Chem 141 Chapter 3

Chem 141 Chapter 3 - 3-1Chemistry 141Summer 2008Silberberg...

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Unformatted text preview: 3-1Chemistry 141Summer 2008Silberberg Chapter 3Dr. Ben Tovrog3-2Silberberg Chapter 3 Problem AssignmentThese problems are for your practice. They will not be collected or graded. Easy and Medium:3.1, 3.2, 3.6, 3.7, 3.8, 3.10, 3.12, 3.14, 3.18, 3.19, 3.20, 3.25, 3.27, 3.33, 3.37, 3.39,3.41, 3.44, 3.46, 3.51, 3.53, 3.55, 3.61, 3.63, 3.65, 3.67, 3.69, 3.71, 3.73, 3.75, 3.77,3.79, 3.83, 3.85, 3.92, 3.94, 3.96, 3.98, 3.102, 3.105, 3.116, 3.118, , 3.120, 3.124, 3.128Hard:3.137, 3.139, 3.142, 3.151, 3.1553-3Mole - Mass Relationships in Chemical Systems3.5Fundamentals of Solution Stoichiometry3.1The Mole3.2Determining the Formula of an Unknown Compound3.3Writing and Balancing Chemical Equations3.4Calculating the Amounts of Reactant and Product3-4mole(mol)- the amount of a substance that contains the same number of entities as there are atoms in exactly 12 g of carbon-12.This amount is 6.022x1023. The number is called Avogadros number and is abbreviated asN.One mole (1 mol) contains 6.022x1023entities (to four significant figures)3-512 red marbles @ 7g each = 84g12 yellow marbles @4g each=48g55.85g Fe = 6.022 x 1023atoms Fe32.07g S = 6.022 x 1023atoms SFigure 3.1Counting objects of fixed relative mass. 3-6Water18.02 gCaCO3100.09 gOxygen32.00 gCopper63.55 gOne mole of common substances.Figure 3.23-7Table 3.1 Summary of Mass TerminologyTermDefinitionUnitIsotopic massMass of an isotope of an elementamuAtomic massMolecular (or formula) mass (also called molecular weight)Molar mass (M)(also called atomic weight)(also called gram-molecular weight)amuamug/molAverageof the masses of the naturally occurring isotopes of an element weighted according to their abundanceSum of the atomic masses of the atoms (or ions) in a molecule (or formula unit)Mass of 1 mole of chemical entities (atoms, ions, molecules, formula units)3-8Information Contained in the Chemical Formula of Glucose C6H12O6( M = 180.16 g/mol)Oxygen (O)Mass/mole of compound6 atoms96.00 gTable 3.2Carbon (C)Hydrogen (H)Atoms/moleculeof compoundMoles of atoms/mole of compoundAtoms/mole ofcompoundMass/moleculeof compound6 atoms12 atoms6 moles of atoms12 moles of atoms 6 moles of atoms 6(6.022 x 1023) atoms 12(6.022 x 1023) atoms 6(6.022 x 1023) atoms6(12.01 amu) =72.06 amu12(1.008 amu) =12.10 amu6(16.00 amu) =96.00 amu72.06 g12.10 g3-9Interconverting Moles, Mass, and Number of Chemical EntitiesMass (g) = no. of moles x no. of grams1 molNo. of moles = mass (g) xno. of grams1 molNo. of entities = no. of moles x6.022x1023entities1 molNo. of moles = no. of entities x 6.022x1023entities1 molgM3-10Moles The Central ConceptShown for molecules. For atoms substitute atomic mass for molar massMoleMass (g)X molar massmolar massX 6.02 x 10 236.02 x 10 23Number of moleculesMolarity (mole/Liter)Volume(L)XVolume(L)Volume of Gas (L)X22.4 liters @STP 22.4 liters @STP3-11Mole ProblemsIn one dozen elephants, how many trunks are there? 12 How many legs? 48 How many methane molecules are there in one mole of methane? 6.022 E 23How many methane molecules are there in one mole of methane?...
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This note was uploaded on 07/30/2008 for the course CHEM 141 taught by Professor Mulfod during the Summer '08 term at Emory.

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Chem 141 Chapter 3 - 3-1Chemistry 141Summer 2008Silberberg...

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