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chem1211%20test%202a%20spring%202012.docx

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Exam 2A - Chem1211 Spring 2012 (CHAPTERS 4 AND 5) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) According to the following balanced reaction, how many moles of NO are formed from 8.44 moles of NO 2 if there is plenty of water present? 3 NO 2 (g) + H 2 O(l) → 2 HNO 3 (aq) + NO(g) 1) _______ A) 1.83 moles NO B) 5.63 moles NO C) 25.3 moles NO D) 2.81 moles NO E) 8.44 moles NO
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  Exam 2A -  Chem1211 Spring 2012 (CHAPTERS 4 AND 5) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) According to the following balanced reaction, how many moles of NO are formed from 8.44 moles of NO2 if there is plenty of water present? 3 NO2(g) + H2O(l) →  2 HNO3(aq) + NO(g) 1) _______ A) 1.83 moles NO B) 5.63 moles NO C) 25.3 moles NO D) 2.81 moles NO E) 8.44 moles NO 2) Convert 1.25 atm to mm Hg. 2) _______ A) 1000 mm Hg B) 875 mm Hg C) 760 mm Hg D) 1520 mm Hg E) 950 mm Hg 3) Which of the following is NOT part of the kinetic theory of gases? 3) _______ A) Gas particles move faster when the temperature increases. B) A gas is composed of very small particles. C) There is very little empty space in a gas. D) Gas particles do not attract or repel one another. E) Gas particles move rapidly. 4) A tank contains helium gas at 490 mmHg, nitrogen gas at 0.75 atm, and neon at 520 torr. What is the total pressure in atm? 4) _______ A) 1.5 atm B) 0.55 atm C) 1600 atm D) 2.1 atm E) 1.0 x atm 5) What volume will a balloon occupy at 1.0 atm, if the balloon has a volume of 7.6 L at 3.8 atm? 5) _______ A) 5.0 L B) 35 L C) 29 L D) 2.0 L E) 17 L 6) To what temperature must a balloon, initially at 25°C and 2.00 L, be heated in order to have a volume of 6.00 L? 6) _______ A) 75 K B) 655 K C) 403 K D) 894 K E) 993 K 7) What pressure will 14.0 g of CO exert in a 3.5 L container at 75°C? 7) _______ A) 1.1 atm B) 4.1 atm C) 6.4 atm D) 2.3 atm E) 5.0 atm 8) Which of the following samples will have the greatest volume at STP? 8) _______ A) 22 g Cl2 B) 22 g O2 C) 22 g He D) 22 g CO E) All of these samples would have the same volume at STP.   9) In a container containing CO, H2 , and O2 , what is the mole fraction of CO if the H2 mole fraction is 0.22 and the O2 mole fraction is 0.58? 9) _______ A) 0.20 B) 0.50 C) 0.10 D) 0.30 10) Give the definition for diffusion. 10) ______ A) gas molecules mix unequally B) average distance between collisions C) gas molecules spread out in a concentration gradient D) gas molecules mix equally E) gas molecules escape from a container into a vacuum through a small hole 11) How many grams of oxygen are formed when 6.21 moles of KOH are formed? 4 KO(s) +  2 H2O(l) →  4 KOH(s) +  O2(g) 11) ______ A) 19.9 g O2 B) 27.9 g O2 C) 11.7 g O2 D) 3.59 g O2 E) 49.7 g O2 12) Determine the theoretical yield of H2S (in moles) if 4.0 mol Al2S3 and 4.0 mol H2O are reacted according to the following balanced reaction. A possibly useful molar mass is Al2S3 =  150.17 g/mol. Al2S3 (s) + 6 H2O(l) →  2 Al(OH)3 (s) + 3 H2S(g) 12) ______ A) 2.0 mol H2S B) 12 mol H2S C) 18 mol H2S D) 4.0 mol H2S E) 6.0 mol H2S 13) Give the percent yield when 28.16 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 8.000 moles of O2. 