Chemistry 121 Fall 2002 Oregon State UniversityExam 1 October 24, 2002 Dr. Richard NafshunDr. Nick DrapelaDO NOT OPEN THIS EXAM UNTIL INSTRUCTED.CALCULATORS ARE NOT TO BE SHARED.Instructions: You should have with you several number two pencils, an eraser, your 3" x 5" notecard, andyour University ID Card. You may use a basic calculator (for example, TI-25X Solar or TI-30XA) if you wish. If you have notes or electronic devices with you, place them in a sealed backpack and place the backpack OUT OF SIGHT. Or place the notes directly on the table at the front of the room. Fill in the front page of the Scantron answer sheet with your last name, first name, middle initial, and student identification number. Leave the class section number and the test form number blank.This exam consists of 18 multiple-choice questions and 7 open-ended questions. Each multiple-choice question has four points associated with it. Select the best multiple-choice answer by filling in the corresponding circle on the rear page of the answer sheet. If you have any questions before the exam, please ask. If you have any questions during the exam, please raise your hand to attract the attention of a proctor. The proctor will come to you. Open and start this exam when instructed. Present your ID card when submitting the exam. Place your open-ended portion of this exam in the appropriate stack. Place your 3" x 5" notecard in the appropriate stack. You may keep the multi-choice portion of this exam, so please mark the answers you selected on it.Avogadro’s Number = 6.02 x 1023[1 g = 10-6 g] [1 mg = 10-3 g]1. 8.2 mg is how many g?a. 0.0082 gb. 0.82 g c. 8.2 gd. 82 ge. 8,200 g2. How many significant figures in the value 0.07040 g?a. 2b. 3c. 4d. 5e. 63. Consider the following operation 57.01010 g + 1.12 g = ? Which answer below contains the correct number of significant figures?a. 58 gb. 58.1 gc. 58.13 gd. 58.130 ge. 58.1301 g4. Acetone, the solvent in nail polish remover, has a density of 0.791 g/mL. What is the volume of 25.0 g acetone?a. 0.0318 mLb. 19.8 mLc. 25.8 mLd. 31.6 mLe. 79.1 mL5. Which of the following chemical formulas does not exist?a. BeOb. CsCNc. CaOHd. RbCle. AlF36. Consider sodium nitrate, NaNO3. How many of each type of atom are present in the compound?a. 1 Na, 1 N, 3 Ob. 1 Na, 3 N, 3 Oc. 3 Na, 3 N, 3 Od. 3 Na, 3 N, 9 Oe. 1 Na, 3 N, 2 O7. Which is the correct formula for the compound formed from barium and fluorine?a. BaF c. BaF2e. Ba3Fb. Ba2F d. Ba2F38. Which of the following is an ionic compound?a. H2Ob. NiCuc. MgF2d. COe. O29. Determine the number of protons in 12C, 13C, and 14C.a.12C has 0, 13C has 1, and 14C has 2b.12C has 4, 13C has 4, and 14C has 4c.12C has 6, 13C has 6, and 14C has 6d.12C has 6, 13C has 7, and 14C has 8e.12C has 12, 13C has 13, and 14C has 1410. Which of the following pairs are isotopes?a.16N and 16Ob.15N and 15Oc.14N and 16Nd.20F− and 20Nee.40Ar and 20Ne11. Which of the following elements is most likely to lose an electron?a. Li c. N e. Clb. C d. O12. Determine the mass of 0.876 mol Ca.a. 0.0219 g b. 35.1 gc. 40.1 gd. 45.7 ge. 87.6 g13. What is the formula mass of Al2(SO4)3?a. 197.43 g/molb. 288.91 g/molc. 342.14 g/mold. 393.02 g/mole. 407.86 g/mol14. How many atoms are present in 0.30 mol Krypton?a. 25 atomsb. 84 atomsc. 2.1 x 1021 atomsd. 1.8 x 1023 atomse. 1.5 x 1025 atoms15. Determine the mass percent composition of CaSO4.a. 16.7% Ca, 16.7% S, 66.7% Ob. 20.0% Ca, 20.0% S, 60.0% O c. 25.1% Ca, 20.5% S, 54.4% Od. 29.4% Ca, 23.6% S, 47.0% Oe. 33.3% Ca, 33.3 % S, 33.3% O16. Consider the following reaction:4 P + 5 O2  P4O10How many moles of phosphorus are required to produce 2.00 moles of P4O10?a. 0.500 mol Pb. 2.00 mol P c. 4.00 mol Pd. 8.00 mol Pe. 16.0 mol P17. Consider the following reaction:2 Na + 2H2O  2NaOH + H2In a given experiment, the theoretical yield of hydrogen gas for the above reaction is 3.00g. If the reaction actually produces 2.50 g hydrogen gas, what is the percent yield for the reaction?a. 0.50 %b. 2.50 %c. 17.7%d. 50.0 %e. 83.3%18. If 0.075 L of 1.0 M HCl solution is diluted to 5.0 L what is the molarity of the resulting solution?a. 0.015 Mb. 0.075 Mc. 0.20 Md. 0.38 Me. 1.0 MChemistry 121 Fall 2002 Oregon State UniversityExam 1 October 24, 2002Student's Name ______________________________________________________________________ID Number ______________________________________________________________________Recitation Instructor (Circle One) Jeff Bilyeu Kaustube Gawande Elliot Ennis Jason HughsonMeg Bojan Ragha Darapu Jessie Hartford Hyrum JonesSayf Munir Thirumal Ravula Jack Rundell Cynthia VillwockRecitation Day (Circle One) M/W T/RRecitation Time (Circle One) 0800 0900 1000 1100 1200 1300 1400 1500 1600YOU MUST SHOW ALL WORK ON NUMERICAL PROBLEMS TO RECEIVE CREDIT19. Give an example of each, and explain why:a. A homogeneous mixtureb. A heterogeneous mixture20. Write the formulas for:a. ammonium carbonateb. lithium sulfide21. Balance the following equation:C9H20 + O2  CO2 + H2O22. Give the name for Cu2S.[TURN OVER FOR QUESTIONS 23-25]23. Potassium metal (K) reacts with diatomic oxygen (O2) to form potassium oxide.a. Write the formula for potassium oxide.b. Write the balanced equation for the reaction.24. If 14.0 g KOH are dissolved in 75.0 mL of total solution, what is the resulting molarity?25. Consider the following equation:2H2 + O2  2H2OIf 64.0 g O2 are reacted…a. How many moles of water are formed?b. How many grams of water are