Fall 2011 CHEM 1110.40413 Test 4, Form A Part I. Multiple Choice: Clearly circle the best answer. (60 pts) Name: 1. The common constituent in all acid solutions is A) H 2 SO 4 B) H 2 C) H + D) OH 2. Which of the following is a weak acid? A) HF B) HBr C) HCl D) H 2 SO 4 3. What are the conditions of STP? A) 273.15 C and 760 torr B) 0 K and 1atm C) 273.15 K and 1 atm D) 0 C and 760 atm 4. What is the oxidation number for sulfur in sulfuric acid, H 2 SO 4? A) 2 B) 4 C) +6 D) +1 5. Select the precipitate that forms when aqueous NH 4 S reacts with aqueous Cu(NO 3 ) 2. A) NH 4 NO 3 B) CuS C) NH 4 (NO 3 ) 2 D) Cu 2 S 6. What is the process where molecules go directly from the solid phase to the gas phase? A) sublimation B) condensation C) melting D) deposition 7. Which of the following is a strong acid? A) H 3 PO 4 B) NaCl C) HNO 3 D) Ba(OH) 2 8. Which of the following is a strong base? A) Al(OH) 3 B) NH 3 C) B(OH) 3 D) Ca(OH) 2 Form A Page 1
9. Which of these chemical equations describes an acid-base neutralization reaction? A) 2KBr(aq) + Cl 2 (g) 2KCl(aq) + Br 2 (l) B) LiOH(aq) + HNO 3 (aq) LiNO 3 (aq) + H 2 O(l) C) 2Al(s) + 3H 2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 (g) D) SO 2 (g) + H 2 O(l) H 2 SO 3 (g) 10. Based on the solubility rules, which one of these compounds should be insoluble in water? A) MgBr 2 B) AgBr C) NaCl D) FeCl 2 11. Deviations from the ideal gas law are greater at A) high temperatures and high pressures. B) low temperatures and low pressures. C) high temperatures and low pressures. D) low temperatures and high pressures. 12. What is the process where molecules go directly from the gas phase to the solid phase? A) sublimation B) condensation C) deposition D) freezing 13. Which one of the following substances should exhibit hydrogen bonding in the liquid state? A) CH 4 B) CH 3 OH C) H 2 S D) PH 3 14. What is the net ionic equation when sodium sulfate is mixed with barium hydroxide? A) Ba + (aq) + SO 2 4 (aq) BaSO 4 (s) B) Ba 2+ (aq) + SO 2 4 (aq) BaSO 4 (s) C) Na + (aq) + OH (aq) NaOH(s) D) Na + (aq) + SO 2 4 (aq) Na 2 SO 4 (s) 15. Which of these choices is the correct net ionic equation for the reaction that occurs when solutions of Pb(NO 3 ) 2 and NH 4 Cl are mixed? A) Pb 2+ (aq) + 2NO 3 (aq) + 2NH + 4 (aq) + 2Cl (aq) 2NH + 4 (aq) + 2NO 3 (aq) + PbCl 2 (s) B) Pb(NO 3 ) 2 (aq) + 2NH 4 Cl(aq) NH 4 NO 3 (aq) + PbCl 2 (s) C) NH + 4 (aq)+ NO 3 (aq) 2NH 4 NO 3 (s) D) Pb 2+ (aq) + 2Cl (aq) PbCl 2 (s) 16. Based on the solubility rules, which of these processes will occur if solutions of CuSO 4 (aq) and BaCl 2 (aq) are mixed? A) BaCl 2 will precipitate; Cu 2+ 2 and SO 4 are spectator ions. B) CuCl 2 will precipitate; Ba 2+ 2 and SO 4 are spectator ions. C) CuSO 4 will precipitate; Ba 2+ and Cl are spectator ions. D) BaSO 4 will precipitate; Cu 2+ and Cl are spectator ions. Form A Page 2
17. Select the precipitate that forms when the following reactants are mixed. Na 2 CO 3 (aq) + BaCl 2 (aq) A) BaCO 3 B) NaCl C) NaCl 2 D) Ba 2 CO 3 18. In which of the following compounds will the molecules not form hydrogen bonds in the liquid state? 19. What is the formula which describes the relationship between the pressure and volume at constant temperature and constant moles? A) P α 1/V B) P α V 2 C) None of the answers is correct D) P α V 20. Arrange the following gases in order of increasing rate of effusion: C 2 H 6, Ar, HCl, and PH 3. A) C 2 H 6 < HCl < PH 3 < Ar B) Ar < PH 3 < C 2 H 6 < HCl C) Ar < HCl <PH 3 < C 2 H 6 D) C 2 H 6 < PH 3 < HCl < Ar 2 21. The oxidation number of Cr in Cr 2 O 7 A) 7 B) +7 C) 12 D) +6 is 22. Which of the following is insoluble in water? A) PbCl 2 B) Li 2 CO 3 C) (NH 4 ) 2 S D) NaOH 23. When the following redox reaction is balanced, what coefficient is in front of Ag (s)? Fe (s) + Ag + (aq) Fe 2+ (aq) + Ag (s) A) 3 B) 4 C) 2 D) 1 Form A Page 3
