Chem 1441 Test Questions from Previous Exams Page 1 of 7 Test 1. Chapters 1, 2, and 3 (Rogers textbook) Chapter 1 – Introduction to the Study of Chemistry 1. How many significant figures are in the measured quantity below? 0.000420 a) 2 b) 3 c) 6 d) 7 e) an infinite number 2. A certain balance will report the mass of a sample to the nearest 0.001 g. A sample that weighs about 25 g is weighed on this balance. How many significant figures should be reported for this measurement? a) 1 b) 2 c) 3 d) 4 e) 5 3. A student began an experiment by measuring out 7.482 g of calcium chloride. A few minutes later, she measured out 4.9 g of additional calcium chloride using a different instrument. When she reports the total mass of calcium chloride, how many significant figures should she use? a) 1 b) 2 c) 3 d) 4 e) 5 4. Perform the calculation below. How should the result of this calculation be expressed, taking into account the appropriate use of significant figures? 29.725 + 91.427.95572 - 0.000720 a) 15.2 b) 15.23 c) 15.229 d) 15.2288 e) 15.22879 5. When the following calculation is performed, how many significant figures will the answer have? 1.900 + 0.020023.75 + 0.25 + 0.06223 = ??? a) 1 b) 2 c) 3 d) 4 e) 5 6. Perform the following calculation and express the result using the appropriate number of significant figures: 2.3 x 10-6 + 3.722 x 10-7 + 7.9788 x 10-4 a) 8.0 x 10-4 b) 8.01 x 10-4 c) 8.006 x 10-4 d) 8.0055 x 10-4 e) 8.005522 x 10-4Chem 1441 Test Questions from Previous Exams Page 2 of 7 Test 1. Chapters 1, 2, and 3 (Rogers textbook) 7. Perform the calculation below. How should the result of this calculation be expressed, taking into account the appropriate use of significant figures? 4.93 x 10-7 + 8.9440 x 10-6 + 7.3 x 10-8 a) 9.5 x 10-6 b) 9.51 x 10-6 c) 9.510 x 10-6 d) 9.5100 x 10-6 e) 9.51000 x 10-6 8. All of the following measurements are expressed using SI units except a) 525 K b) 155 m/s c) 1.88 kg of iron d) 3.42 mol of CH4 e) 5.75 L of N2 9. What is the SI unit of mass, and what is the SI unit of volume? a) mg, cm3 b) g, cm3 c) g, L d) kg, L e) kg, m3 10. Convert 475 ºC to Kelvin. a) 202 K b) 748 K c) 246 K d) 887 K e) 704 K 11. Convert 34.2 µg to cg. a) 3.42 x 10-4 cg b) 3.42 x 10-2 cg c) 3.42 x 10-5 cg d) 3.42 x 10-3 cg e) 3.42 x 10-7 cg 12. Acceleration due to gravity of a free-falling object is 9.8 m/s2. Express this value in units of inches/ms2. a) 3.9 x 10-4 in/ms2 b) 0.39 in/ms2 c) 0.039 in/ms2 d) 3.9 x 10-3 in/ms2 e) 3.9 x 104 in/ms2 13. The density of titanium is 4.50 g/cm3. What is the mass, in pounds, of 1.00 ft3 of titanium? a) 139 lbs b) 9.92 lbs c) 281 lbs d) 43.6 lbs e) 302 lbsChem 1441 Test Questions from Previous Exams Page 3 of 7 Test 1. Chapters 1, 2, and 3 (Rogers textbook) 14. An acetaminophen suspension for infants contains 80 mg / 0.80 mL suspension. The recommended dose is 15 mg/kg body weight. How many mL of this suspension should be given to an infant weighing 17 lb? (Assume two significant figures.) a) 1.2 mL b) 51 mL c) 5.6 mL d) 0.0051 mL e) 7.4 mL Chapter 2 – Atoms, Molecules, and Ions 15. A particular copper ion has 28 electrons and 36 neutrons. What is the mass number of this ion? a) 63 b) 64 c) 65 d) 66 e) 67 16. What is the symbol for an ion containing 50 neutrons, 40 protons, and 36 electrons? a) 90Zr4+ b) 90Zr4- c) 50Zr4+ d) 50Sn4+ e) 90Sn4- 17. Which of the following statements correctly describes the relative masses of protons, neutrons, and electrons? a) Protons and neutrons are equal in mass; electrons are much lighter than protons and neutrons. b) A neutron is slightly heavier than a proton; electrons are much lighter than protons and neutrons. c) Protons and electrons are equal in mass; neutrons are slightly lighter than protons and electrons. d) An electron is slightly lighter than a neutron which is slightly lighter than a proton. e) A proton is slightly heavier than a neutron; electrons are much lighter than protons and neutrons. 18. Copper has two naturally occurring isotopes, 63Cu (isotopic mass 62.9396 amu) and 65Cu (isotopic mass 64.9278 amu). If copper has an atomic mass of 63.546 amu, what is the fractional abundance of 63Cu? a) 0.577 b) 0.695 c) 0.423 d) 0.723 e) 0.305 19. Gallium has two naturally occurring isotopes, gallium-69 with a mass of 68.9257 amu and gallium-71 with a mass of 70.9249 amu. Its average atomic mass is 69.72 amu. What is the percent abundance of the gallium-69 isotope? a) 60.3% b) 69.7% c) 39.7% d) 30.3% e) 24.1% 20. Which of the following symbol/name combinations is incorrect? a) Ag, silver b) Au, gold c) W, tungsten d) Na, sodium e) P, potassiumChem 1441 Test Questions from Previous Exams Page 4 of 7 Test 1. Chapters 1, 2, and 3 (Rogers textbook) 21. Which of the following symbol/name combinations is incorrect? a) Ag, silver b) Sn, tin c) Pt, potassium d) Pb, lead e) W, tungsten 22. Which of the following are incorrectly paired? a) potassium, alkali metal b) strontium, transition metal c) bromine, halogen d) argon, noble gas e) silicon, semimetal 23. Which of the following elements is a halogen? a) Br b) S c) Ni d) Ca e) Ne 24. Which of the compounds listed below are ionic? I. KF II. HCl III. NH4Br IV. PCl3 a) I only b) I and II c) I, II and III d) I and IV e) I and III 25. What is the formula for aluminum sulfate? a) Al2(SO3)3 b) Al2(SO4)3 c) Al2S3 d) Al3(SO4)2 e) Al3(SO3)2 26. What is the formula for calcium peroxide? a) Ca(OH)2 b) CaO2 c) CaO d) Ca2O e) Ca2O2 27. Which of the compounds below has the correct formula written next to it? I. mercury(I) chloride, HgCl II. titanium(IV) oxide, TiO2 III. sulfurous acid, H2SO3 IV. iron(III) oxide, Fe3O2 V. sodium bicarbonate, NaHCO3 a) I, III, and IV b) III and V c) II, III, and V d) II, III, IV, and V e) I, III, and VChem 1441 Test Questions from Previous Exams Page 5 of 7 Test 1. Chapters 1, 2, and 3 (Rogers textbook) 28. Which of the following acids is