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[Exam Tutorial] Chem 112 2009 Midterm Questions

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CHEM 112
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University of Saskatchewan Department of Chemistry CHEMISTRY 1th.3 Midterm Examination (Sat. Oct 24 , 2009, 10:00 AM – 12:00 noon) (VERSION A) Family Name (please print carefully!)____________________________________________ Given Name (please print carefully!)_____________________________________________ Student Number Signature___________________________________ Please indicate your section: Section 01 MWF 8:30 am Dr. K. Brown Section 03 MWF 9:30 am Dr. A. Grosvenor Section 05 TTh 10:00 am Dr. A. Baranski Section 91 TTh 8:30 am Dr. L. Wilson Section 97 Muenster Dr. A. Szmigielski Section C11 Melfort Dr. A. Szmigielski Section C15 Prince Albert Dr. P. Ahiahonu Section C51 North Battleford Dr. K. Pasha INSTRUCTIONS - PLEASE READ THIS FIRST! a) This is a closed-book examination. A data-sheet with a Periodic Table can be found as the last page of this examination paper. b) Simple scientific calculators (maximum two-line display) are permitted; graphing calculators, PDA's, electronic dictionaries, etc. are not. No equations should be stored in memory. c) This examination paper has 10 pages. To ensure your copy is complete and to become familiar with the questions, please read through the entire examination before you answer any questions. d) You can use the backsides of the 10 pages as scratch paper (more paper will be available on request). e) A total of 100 marks can be obtained. Each of the 40 questions will be weighted with 2.5 marks. You should spend on average 3 min. on each question. ONLY one answer per question is correct! f) Please fill out the top of this paper and on the blue sheet, print your name and code your student number in soft pencil. g) On the blue sheet, after your name, write in brackets the version of the exam (A or B) as shown on the top of this paper. h) Answer multiple choice questions by circling a response on this paper AND by filling in the corresponding response on the blue opscan sheet USING ONLY A SOFT-LEAD PENCIL. No deductions will be made for incorrect answers. Multiple answers will be treated as NO answer; if you change your mind, erase carefully. In the event of a discrepancy between an answer on the examination paper and on the computer sheet, the response on the opscan sheet will count. i) HAND-IN ALL your material: question sheet, computer sheet, and scratch paper (if you use one). 1 1. State the answer to the following question using the proper number of significant figures. Assume that all these numbers represent results of experimental measurements (they are not exact numbers) and all are written with correct number of significant figures. 37.123(7.12.32) 4 11.0001 A. 1.377 B. 1.4 C. 1  D. 1.40 E. 1.38 2. C(s)raphite) is deposited onto Ni metal by vapour deposition forming NiC at(s)e surface after heating. What type of change is this? A. Chemical B. Physical C. Not enough information is provided D. Neither (a) or (b) E. Both (a) and (b) 2+ 3. A single Cu ion has: A. 61 electrons B. 34 protons C. 29 neutrons D. 27 electrons E. None of the above 4. Which of the following elements is an alkali metal? A. Xe B. Li C. Ca D. Zn E. F 5. Calculate the atomic mass of element X knowing that X has only 2 naturally occurring isotopes with the 107lowing masses and natural abundances: X: 106.90509 amu, 51.84% 109X: 108.90476 amu, 48.16% A. 107.87 amu B. 107.94 amu C. 107.00 amu D. 108.32 amu E. None of the above 2 6. How many xenon atoms are contained in 2.36 moles of xenon? 23 A. 2.55 × 10 xenon atoms B. 3.92 × 10 xenon atoms 24 C. 1.42 × 10 x25on atoms D. 7.91 × 10 xenon atoms E. 1.87 × 10 xenon atoms 7. Which of the following species contains the greatest number of S atoms? A. 0.12 mol S 8 B. 0.5 mol S O2 C. 32 g SO 2 D. 76 ml of CS (d2nsity = 1.2 g/ml) E. 32 g S 8 8. What is the name of OsCl . 