LAST NAME, FirstCHEM 107 (Spring-2004)Exam 2 (100 pts)Name: ------------------------------------------------------------------------, SSN -------------------------------- LAST NAME, First(Circle the alphabet segment of your LAST NAME): A,B C-H I-L M-R S-Z Please answer the following questions:Part I: Multiple Choices (48 pts: 12 @ 4 pts each). Circle the ONE best answer:1. The number of ions formed when Al(NO3)3 is dissolved in water is:a) 13 b) 3 c) 2 d) 42. For the reaction: a Al(OH)3 (s) + b H2SO4 (aq) c Al2(SO4)3 (aq) + d H2O The corresponding order for the coefficients a, b, c and d is:a) 2, 3, 1 and 6 b) 1, 1, 1 and 3 c) 2, 1, 2 and 6 d) 2, 3, 1 and 3 3. In dilute nitric acid, HNO3, copper metal dissolves according to the following equation:3 Cu (s) + 8 HNO3 (aq) 3 Cu(NO3)2 (aq) + 2 NO2 (g) + 4 H2O (l)How many grams of HNO3 are needed to dissolve 11.45 g of Cua) 30.27 g b) 0.4805 g c) 1.441g d) 0.18024. For the reaction: 2 Al (s) + 6 HCl (aq) 2 AlCl3 (aq) + 3 H2 (g) the spectator ion(s) are: a) only Cl- b) Al3+ and H+ c) H+ and Cl- d) Al3+ and Cl- 5. Which of the following salts are expected to be insoluble in water? a) CaBr2 b) NiS c) K3PO4d) CsOH 6. In the reaction: CaCO3 (s) + 2 HCl (aq) CaCl2 (aq) + H2O (l) + CO2 (g)What volume of 6.0 M HCl will be needed to react with 0.350 mol of CaCO3? a) 42.0 mL b) 117 mL c) 1.17 L d) 583 mL7. Calculate the molarity of F- in a 250.0 mL solution containing 18.34 g LiF and 4.32 g NaF?a) 0.810 b) 0.202 c) 3.24 d) 4.7718. Which of the following is a weak electrolyte:a) potassium chloride (KCl) b) hydrobromic acid (HBr) c) nitrous acid (HNO2) d) Nitric acid (HNO3)9. Styrene, the raw material for polystyrene foam plastics, has an empirical formula of CH. Its molecular mass is 104. What is its molecular formula? a) 8 b) CH c) (CH)nd) C8H810. A sample of tin (Sn) and chlorine compound with a mass of 2.57 g was found to contain 1.17 g of tin. What is empirical formula of the compound?a) SnCl2b) SnClc) Sn4Cl d) SnCl411. Calculate the molarity of 0.105 g of backing soda (NaHCO3, molar mass = 84 g/mol) in 2.5 mL of solution.a) 0.5 M b) 5.0 x 10-4 M c) 0.042 M d) 42 M12. In a titration, 23.25 mL of 0.105 M NaOH was needed to react with 21.45 mL of HCl. What is the molarity of the acid?a) 2.44 M b) 0.114 Mc) 0.105 M d) no answer was given -----------------------------------------------------------------------------------------------------------------Part II. Equations and formulas (20 pts) Write balanced chemical equations for each of the following. Including physical states as (s, l, g aq) and be careful about the type of arrow you use as or (Use the periodic chart for charges on each ion and reference sheet). Please write N. R. if there is no reaction.1. (6 pts) Write the equation (if any) which represents what happened when KNO3 is mixed with CuCl2 in water: 2. (6 pts) Write the NET IONIC equation for the reaction of Na2SO4 (aq) with BaCl2 (aq) 23. (8 pts) Write the NET IONIC equation for the reaction of a solution of Pb(NO3)2 with a solutionof KI and then identify the spectator ion(s).Part III. Calculations (32 pts) Show all work for full credit. Please express all answers with the proper units and correct number of significant figures.1. (20 pts) A chemist set up a synthesis of phosphorus trichloride by mixing 12.0 g P with 35.0 gCl2. The equation for the reaction is:2 P (s) + 3 Cl2 (g) 2 PCl3 (l)a) Which reagent will be totally consumed (limiting reactant)?b) What is the maximum number of grams of PCl3 that can be produced (theoretical yield)?c) What is the percent yield of the reaction, if 42.4 g of PCl3 wasobtained?3Net ionic equation:Spectator ion(s):Limiting Reactant:Mass of PCl3 =2. (12 pts) Gold(III) hydroxide, Au(OH)3, is used for electroplating gold onto other metals. It can be made by the following reaction:2 KAuCl4 (aq) + 3 Na2CO3 (aq) + 3 H2O 2 Au(OH)3 (aq) + 6 NaCl (aq) + 2 KCl (aq) +3 CO2 (g) To prepare a fresh supply of Au(OH)3 (247.99 g/mol), a chemist at an electroplating plant has mixed 20.00 g of KAuCl4 (377.88 g/mol) with 500.0 mL of 0.472 M Na2CO3 solution. What is the maximum number of grams of Au(OH)3 that can form?4% yield =Limiting Reactant:Maximum mass of Au(OH)3 that can form:Exam 2 – Spring 2004You will have 60 minutes to complete this exam. The exam has 5 pages plus the Periodic Table and Reference page.When you are told to do so, tear off the Periodic Table cover sheet and use as required during the exam. 11H1.01Periodic Table of the Elements2He4.0023Li6.944Be9.015B10.816C12.017N14.018O16.009F19.0010Ne20.18311Na22.9912Mg24.3013Al26.9814Si28.0815P30.9716S32.0617Cl35.4518Ar39.95419K39.120Ca40.0821Sc44.9622Ti47.8823V50.9424Cr52.0025Mn54.9426Fe55.8527Co58.9328Ni58.6929Cu63.5530Zn65.3831Ga69.7232Ge72.5933As74.9234Se78.9635Br79.9036Kr83.80537Rb85.4738Sr87.6239Y88.9140Zr91.2241Nb92.9142Mo95.9443Tc(98)44Ru101.145Rh102.946Pd106.447Ag107.948Cd112.449In114.850Sn118.751Sb121.852Te127.653I126.954Xe131.1655Cs132.956Ba137.357La138.972Hf178.573Ta181.074W183.875Re186.276Os190.277Ir192.278Pt195.179Au197.080Hg200.681Tl204.482Pb207.283Bi209.084Po(209)85At(210)86Rn(222)787Fr(223)88Ra226.089Ac227.0104Rf(261)105Db(262)106Sg(263)107Bh(262)108Hs(265)109Mt(266)110Uun(269)111Uuu(272)112Uub(277)58Ce140.159Pr140.960Nd144.261Pm(145)62Sm150.463Eu152.064Gd157.265Tb158.966Dy162.567Ho164.968Er167.369Tm168.970Yb173.071Lu175.090Th232.091Pa231.092U238.093Np237.094Pu(244)95Am(243)96Cm(247)97Bk(247)98Cf(251)99Es(252)100Fm(257)101Md(258)102No(259)103Lr(260)PREFERENCE SHEET FOR CHEM 107Equations and Constants:Density = Mass/Volume K = 273 + C Avogadro’s Number = 6.022 x 1023 General Solubility GuidelinesAll nitrates are soluble.All salts of sodium, potassium and ammonium are soluble.All chlorides, bromides and iodides are soluble except Ag+, Hg22+, and Pb2+.All sulfates are soluble except Ba2+, Sr2+, Pb2+ and Hg22+.All acetates, chlorates and perchlorates are soluble.Everything else will be considered