Ch. 3 Chem. 107 Notes
Ch. 3 Chem. 107 Notes CHEM 107
University of Louisiana at Lafayette
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This 2 page Class Notes was uploaded by Kalia Notetaker on Thursday February 11, 2016. The Class Notes belongs to CHEM 107 at University of Louisiana at Lafayette taught by Richard Perkins in Spring 2016. Since its upload, it has received 23 views. For similar materials see General Chemistry I in Chemistry at University of Louisiana at Lafayette.
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Date Created: 02/11/16
Ch. 3 Notes “Stoichiometry” Atomic mass – sometimes called atomic weight - ,ass of an atom in atomic mass units (amu) o Amu = 1/12 the mass of one carbon-12 atom aka Dalton (Da) o Average atomic mass – what we refer to because there is always a mixture of isotopes Avogadro’s number – actual number of atoms in 12g of carbon-12 (N ) =A 6.0221415 x 10 round to 6.022 x 10 = 1 mol 12g = about 1/2 an ounce o Mole (mol) – amount of a substance that contains as many elementary entities (atoms, molecules, or other particles) as there are atoms in exactly 12g (or 0.012 kg) of the carbon-12 isotope *A Unit to count # of particles * ex. dozen=12 pair=2 o Molar mass – mass (grams or kilograms) of 1 mole of units of a substance g/mol is equal to atom’s atomic mass Molecular mass – molecular weight , sum of the atomic mass (in amu) in a molecule o Molecular mass (amu) = molar mass (grams) o Ex: 1 molecule SO 2 64.07 amu 1 mole = 64.07 g Formula mass – sum of the atomic masses (in amu) in a formula unit of an ionic compound o same as molecular, as up atomic masses formula mass = molar mass Percent composition – element in a compound = n x molar mass of element / molar mass of compound x 100% o N is the 3 of moles of the element in 1 mole of the compound Chemical reaction – process in which one or more substances is changed into one or more new substances Chemical equation – uses chemical symbols to show what happens during a chemical reaction o Reactants Products o Balancing chem. Equation by writing reactant on left side and product on right side, then change the numbers in front of the formulas (coefficients) to make the # of atoms of each element the same on both sides – don’t change subscripts Check to make sure you have some number of atoms on each side Method – balancing by inspection Reaction yield - # of grams you get o Theoretical – amount of product that would result if all the limiting reagent reacted (aka calculated yield) o Actual yield – amount of product actually obtained from a reaction o Percentage – proportion of the actual yield to the theoretical yield times 100
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