CHEM 1001 1st Edition Lecture 6Outline of Last Lecture I. The Father of Modern Chemistry a. Antoine Lavoisier II. Chemical equations a. Balancing equations III. Patterns of Chemical Reactivity a. Combination reactionsb. Decomposition reactionc. Combustion reaction IV. Formula Weights and MassOutline of Current Lecture I. Mole a. Molar Massb. Formula mass II. Empirical Formulas III. StoichiometryThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.a. ConversionsIV. Limiting Reactants b. Theoretical yield c. Percent yield Current LectureI. Mole a. Molar mass = M – the mass in grams of 1 mole of substance (atoms, molecules, ions or formula unitsb. Formula mass- in (amu) and molar mass (in grams) are the same number II. Determining Empirical Formulas a. Ratio of moles = ratio of atoms b. % -> gram -> mol -> divide each element by the smallest value to get a number for the chemical equation i. Molecular formula 1. # you multiply the numbers from the empirical formula =molecualr weight (typically given)empirical FWIII. Stoichiometrya. Stoichiometry – the quantitative study of the reactants and products of a chemical reaction i. Nearly all stoichiometry problems involve figuring out the relationship between two or more of your reactants. But, often both the data and results are masses IV. Limiting reactants in reactions a. Limiting reactions: reactants that makes the least amount of productb. Theoretical yield: amount of product that can be made into a chemical reaction based on the limiting reaction c. Percent Yield = actual yeild (typically given)theoretical yield x
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