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by: Notetaker

CHEM 111 STUDY GUIDE EXAM #1 111/40551

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Everything from chapters 1 -3, answer key included
General Chemistry I
Study Guide
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This 8 page Study Guide was uploaded by Notetaker on Wednesday September 30, 2015. The Study Guide belongs to 111/40551 at University of St. Thomas taught by Uzcategui-White in Summer 2015. Since its upload, it has received 55 views.

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Date Created: 09/30/15
Chemistry Exam #1 Study Guide: Chapter 1: 1. Determine which kind of change occurs: chemical or physical a) Passing an electric current through molten magnesium chloride yields molten magnesium and gaseous chlorine. b) The iron in discarded automobiles slowly forms reddish brown, crumbly rust. c) Boiling canned soup d) Toasting a slice of bread e) Evaporating sweat 2. Which has higher kinetic energy? a) a sled resting at the top of a hill or a sled sliding down a hill b) water above a dam or water falling over the dam 3. The average radius of a molecule of lysosome is 1430. pm. What is its radius in cm? 4. A small hole in the wing of a space shuttle requires a 19.0 cm^2 patch. a) what is the patch’s area in km^2? b) if the patching material costs $2.76/ in^2, what is the cost of the patch? 5. The average density of a planet is 4.68 g/cm ^3. What is its density in kg/ m^3? 6. How many cubic meters of milk are in 7.65 qt (1 qt = 964.4 mL) ? 7. An empty vial weighs 58.47 g. If the vial weighs 259.50 when filled with liquid mercury (d = 13.53 g/cm^3), what is its volume? 8. Convert 177 F to C and K 9. How many significant figures in each number? a) 0.410 b) 0.0410 c) 0.04100 d) 4.01000 x 10^5 10. Perform the calculation with the right amount of sig figs 3.595 m x 6.10 m/ 4.28 m 11. “” 7.43 g/ 17.0 g – 8.44 g 12. “” (6.626 x 10^-34 J x s) (2.9979 x 10^8 m/s)/ 8.25 x 10^-7 m 13. which statements include exact numbers? a) 8 known planets in the solar system b) the volume of a soda in a can is 12 fluid ounces c) there are 1000 mm in 1 m d) there are 15 books on a shelf e) the height of the empire state building f) the number of seconds in a day 14. A pool is 49.0 m long and 28.0 m wide. How many mL of water are needed to fill the pool to an average depth of 6.30 ft? 15. Earth’s oceans have an average depth of 3800m, a total surface area of 3.63 x 10^8 km^2 and an average concentration of dissolved gold of 5.8x 10^-9 g/L. a) how many grams of gold are in the oceans? B) how many cubic meters? C) price of gold is $370.00/ troy oz, what is the value of gold in the oceans (1 troy oz= 31.1 g, d= 19.3 g/cm^3)? 16. Determine which of the following is a chemical or physical property. a) water boils at 100 C b) ultraviolet light converts 03 to 02 c) sodium metal is soft and can be cut with a knife d) chlorine is a green gas CHAPTER 2: 1. Classify each of the following substances as an element, compound or mixture. a) Calcium chloride, used to melt ice on roads, consists of 2 elements, calcium and chlorine in a fixed mass ratio. b) Sulfur consists of sulfur atoms combined into octatomic molecules c) Baking powder, a leavening agent, contains 26% to 30% sodium hydrogen carbonate and 30% to 50% calcium dihydrogen phosphate by mass. d) Cytosine, a component of DNA, consists of H, C, N and O atoms bonded in a specific arrangement. 2. State the mass law(s) demonstrated by the following experimental results (law of mass conservation, multiple proportions or definite composition). 1. A student heats 1.00 g of a blue compound and obtains .64 g of a white compound and .36 g of a colorless gas. 2. A second student heats 3.25 g of the same blue compound and obtains 2.08 g of a white compound and 1.17 g of a colorless gas. 3. Fluorite, a mineral of calcium, is a compound of the metal with fluorine. Analysis shows that a 24.71 g sample of fluorite contains 12.03 g of fluorine. Calculate: a) mass of calcium b) mass fractions of calcium and fluorine in fluorite c) mass percents of calcium and fluorine in fluorite. 4. A compound of cesium and iodine contains 81.86 g of metal and 78.03 g of nonmetal. How many grams of cesium are in a 71.76 g sample of the compound? How many grams of iodine? 5. Element X has two naturally occurring isotopes, 65 X (isotopic mass 64.8401 amu, abundance 60.63%) and 67X (isotopic mass 66.9272 amu, abundance 39.37%). Calculate the atomic mass of element X. 6. Which monatomic ions do the following form? a) Strontium (z= 38) b) Nitrogen (z=7) 7. An ionic compound forms when Lithium (z= 3) reacts with oxygen (z=8). If a sample of the compound contains 7.72 x 10^22 lithium ions, how many oxide ions does it contain? 