C2F2009 - CHEM 1331 Fall Semester 2009 Chemistry for...

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UH Department of Chemistry CHEM 1331 Professor Geanangel If you have an incomplete in CHEM 1331, print your name and PS number on my list today. Syllabus text readings define our course. Please read them BEFORE you come to class. 1 CHEM 1331 Fall Semester 2009 I nstructor: Prof. Geanangel Office: 123B-Fleming Please use Blackboard mail to contact me. Chemistry for Science and Engineering Majors BlackBoard : www.uh.edu/webct (Pass MPT soon!) Office Hours: MWF 1:00 - 2:00 pm Read your syllabus! Keep it for reference. 1 Sections 22990 MWF 10-11 AM 160F 22998 MWF 1-2 PM 160F UH Department of Chemistry CHEM 1331 Professor Geanangel CHEM 1331 Fall Semester 2009 Chapter 2: The Components of Matter 2.1 2.2 The Observations That Led to an Atomic View of Matter 2.3 Dalton’s Atomic Theory 2.4 The Observations That Led to the Nuclear Atom Model 2.5 The Atomic Theory Today 2.6 Elements: A First Look at the Periodic Table 2.7 Compounds: Introduction to Bonding 2.8 Compounds: Formulas, Names, and Masses 2.9 Mixtures: Classification and Separation 2
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UH Department of Chemistry CHEM 1331 Professor Geanangel 3 Observations that led to an atomic view of matter The total mass of substances does not change during chemical reactions. The number of substances may change, but the total amount of matter remains constant. Conservation of Mass (nothing gets lost) reactant 1 + reactant 2 product(s) total mass total mass = calcium oxide + carbon dioxide calcium carbonate CaO + CO 2 CaCO 3 56.08g + 44.00g 100.08g UH Department of Chemistry CHEM 1331 Professor Geanangel 4 Problem: When 0.2250 g Mg was heated with 0.5331 g N 2 (g), all the Mg was consumed forming 0.3114 g Mg 3 N 2 . What mass of N 2 is left over ? Mg(s) + N 2 (g) => Mg 3 N 2 (s) (unbalanced) Start 0.2250g 0.5331g 0 g End 0g x g 0.3114 g 0.3114 g - 0.2250 g (Mg) = 0.0864 g N 2 used x = 0.5331 g N 2 (start) - 0.0864 g N 2 (used) = 0.4467 g N 2 left
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UH Department of Chemistry CHEM 1331 Professor Geanangel 5 Definite Composition What’s in it and how much? A chemical compound is always composed of the same elements in the same fractions by mass . Experimental analysis of the elemental mass composition of 20.0 g calcium carbonate: Mass Analysis (grams/20.0 g) 8.0 g calcium 2.4 g carbon 9.6 g oxygen 20.0 g total Mass Fraction (parts/1.00 part) 0.40 calcium 0.12 carbon 0.48 oxygen 1.00 part by mass Percent by Mass (parts/100 parts) 40% calcium 12% carbon 48% oxygen 100% by mass UH Department of Chemistry CHEM 1331 Professor Geanangel 6 Mass of an Element X in a Compound Galena is a mineral consisting of Pb and S. A 1.27 g quantity of Galena contains 1.10 g of Pb. How many grams of S are present in a 1 kg sample of Galena ? mass of X in sample = mass fraction x mass of sample
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This note was uploaded on 03/01/2010 for the course BA 13213 taught by Professor Deez during the Spring '10 term at Aarhus Universitet, Aarhus.

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C2F2009 - CHEM 1331 Fall Semester 2009 Chemistry for...

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