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Using Chemical Formulas Chapter 7.3
Objectives Calculate the formula mass or molar mass of any given compound. Use molar mass to convert between mass in grams and amount in moles of a chemical compound. Calculate the number of molecules, formula units, or ions in a given molar amount of a chemical compound. Calculate the percentage composition of a given chemical compound.
Formula Masses Defined as:  of any molecule, formula unit, or ion is the sum of the average atomic masses of all the atoms represented. ,[object Object],K	1     x     39.10  amu     =   Cl	1     x     35.45   amu    = O	3     x     16.00  amu     =               _                    39.10 amu 35.45 amu 48.00 amu 122.55 amu ,[object Object],  2.02 amu H	2     x     1.01  amu       =   S	1     x     32.07   amu    = O	4     x     16.00  amu     =               _                    32.07 amu 64.00 amu 98.09 amu
Molar Mass Defined as:  mass in grams of one mole, or approximately  6.022 x 1023 particles. ,[object Object]
Formula mass is the mass of one atom
Although different meaning :
Molar mass and formula mass are numerically equal
Find the molar  mass of barium nitrate, Ba(NO3)2.137.33 g/mol Ba	1     x    137.33  g/mol     =   N	2     x     14.01  g/mol     = O	6     x     16.00  g/mol     =               _                    28.01 g/mol 96.00 g/mol 261.35 g/mol ,[object Object],Answers: 150.17 g/mol Al2S3 B)   Ba(OH)2 B)   171.35 g/mol
Molar Mass as a conversion Amount of compound  (moles) Mass of a compound (grams) Number of molecules or formula units  Molar mass 6.02 x 1023 ÷ x  6.02 x 10 23  Molar mass ÷ x

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Chapter 7.3 : Using Chemical Formulas

  • 2. Objectives Calculate the formula mass or molar mass of any given compound. Use molar mass to convert between mass in grams and amount in moles of a chemical compound. Calculate the number of molecules, formula units, or ions in a given molar amount of a chemical compound. Calculate the percentage composition of a given chemical compound.
  • 3.
  • 4.
  • 5. Formula mass is the mass of one atom
  • 7. Molar mass and formula mass are numerically equal
  • 8.
  • 9. Molar Mass as a conversion Amount of compound (moles) Mass of a compound (grams) Number of molecules or formula units Molar mass 6.02 x 1023 ÷ x 6.02 x 10 23 Molar mass ÷ x
  • 10.
  • 11. How many molecules of ibuprofen are in the bottle? 6.022 x 1023 molecules o.16 mol = 9.6 x 1022 molecules X 1 mol More Practice problems How many moles of the compound are there in 6.60 g (NH4)2SO4? How many molecules are there in 25.0 g H2SO4? What is the mass in grams of 6.25 mol of copper(II) nitrate Answer: 0.0500 mol Answer: 1.53 x 1023 molecules Answer: 1170 g
  • 12. Percentage composition Useful in determining the percent by mass of each element in a compound 1. Find the percent composition of copper(I) sulfide, Cu2 S. First: find the total molar mass Cu 2 x 63.55 g = 127.1 g Cu S 1 x 32.07 g = 32.07 g S 159.2 g Cu2S Second: find the percent of each 127.1 g Cu X 100 = 79.84 % Cu 159.2 g Cu2S 32.07 g S X 100 = 20.14 % S 159.2 g Cu2S
  • 13. More Practice: percent composition Find the mass percentage of water in sodium carbonate decahydrate, Na2CO3 10H2O, which as a molar mass of 286.14 g/mol. Find the percentage composition of PbCl2 Ba(NO3)2 10 mol H2O x 18.02 g H2O 1 mol H2O = 180.2 g H2O 180.2 g H2O x 100 = 62.98 % 286.14 g Na2CO3 10 H2O Answer: 74.51 % Pb, 25.49 % Cl Answer: 52.55 % Ba, 10.72 % N, 36.73 % O