Empirical formula = CH & Formula Mass = 78, find Molecular Formula

Mass of H2O = 12 – 8 = 4 g Percent H2O = 4/12 X 100% Percent salt = 8/12 X 100% 12 grams of hydrated salt is heated. After heating the mass is 8.0 grams. What is the percent salt & the percent H2O?

1 atom of He or 1 mole of He 1 atom per molecule

1 molecule of O2 or 1 mole of O2 2 atoms per molecule

1 molecule of O3 or 1 mole of O3 3 atoms per molecule