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Page 1: Percent Composition AKA “Mass Percent” AKA “Mass Percent” AKA “Percent by Mass” AKA “Percent by Mass” Component Mass Component Mass Total Mass Example:

Percent CompositionPercent Composition AKA “Mass Percent”AKA “Mass Percent” AKA “Percent by Mass”AKA “Percent by Mass” Component Mass Component Mass

Total MassTotal Mass

Example: Example: CC22HH44OO22

2(12.01 g/mol) = 24.02 g/mol2(12.01 g/mol) = 24.02 g/mol Mass CMass C4( 1.01 g/mol) = 4.04 g/mol 4( 1.01 g/mol) = 4.04 g/mol Mass HMass H++ 2(16.00 g/mol)2(16.00 g/mol) = 32.00 g/mol = 32.00 g/mol Mass OMass O 60.06 g/mol60.06 g/mol Mass CMass C22HH44OO22

X 100%X 100%

Page 2: Percent Composition AKA “Mass Percent” AKA “Mass Percent” AKA “Percent by Mass” AKA “Percent by Mass” Component Mass Component Mass Total Mass Example:

% Composition % Composition

% C % C

% H% H

% O% O

Total = 100.00% Total = 100.00%

%100g/mol 60.06g/mol 02.24

%100Mass Total

MassComponent

100% g/mol 60.06g/mol 4.04

100% g/mol 60.06g/mol 32.00

39.99% 39.99% CC

53.28% 53.28% OO

6.73% H6.73% H

Page 3: Percent Composition AKA “Mass Percent” AKA “Mass Percent” AKA “Percent by Mass” AKA “Percent by Mass” Component Mass Component Mass Total Mass Example:

Practice:Practice:What is the percent composition for each What is the percent composition for each component in sodium carbonate, Nacomponent in sodium carbonate, Na22COCO33??

2(22.99 g/mol) = 45.98 g/mol2(22.99 g/mol) = 45.98 g/molNaNa

12.01 g/mol = 12.01 g/mol12.01 g/mol = 12.01 g/molCC+ 3(16.00 g/mol)+ 3(16.00 g/mol) = 48.00 g/mol = 48.00 g/molOO

105.99 g/mol Na105.99 g/mol Na22COCO33

Page 4: Percent Composition AKA “Mass Percent” AKA “Mass Percent” AKA “Percent by Mass” AKA “Percent by Mass” Component Mass Component Mass Total Mass Example:

Na:Na:

C:C:

O:O:

Total = Total = 100.00%100.00%

%100g/mol 105.99g/mol 98.45

%100g/mol 105.99

g/mol 2.011

%100g/mol 105.99g/mol 48.00

43.38% Na43.38% Na

45.29% O45.29% O

11.33% C11.33% C

Page 5: Percent Composition AKA “Mass Percent” AKA “Mass Percent” AKA “Percent by Mass” AKA “Percent by Mass” Component Mass Component Mass Total Mass Example:

Converting Mass Percent to an Converting Mass Percent to an Empirical Formula (Mole Ratio)Empirical Formula (Mole Ratio)

Determine the empirical formula of a Determine the empirical formula of a compound that contains 58.84% Barium, compound that contains 58.84% Barium, 13.74% Sulfur and 27.43% Oxygen.13.74% Sulfur and 27.43% Oxygen.

Assume 100 gAssume 100 g

58.84% Ba58.84% Ba 58.84 g Ba58.84 g Ba13.74% S13.74% S 13.74 g S13.74 g S27.43% O27.43% O 27.43 g O27.43 g O

Page 6: Percent Composition AKA “Mass Percent” AKA “Mass Percent” AKA “Percent by Mass” AKA “Percent by Mass” Component Mass Component Mass Total Mass Example:

Ba mol 0.4285 g 137.32

mol 1 g 58.84 :Ba

S mol 0.4286 g 32.06

mol 1 g 13.74 :S

O mol 1.714 g 16.00

mol 1 g 27.43 :O

Did somebody ask for a mole?

Page 7: Percent Composition AKA “Mass Percent” AKA “Mass Percent” AKA “Percent by Mass” AKA “Percent by Mass” Component Mass Component Mass Total Mass Example:

Ba : S : OBa : S : O0.4285 mol0.4285 mol : : 0.4286 mol0.4286 mol : : 1.714 mol1.714 mol 0.4285 mol 0.4285 mol 0.4285 0.4285 mol 0.4285 mol 0.4285

mol mol

1.000 : 1.000 : 4.0001.000 : 1.000 : 4.000

BaSOBaSO44

Barium SulfateBarium Sulfate


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