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Quantities in Chemical Reactions
(4.1/4.5) Proportions in Compounds and Percentage
Composition
Law of Definite Proportions a specific compound always contains the same
elements in definite proportions by mass, regardless of how it is synthesized
compounds with the same mass proportions must be the same compound
the proportions are found by calculating the percent by mass.
Percent by Mass (percentage composition) based on the law of conservation of
mass
% by mass = MASSelement x 100% MASScompd
MASS compd = sum of MASSES elements
Percent by Mass
example: H2O
made up of 2 atoms of hydrogen and 1 atom of oxygen
to find percent by mass of each element:
H= (mass H / mass of water) x 100%O= (mass O / mass of water) x 100%
Percent by Mass of H2OMass % of H = mass of H (X2) X 100
mass of H2O
= 1.01u X 2 X 100 1.01u X 2 + 16.00
= 2.02u X 10018.02u
= 11.2%
Mass % of O = 100% - 11.2%= 88.8%
Practice ProblemsQ: A 78.0 g sample of an unknown
compound contains 12.4g of hydrogen. What is the percent by mass of hydrogen in the compound?
A: % Mass H = mass H x 100%
mass comp
= 12.4g x 100%
78.0g
= 15.9%
Practice ProblemsQ: How many grams of oxygen can be
produced from the decomposition of 100.0 g of KClO3?
A: % mass O = mass O x 100%
mass KClO3
= 3(16.00)u x 100%
[39.10+35.45+3(16.00)]u
= 39.17%
Practice ProblemsQ: How many grams of oxygen can be
produced from the decomposition of 100.0 g of KClO3?
A (continued):
mass O = %O x mass KClO3
= 0.3917 X 100.0g
= 39.17g
Practice ProblemsQ: Two unknown compounds are tested.
Compound 1 contains 15.0g of hydrogen and 120.0g oxygen. Compound 2 contains 2.0g of hydrogen and 32.0g oxygen. Are the compounds the same?
HINT!! If % Masses are equal , then they are the same
A: Compd 1-
%H = [15.0 / (15.0+120.0)] x 100%
= 11.1%
%O = [120.0 / (15.0+120.0)] x 100%
= 88.9%
Compd 2-
%H = [2.0 / (2.0+32.0)] x 100%
= 5.9%
%O = [32.0 / (2.0+32.0)] x 100%
= 94.1%
NOT THE SAME COMPOUNDS
HomeworkRead pg. 160 – 162 & pg. 178 - 184 Finish “Percent Composition Worksheet” pg. 184 “Section 4.5 Questions” #3 - 5