2 C8H18  +  25 O2  →  16 CO2  +  18 H2O 13) ______ A) 25.00% B) 20.00% C) 50.00% D) 12.50% 14) How many milliliters of a 0.184 M NaNO3 solution contain 0.113 moles of NaNO3? 14) ______ A) 543 mL B) 163 mL C) 326 mL D) 885 mL E) 614 mL 15) Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution. 15) ______ A) 1.50 M B) 0.768 M C) 1.18 M D) 0.130 M E) 2.30 M 16) How many molecules of sucrose (C12H22O11 , molar mass =  342.30 g/mol) are contained in 14.3 mL of 0.140 M sucrose solution? 16) ______ A) 5.90  ×  1024 molecules C12H22O11 B) 1.21 ×  1021 molecules C12H22O11 C) 8.29 ×  1022 molecules C12H22O11  D) 1.63 ×  1023 molecules C12H22O11 E) 6.15 ×  1022 molecules C12H22O11 17) Which of the following is considered a STRONG  electrolyte? 17) ______ A) C12H22O11 B) CH3OH C) PbCl2 D) HC2H3O2 E) NH4NO3 18) Which of the following is a precipitation reaction? 18) ______ A) 2 LiI(aq) + Hg2(NO3)2(aq) →  Hg2I2(s) + 2 LiNO3(aq) B) Zn(s) + 2 AgNO3(aq) →  2 Ag(s) + Zn(NO3)2(aq) C) HCl(aq) + KOH(aq) →  KCl(aq) + H2O(l) D) NaCl(aq) + LiI(aq) →  NaI(aq) + LiCl(aq) E) None of the above are precipitation reactions. 19) Give the net ionic equation  for the reaction (if any) that occurs when aqueous solutions of K2S and Fe(NO3)2 are mixed. 19) ______ A) K+(aq) + NO3 - (aq) →  KNO3(s) B) Fe2 + (aq) +  S2 - (aq) +  2 K + (aq) +  2 NO3 - (aq) →  Fe2 + (aq) +  S2 - (aq) +  2 KNO3(s) C) Fe2+(aq) + S2 - (aq) →  FeS(s) D) Fe2 + (aq) +  S2 - (aq) + 2 K + (aq) +  2 NO3 - (aq) →  FeS(s) + 2 K + (aq) +  2 NO3 - (aq) E) No reaction occurs. 20) Determine the oxidation state of Sn in Sn(SO4)2. 20) ______ A) +2 B) - 2 C) +4 D) +6 E) 0 21) Determine the reducing agent in the following reaction. 2 Li(s) + Fe(C2H3O2)2(aq) →  2 LiC2H3O2(aq) + Fe(s) 21) ______ A) C B) Li C) Fe D) H E) O 22) How many milliliters of a 0.266 M LiNO3 solution are required to make 150.0 mL of 0.075 M LiNO3 solution? 22) ______ A) 42.3 mL B) 35.1 mL C) 18.8 mL D) 23.6 mL E) 53.2 mL 23) Which of the following gas samples would be most likely to behave ideally under the stated conditions? 23) ______ A) CO at 200 atm and 25°C B) SO2 at 2 atm and 0 K C) Ne at STP D) O2 at 400 atm and 25°C E) N2 at 1 atm and - 70°C 24) Which of the following statements is TRUE? 24) ______ A) The smaller a gas particle, the slower it will effuse  B) The higher the temperature, the lower the average kinetic energy of the sample. C) At a given temperature, lighter gas particles travel more slowly than heavier gas particles. D) At low temperatures, intermolecular forces become important and the pressure of a gas will  be lower than predicted by the ideal gas law. E) None of the above statements are true. 25) Which of the following is an acid base reaction? 25) ______ A) C(s) + O2(g) →  CO2(g) B) 2 HClO4(aq) + Ca(OH)2(aq) →  2 H2O(l) + Ca(ClO4)2(aq) C) MgSO4(aq) + Ba(NO3)2(aq) →  Mg(NO3)2(aq) + BaSO4(s) D) Fe(s) + 2 AgNO3(aq) →  2 Ag(s) + Fe(NO3)2(aq) E) None of the above are acid base reactions.
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