8. Give the name and formula of the compound formed from the following elements: a) Cesium and nitrogen b) Beryllium and oxygen c) Aluminum and bromine 9. Give the name and formula formed from the elements 38L and 16M 10. Give the formula for lead (IV) iodide 11. Give the name for Mn2O3 12. Give the formula for potassium carbonate dehydrate 13. Give the formula for ammonium hydroxide 14. Give the name and formula of the compound whose molecules consist of 2 chlorine atoms and 5 oxygen atoms 15. Give the number of atoms and calculate the molar mass for Pb4SO4 (CO3)2 (OH)2 16. Give the formula for sodium hydrogen sulfate and determine its molar mass 17. In a reaction, 34.0 g of chromium (III) oxide reacts with 12.1 g of aluminum to produce chromium and aluminum oxide. If 23.3 g of chromium is produced, what mass of aluminum oxide is produced? Chapter 3: 1. How many grams of Ag are in .0342 mol of Ag? 2. How many Ga atoms in 2.85 x 10^-3 mol of Ga? 3. How many Fe atoms in 95.8 g of Fe? 4. How many O atoms in 7.3 x 10^-3 g of CaSO4 x 2H2O 5. What is the mass percent of Iodine in strontium perchlorate? 6. Convert into a balanced equation: Gallium metal heated in Oxygen gas forms solid gallium (III) oxide. 7. “” When Calcium chloride and sodium phosphate are mixed, solid calcium phosphate forms. 8. Calcium reacts as followed: 2Ca (s) + O2 (g)  2Ca) (s). Calculate the mass of calcium oxide that can be produced from 4.30 g Ca and 2.80g O2. a) What amount (mol) of CaO can be produced from the given mass of Ca? b) What amount (mol) of CaO can be produced from the given amount of O2? c) Which is the limiting reactant? d) How many grams of CaO can be produced? e) How many grams of the excess reactant remains? 9. What is the percent yield of a reaction where 45.5 g tungsten (IV) oxide (WO3) reacts with excess hydrogen gas to produce metallic tungsten and 9.60 mL of water? 10. Find the empirical formula for: a) .063 mols of chlorine atoms and 0.22 mols of oxygen atoms. b) 27.3 mass %C + 72.7 mass % O 11. Find the volume of 2.26 M potassium hydroxide that contains 8.42 g of solute. 12. How many grams of solid barium sulfate form when 35.0 mL of . 160 M barium chloride reacts with 58.0 mL of .065 M sodium sulfate? Aqueous sodium chloride also forms. 13. Write balanced equations for each of the following: a) ___ Cu + ___S8  ___Cu2S b) ___P4O10 + ___ H2O  ___ H3PO4 c) ___ B2O3 + ___ NaOH  ___ Na3BO3 + ___ H2O 14. Potassium nitrate decomposes on heating, producing potassium oxide and gaseous nitrogen and oxygen: 4KNO3  2K2O + 2N2 + 5O2 To produce 56.6 g of oxygen, how many (a) moles of KNO3 and b) grams of KNO3 must be heated? 15. Calculate each of the following quantities: a) Molarity of a solution prepared by diluting 37.00 mL of .250 M potassium chloride to 150.00 mL b) Molarity of a solution prepared by diluting 25.71 mL of 0.0706 M of ammonium sulfate to 500.00 mL 16. When .100 mol of carbon is burned in a closed vessel with 8.00 g of oxygen, how many grams of carbon dioxide can form? Which reactant is in excess and how many grams of it remain after the reaction? Chemistry Exam #1 Answers: 1. a) chemical b) chemical c) physical d) chemical e) physical 2. a) sled sliding down the hill b) water falling over the dam 3. 1.430 x 10^/7 4. a) 1.9 x 10^/9 km ^2 b) $8.14 5. 4.68 x 10^3 kg/m^3 6. 7.24 x 10^-3 7. 14.9 m^3 8. C= 80.6, K= 359.15 9. a) 3 b) 3 c) 4 d) 6 10. 5.12 m 11. .86 g 12. 2.41 x 10^-19 13. a) yes b) no c) yes d) yes e) no f) yes 14. 2.634 x 10^9 mL 15. a) 8.0 x 10^12 g b) 4.1 x 10^5 m^3 c) 9.5 x 10^5 dollars 16. a) physical b) chemical c) physical d) physical CHAPTER 2: 1. a) compound b) element c) mixture d) compound 2. law of mass conservation 3. a) 12.68 g Ca b) .513 mass fraction Ca, .487 mass fraction F c) 51.3% Ca, 48.7% F 4. 36.74 g Cs, 35.02 g I 5. 65.66 amu 6. a) Sr2+ b) N3- 7. 3.86 x 10^22 O2- ions 8. a) cesium nitride, Cs 3 N b) beryllium oxide, BeO c) aluminum bromide, AlBr3 9. strontium sulfide, SrS 10. PbI4 11. Manganese (III) oxide 12. K2CO3 x 2H2O 13. NH4 OH 14. Dichlorine pentaoxide , Cl2 O5 15. 12 O atoms, 1078.89 amu 16. NaHSO4, 120.1 amu 17. 22.8 g aluminum oxide Chapter 3: 1. 3.69 g Ag 2. 1.72 x 10^21 Ga atoms 3. 1.04 x 10^24 atoms Fe 4. 1.5 x 10^20 O atoms 5. 54.07 % 6. 4 Ga (s) + 3 O2 (g)  2 Ga2 O3 (s) 7. 3 CaCl2 (aq) + 2Na3PO4 (aq)  Ca3(PO4)2 + 6 NaCL (aq) 8. a) .105 mol CaO b) .175 mol CaO c) calcium d) 5.89 g CaO e) 1.12 g O2 9. 90.5% 10. a) Cl2O7 b) C02 11. 66.4 mL 12. .87 g BaSO4 13. a) 16Cu + S8  8Cu2S b) P4O10 + 6H2O  4H3PO4 c) B2O3 + 6NaOH  2 Na3 BO3 14. a) 1.42 x 10^3 mol KNO3 b) 1.43 x 10^5 g KNO3 15. a) .016 M KCL b) .00363 M KI 16. 4.42 g CO2, 4.80 g O2 excess


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