Price Review


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CHEMISTRY 1031 (PRICE) – INFORMATION FOR EXAM II WEDNESDAY, MARCH 26 TH , 8:30 – 9:30 am, BE 160 Exam II will cover the material I lectured on from chapters 4, 5, and part of 6. There will be about 25 multiple choice questions worth a total of 90 points and 20 points-worth of longer problems/short answer questions. This totals 110 points, but your exam score will be out of 100 points, i.e., there are 10 bonus points! The following study guide and suggested problems should help you prepare for the exam. In addition, you should try the practice exam questions that appear at the end of this document. Note that the exam will start at 8:30 am prompt, so as to give you 10 minutes more than last time. Chapter 4 Sections 4.1, 4.2: You should be able to calculate molecular mass (sometimes called molar mass, or formula mass) of a compound given its chemical formula and atomic masses of the elements. Know what is meant by a mole and Avodagro’s number (6.02 x 10 23 mol –1 ) and convert from mass to moles to number of atoms/molecules and vice versa . Try Practice Exercises 2 – 9 (within the chapters). Section 4.3: Given the mole-to-mole conversion factor in a compound or chemical reaction, you can calculate moles and/or grams of an element given the mass of another. Try Practice Exercises 10 – 12. Section 4.4: Be able to calculate percentage by mass of an element in a compound given the grams of each element in the compound (try Practice Exercise 13) or from the chemical formula and the atomic masses (try Practice Exercise 14). Given the mass of each element in a compound (or the percent mass of each element) you can determine the empirical formula of the compound (try Practice Exercises 15, 16, 17). Using combustion analysis data (usually for organic compounds which burn in O 2 to give CO 2 and H 2 O), you can use the mass of CO 2 and H 2 O obtained to determine the empirical formula (try Practice Exercise 18). Given the molar mass, you can divide this by the empirical molar mass to get a whole number which you can use to get the actual chemical formula (try Practice Exercise 19). Sections 4.5, 4.6: Given a balanced chemical equation (try Practice Exercise 23), you should be able to calculate grams (or moles) of a product (or reactant) given the grams (or moles) of another product (or reactant). Remember: grams A moles A moles B grams B (figure 4.4). Try Practice Exercises 20 – 22. Section 4.7: Given the mole ratio of reactants in a balanced chemical equation, you should be able to determine which one is the limiting reactant (LR) and which is in excess (INXS). There are several methods. I showed in class how you can compare the mole ratios of reactants from the equation (moles required) with the mole ratios given, and use these ratios to determine the LR and the reactant INXS. Alternatively, you can calculate the moles (or mass) of one of the products from the mass of each of the
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