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Empirical formula

AP Chemistry Zumdahl 7E Chapter 3 Notes

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Chemistry
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Stoichiometry
Chemical properties
Mass
Amount of substance
Chemical reactions
Yield
Mole
Limiting reagent
Atomic mass
Empirical formula
Molar mass
Chemistry

AP Chemistry A. Allan Chapter 3 Notes - Stoichiometry 3.1 Atomic Masses A. C-12, the Relative Standard 1. C-12 is assigned a mass of exactly 12 atomic mass units (amu) 2. Masses of all elements are determined in comparison to the carbon - 12 atom (12C) the most common isotope of carbon 3. Comparisons are made using a mass spectrometer B. Atomic Mass (Average atomic mass, atomic weight) 1. Atomic masses are the average of the naturally occurring isotopes of an element 2. Atomic mass does not represent the mass of any actual atom 3. Atomic mass can be used to "weigh out" large numbers of atoms 3.2 The Mole A. Avogadro's number 1. 6.022 x 1023 units = 1 mole 2. Named in honor of Avogadro (he did NOT discover it) B. Measuring moles

Percent composition and mole conversions pt 2 - Notes

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Mole fraction

Percent Composition PURPOSE and PROCEDURE To find out the percentage (by mass) of a particular element in a chemical compound. Calculate the molar mass for the compound. Divide the mass of the element you want to find the percentage of by the molar mass of the compound. Write the answer you get from step B in percentage form. Round your percentage to the tenth. EXAMPLES What percent of Cu2O is O? 2 x Cu = 2 x 63.5 = 127.0 g 1 x O = 1 x 16.0 = 16.0 g molar mass = 143.0 grams/mol % O = Part ? Total = 16.0 ? 143 = .1118 x 100% = 11.2% Example What percent of Al2O3 is Al? 2 x Al = 2 x 27.0 = 54.0 g 3 x O = 3 x 16.0 = 48.0 g molar mass = 102.0 grams/mole % Al = Part ? Total = 54 ? 102 = .5294 x 100% = 52.9% Practice - Find the percent composition

Principles of Chemistry I Chapter 3

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Analytical chemistry
Empirical formula
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Mole
Molar mass
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C18H37NO2
C10H12O4

Chapter 3 ? Stoichiometry this term refers to mass relationships and changes during a chemical reaction. Mass is conserved, but atoms in product are arranged differently than they are reactants. I) Mole ? A) molecules composed of atoms in definite proportion by mass and in specific ratio: butyric acid has 54.5% C, 36.4% O and 9.1 % H it also has the atoms C/H/O in the ratio 2/4/1 B) Mole is used as a measure of the amount of a substance. 1 mole is the number of 126C atoms in 12.00 g Notice it relates number of atoms to mass of those atoms in grams. It is always 6.02 x 1023 So 6.02 x 1023 atoms of 12C weigh 12.00 g Instead of looking at masses of isotopes, can use average atomic mass of atoms: Find Se on periodic table
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