24. Based on the solubility rules, which one of these compounds should be soluble in water? A) PbSO 4 B) CaSO 4 C) K 2 SO 4 D) BaSO 4 25. Which of the following should have the highest boiling point? A) CI 4 B) CBr 4 C) CF 4 D) CCl 4 26. Which of the following terms refers to the resistance of a liquid to flow? A) Viscosity B) Adhesion C) Capillary action D) Surface tension 27. What is the volume of NH 3 produced in the following reaction when 3.0 L of H 2 reacts with excess N 2 at constant temperature and pressure? N 2 (g) + 3H 2 (g) 2NH 3 (g) A) 4.5 L B) 3.0 L C) 6.0 L D) 2.0 L 28. What is the formula which describes the relationship between the volume and temperature at constant pressure and constant moles? A) V 2 α T B) None of the answers is correct C) V α T D) V α 1/T 29. In the following reaction, what ions, if any, are spectator ions? Pb(NO 3 ) 2 (aq) + 2NaCl(aq) PbCl 2 (s) + 2NaNO 3 (aq) A) Na + (aq), Cl (aq) B) Pb 2+ (aq), Cl (aq) C) Na + (aq), NO 3 (aq) D) Pb 2+ (aq), NO 3 (aq) 30. What is the Kelvin temperature at 24 C? A) 11.4 K B) 297 K C) 249 K D) 297 K Form A Page 4
Part II. Calculations: Clearly show all work for full credit. (35 pts) 1. (10 pts) If a constant number of moles of a gas is at a pressure of 1.35 atm and has a volume of 23.8 L at a temperature of 205.1 K then what is the final volume of the gas if the pressure changes to 2.84 atm and the temperature rises to 233.4 K? 2. (15 pts) Elemental chlorine gas is usually produced by the electrolysis of sodium chloride. How many liters of chlorine gas at 25 C and 0.950 atm can be produced by the reaction of 120.0 g of NaCl? (R = 0.08206 L atm/k mol, MM of NaCl = 58.43 g/mol) 2 NaCl + 2 H 2 O Cl 2 + H 2 + 2 NaOH 3. (10 pts) What is the mole fraction of NO in a 55.0 L gas cylinder at 30 o C which comes from a mixture of N 2 and NO if you have 3.238 mol of N 2 and the gas cylinder has a total pressure of 2.14 atm? Form A Page 5
Part III. Phase Diagrams (5 pts): In the phase diagram below, label the three phases (s, l, and g) and the triple point (TP). Also, indicate the phase boundary where sublimation occurs. IA VIIIA 1 2 1 H He 1.008 IIA IIIA IVA VA VIA VIIA 4.00 3 4 5 6 7 8 9 10 2 Li Be B C N O F Ne 6.94 9.01 10.81 12.01 14.01 16.00 19.00 20.18 11 12 13 14 15 16 17 18 3 Na Mg Al Si P S Cl Ar 22.99 24.31 IIIB IVB VB VIB VIIB VIIIB IB IIB 26.98 28.09 30.97 32.06 35.45 39.95 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 39.10 40.08 44.96 47.90 50.94 52.00 54.94 55.85 58.93 58.71 63.55 65.37 69.72 72.59 74.92 78.96 79.90 83.80 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 85.47 87.62 88.91 91.22 92.91 95.94 [98] 101.1 102.9 106.4 107.9 112.40 114.8 118.7 121.8 127.60 126.90 131.30 55 56 71 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 6 Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 132.9 137.3 175 178.5 181 183.9 186.2 190.2 192.2 195.1 197 200.59 204.4 207.2 209 [209] [210] [222] 87 88 103 104 105 106 107 108 109 110 111 112 113 114 115 116 118 7 Fr Ra Lr Rf Db Sg Bh Hs Mt Ds Rg Uub Uut Uuq Uup Uuh Uuo [223] [226] [262] [267] [268] [271] [272] [270] [276] [281] [280] [285] [284] [289] [288] [293] [294] 57 58 59 60 61 62 63 64 65 66 67 68 69 70 La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb 138.9 140.1 140.9 144.2 [145] 150.4 152 157.3 158.9 162.5 164.93 167.3 168.9 173 89 90 91 92 93 94 95 96 97 98 99 100 101 102 Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No [227] 232 [231] 238 [237] [244] [243] [247] [247] [251] [252] [257] [258] [259] Form A Page 6