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Chemistry 110 Chapter 5

by: Mikaela Notetaker

Chemistry 110 Chapter 5 CHEM 110

Marketplace > West Virginia University > Chemistry > CHEM 110 > Chemistry 110 Chapter 5
Mikaela Notetaker

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About this Document

Covers Molarity, density, molar mass, etc.
Introduction to Chemistry
Melissa G. Ely
Class Notes
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This 5 page Class Notes was uploaded by Mikaela Notetaker on Sunday March 13, 2016. The Class Notes belongs to CHEM 110 at West Virginia University taught by Melissa G. Ely in Spring 2016. Since its upload, it has received 15 views. For similar materials see Introduction to Chemistry in Chemistry at West Virginia University.


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Date Created: 03/13/16
Chapter 5 SI system: international system of units based upon the metric system scientific community has agreed to use these units for papers, etc. Measurements SI Mass Kg Length m Time sec(s) Temperature K (kelvin) Amount of solution mole (or mol) Mole: amount of a chemical substance 1. A counting unit term a. 1 dozen = 12 b. 1 case = 24 23 c. 1 mole = 6.0221 x 10 particles (atoms, molecules, formula units) 2. We work with miles because the amount of chemicals worked with in the lab are large scaled amounts. It’s a pain to work with large exponential numbers so convert to counting unit of mole and then numbers are nicer and closer to one. 23 3. Avogadro’s number = N =6.0A21 x 10 particles/mole a. Macroscale: moles, grams, molar mass b. Microscale: atoms, molecules, formula i. To convert macro to micro, and vice versa, use Avogadro’s number. A. 2.0 moles CH -> molecules 4 23 24 a. 2.0 moles CH 4 6.0221 x 10 molecules = 1.2 x 10 molecules 1 mole CH 4 B. 2.0 moles CH ->4Atoms 23 a. 2.0 moles CH 4 6.0221 x 10 molecules CH 4 (1 C + 4 H) 5 atoms CH 4 = 6.0 x 10 24 1 mole CH 4 1 molecule CH 4 atoms CH 4 C. 0.543 mol CaCl ->2Formula Units (f.u.) 23 23 a. 0.543 moles CaCl 2 6.0221 x 10 f.u. CaCl2= 3.27 x 10 f.u. CaCl2 1 mole CaCl 2 D. 9.81 x 10 21molecules Cl -> moles Cl 21 2 2 a. 9.81 x 10 molecules Cl 2 1 mole Cl 2 = 0.0163 mole Cl 2 6.0221 x 10 23 molecules Note: Ions are the same as atoms. Molar Mass: Mass of 1 mole of a substance. 1. Atomic mass: molar mass of element. a. Given as a non-integer number below the element on the periodic table i. Atomic mass Ga = 69.72 amu or 69.72 g/mol 2. Molecular mass: molar mass of molecular compound 3. Formula mass: molar mass of an ionic compound. A. 3.0 mol Ga -> g Ga (molar mass) a. 3.0 moles Ga 69.72 g Ga = 209 = 2.1 x 10 g Ga2 1 mole Ga B. 15 g Ga -> mole Ga b. 15 grams Ga1 mole Ga = .22 mole Ga 69.72 g Ga C. 17.32 g S -> atoms S c. 17.32 g S 1 molecule S 6.0221 x 10 23atoms S = 3.252 x 10 23atoms 32.07 g S 1 molecule S D. 0.75 mol Ba (P3 ) 4 2g Ba (PO 3 4 2 a. Molar Mass: i. Ba -> 3 x 137.33 g = 411.99g ii. P -> 2 x 30.97 g = 61.94g iii. O -> 8 x 16.00 g = +128.00g iv. 601.93g/mol 2 d. 0.75 mol Ba (3O )4 2 601.93 g/mol = 4.5 x 10 g Ba (PO )3 4 2 1 mol Ba (3O )4 2 E. 13.32 g CH ->4mol CH 4 a. Molar Mass: i. C -> 1 x 12.01 g = 12.01g ii. H -> 4 x 1.008 g= + 4.032g iii. 16.04(2)g e. 13.32 g CH 4 1 mol = 0.8303 mol CH 4 16.04(2) g CH 4 Density = Mass of substance / Volume of substance Units = g/mL, g/cm , g/L for gases  The higher the density the bigger a substances percent value  As temperature increases density decreases (except H O) 2  Density should be on your conversion sheet Substance Density o H 2 (L) 1,000 (at 4 C) H 2 (s) 0.917 Fat .94 Hg(L) 13 Ice and fat will float on liquid water because it is less dense. Mercury will sink. Use density to convert mass to volume 3 A. 25 g Ag -> volume, density = 10.50 g/cm Ag f. 25 g Ag 1 cm 3 = 2.4 cm Ag 3 10.50 g Ag 3 B. 5.0 cm Pb -> g Pb, Den = 11.35 g/cm Pb g. 5.0 cm Pb 11.35 g Pb = 57 g Pb 1 cm Pb Gas Volume: at same temp. and pressure equal volume of gas contain the same number of gas partials and thus the same number of mols of gas. I mean that the volume of gas is independent of identity of gas and only depends on how much gas is present. Under STP (Standard Temp Pressure) T = 0 C, P = 1 atom -> 1 mole gas occupies 22.4 L independent gas identity. Only for gases at STP -> 1 mol = 22.4 L (Standard Molar gas volume, not solid or liquids) Concentration: used to specify the amount of a substance dissolved in a volume (mL or L) of solution. Solute- substance dissolved Solvent- substance that dissolves solute Solution- the solute + solvent Concenstration = Mass solute / Volume Solution Units = g/mL, g/L


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