Chem 107, ch 3
Chem 107, ch 3 Chem 107
University of Louisiana at Lafayette
Popular in General Chemistry I
Popular in Chemistry
This 2 page Class Notes was uploaded by Alexandra Notetaker on Wednesday October 5, 2016. The Class Notes belongs to Chem 107 at University of Louisiana at Lafayette taught by Dr. Daniel Rivera in Fall 2016. Since its upload, it has received 4 views. For similar materials see General Chemistry I in Chemistry at University of Louisiana at Lafayette.
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Date Created: 10/05/16
Chemistry notes Stoichiometry Atomic mass units are used to measure the weight of elements and compounds o One AMU is defined as I/12 the mass of a carbon 12 atom o Carbon 12 is exactly 12 AMU Atomic mass is defined as the weighted average mass of all of the isotopes of that element o Depends on the natural abundance of each particular isotope Molecular mass- also called the molar mass is the sum of the atomic masses in a particular molecule o Molecule is the smallest unit of a molecular substance and a mole is Avogadro’s number 23 6.02 X 10 Mass spectrometer- device that helps figure out the relative atomic masses of the imputed substances Percent composition- defined as the molar mass of the element (n) / molar mass of the compound o N is the number of moles of that element Chemical reactions- a reaction where the reactants are chemically changed to form a product(s) o Chemical equations must be balanced Only the subscripts can be changed when balancing equations o Chemical reactions are portrayed by having reactant (+) reaction -> product (+) product Stoichiometry is the quantitative study of the reactants and products formed in a chemical reaction The mole method establishes the coefficients in a chemical equation o They represent the moles of substance o The mole ratio is between the number of moles of an two substances involved in a chemical reaction The general steps for performing stoichiometric problems is Mass of A> moles of A> to moles of B> to mass of B Limiting reagents:the amount of product limits the amount of reagents there were to being with o It limits the amount of product that can form o If you have 4 moles of Na and 2 moles of Cl you can only make 2 moles of NaCl because Cl limits that reaction o In the same instance Na is the excess reactant Reaction yield: amount of products determined by how much the actual yield produced divided by the theoretical yield times 100% Scientist can see how efficient the reaction was based upon the percentage yield that that particular reaction produced
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