3 A. Osmium (IV) chloride B. Osmium tetrachloride C. Osmium (III) chloride D. Osmium chloride E. Osmium trichloride 9. Write the chemical formula for perchloric acid. A. HClO 3 B. HClO 2 C. H 2lO 3 D. HClO 4 E. HClO 10. Write the balanced equation for the reaction of O (g), 2O (g), an2 H O(l) whi2h forms aqueous nitric acid (HNO ).3 A. NO (2) + O (g)2+ H O(l)2 HNO (aq) 3 B. 4NO (g2 + O (g)2+ 2H O(l)2 3HNO (aq) 3 C. 2NO (g2 + O(g) + H O(l)2 2HNO (aq) 3 D. 3NO (g2 + O (g)2+ 2H O(l) 2 4HNO (aq) 3 E. 4NO (2) + O (g)2+ 2H O(l)2 4HNO (aq) 3 11. Write the balanced equation for the reaction of liquid pentane (C H ) with O (g) to form gaseous carbon 5 12 2 dioxide, CO (g2, and liquid water. A. C H (l) + 7O (g)  4CO (g) + 5H O(l) 5 12 2 2 2 B. C 5 (12 + 8O (g)2 5CO (g) + 2H O(l) 2 C. C H (l) + O (g)  CO (g) + H O(l) 5 12 2 2 2 D. 2C H5(l12+ 8O (g)2 5CO (g) + 62 O(l) 2 E. C 5 (12 + 4O (g)2 3CO (g) + 2H O(l) 2 3 12. Calculate the empirical formula of methamphetamine (aka crank) containing, by mass, 80.5 % C, 10.1 % H, and 9.4% N. A. C 10N15 B. C 5 12 2 C. C 9 16 D. C 8 N25 2 E. C H N 8 17 13. Combustion of 0.3204 g of a C, H, and O containing compound produces 0.4401 g of CO and 0.3623 g of H O. What is the empirical formula of the compound? 2 A. C 6 O6 B. CH O 4 C. C 2O D. C 3 O6 E. None of the above 14. How many of the following elements are classified as diatomic molecular elements. Oxygen [O], Neon [Ne], Chlorine [Cl], Sulfur [S], Nitrogen [N] A. 0 B. 1 C. 2 D. 3 E. 4 15. In calcium perchlorate, what type of bonding occurs between (i) the cation and the polyatomic anion, and (ii) the atoms within the polyatomic anion? A. (i) covalent, (ii) ionic B. (i) ionic, (ii) ionic C. (i) covalent, (ii) covalent D. (i) ionic, (ii) molecular E. (i) ionic, (ii) covalent 16. What are the correct values of the smallest integer stoichiometric coefficients (a, b, c and d) required to balance this equation? a Fe(OH) +3b H SO2 c4Fe (SO )2+ d 4 3 2 A. a=1, b=1, c=1, d=1 B. a=1, b=2, c=3, d=6 C. a=3, b=2, c=6, d=1 D. a=2, b=3, c=1, d=6 E. None of the above 4 17. For the reaction CaCl (2q) + Na CO2(aq)3 CaCO (s) + 2N3Cl(aq), what is the net ionic equation? + – A. Ca 2+q) + CO (a3)2– CaCO (s) 3 B. Ca (aq) + CO 3 (aq)  CaCO (s)3 C. 2Na (aq) + 2Cl  2NaCl(aq) 2+ + 2– – + – D. Ca (aq) + 2Na (aq) + CO 3 (aq) + 2Cl  CaCO (s) +32Na (aq) + 2Cl E. None of the above 18. The molarity of a solution of 30.0 g of potassium sulfate (K SO 2 dis4olved in water having a total volume of 500 mL is: A. 0.704 M B. 0.344 M C. 3.62 M D. 4.10 M E. None of the above 19. A 112 mL solution of 0.351 M HCl is added to 52.0 mL of 0.161 M HCl. What is the new concentration of HCl? A. 0.100 B. 0.420 C. 0.194 D. 0.291 E. None of the above 20. When equal volumes of 0.2 M solutions are mixed which of the following combinations will form a precipitate? A. NaCl(aq) + NH NO (aq) 4 3 B. K 2O (4q) + CuCl (aq)2 C. Na 3O (a4) + AgNO (aq) 3 D. Ba(OH) (a2) + HCl(aq) E. Fe(NO )3 3q) + Zn(SO ) (a4 2 21. For the reaction: CS 2l) + 3O (g2  CO (g) 2 + 2SO (2) starting with 2.8 mols CS and 8.4 mols O , the limiting reagent is: 2 2 A. CS 2 B. O 2 C. CO 2 D. SO 2 E. Both reactants are provided in the stoichiometric ratio 5 22. Which reaction is a neutralization reaction? A. C 6 O12s)6+ 6O (g) 2 6CO (g) + 6H2O(l) 2 B. 3HCl(aq) + Al(OH) (s)3 3H O(l) 2 AlCl (aq) 3 C. PCl 3s) + Cl 2g)  PCl (s5 2– – 3+ D. Cr 2 7 (aq) + Cl (aq)  Cr (aq) + Cl (g)2 E. H 2g) + Cl (g2  2 HCl(g) – 23. When 250 mL of 0.10 M AlCl is add3d to 250 mL of 0.30 M Ca(NO ) the concent3 2ion of Cl ions after mixing is: A. Almost zero B. 0.075 M C. 0.15 M D. 0.20 M E. 0.30 M 24. Choose the statement below that is TRUE. A. A molecular compound that does not ionize in solution is considered a strong electrolyte B. A weak acid solution consists of mostly nonionized acid molecules C. The term "weak electrolyte" means that the substance is inert D. A strong acid solution consists of only partially ionized acid molecules E. The term "strong electrolyte" means that the substance is extremely reactive 25. Which of the following is an acid base reaction? A. 2 HClO (a4) + Ca(OH) (aq)2→ 2 H O(l) + 2a(ClO ) (aq) 4 2 B. Fe(s) + 2 AgNO (aq) → 2 Ag(s) + Fe(NO ) (aq) 3 3 2 C. MgSO (aq4 + Ba(NO ) (aq)3 2Mg(NO ) (aq) + B3 2 (s) 4 D. C(s) + O (2) → CO (g) 2 E. None of the above is an acid base reaction. 26. The titration of 25.0 mL of an unknown concentration H SO sol2tio4 requires 83.6 mL of 0.12 M LiOH solution. What is the concentration of the H SO2sol4tion? A. 0.10 M B.
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