Chem October 31, Dr. Susan E. Bates
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1 Chem 1711 Exam 2 ID#: October 31, 2013 Dr. Susan E. Bates Name 9:00 OR 10:00 PV = nrt 1 atm = 760 mmhg = kpa u = (3RT/M m ) 1/2 R = L atm K 1 mol 1 OR J K 1 mol L/mol at STP 1 J = 1 kg m 2 /s 2 ΔE = q + w = q PΔV ΔH = q p = msδt = CΔT 1 L atm = J 1 ml = 1 cm 3 N A = x 23 mol 1 ph = log[h 3 O + ] I A II A III B IV B V B VI B VII B VIII I B II B III A IV A V A VI A VII A inert gases 1 H Li Na K Rb Cs Fr (223) 4 Be Mg Ca Sr Ba Ra Sc Y * La * Ac (227) 22 Ti Zr Hf Rf (261) 23 V Nb Ta Db (262) 24 Cr Mo W Sg (263) 25 Mn Tc Re Bh (262) 26 Fe Ru Os Hs (265) 27 Co Rh Ir Mt (266) 28 Ni Pd Pt (269) 29 Cu Ag Au (272) 30 Zn Cd Hg (277) 5 B Al Ga In Tl ? 6 C Si Ge Sn Pb (289) 7 N P As Sb Bi O S Se Te Po (210) 9 F Cl Br I At (210) 2 He Ne Ar Kr Xe Rn (222) 58 Ce Th Pr Pa (231) 60 Nd U Pm (147) 93 Np (237) 62 Sm Pu (242) 63 Eu Am (243) 64 Gd Cm (247) 65 Tb Bk (247) 66 Dy Cf (251) 67 Ho Es (254) 68 Er Fm (253) 69 Tm Md (256) 70 Yb No (254) 71 Lu Lr (257)
2 Chem 1711: Exam 2 Part I (43 points): Short Answer. Name 1. Balance the following chemical equation, and then write the corresponding, balanced full and net ionic equations for the reaction. Include all physical states and charges on ions. KI (aq) + Pb(NO 3 ) 2 (aq) KNO 3 (aq) + PbI 2 (s) full ionic equation: net ionic equation: 2. Air is trapped in a closed flask at 21 C, which is connected to a pressure sensor that reads 97.3 kpa. Determine the pressure exerted (in kpa) by the air in the flask when the flask is submerged into a bath of ice water at 3 C. kpa. 3. A student in lab studied Boyle s law and graphed pressure (P) vs. volume (V) for an ideal gas. Using the graph to the right, sketch the line or curve showing the expected trend of the data points. P V 4. Which of the following substances are soluble in water? Circle all that are appropriate. KH 2 PO 4 AgC 2 H 2 O 2 Co 3 O 4 PbSO 4 MgCl 2 CuS 5. Circle the oxidizing agent in the following reaction: Br 2 (l) + K 2 SO 3 (aq) + H 2 O (l) 2 KBr (aq) + H 2 SO 4 (aq) 6. A sample of household ammonia cleaning solution has [H 3 O + ] = 9.2 x M. Determine the ph of this solution. ph = 7. Consider that 1 mole of Ca(NO 3 ) 2 solid is dissolved in water. How many moles of ions are present in the resulting sol n? mol 8. How much heat (in kj) must be absorbed by a 20.0 g sample of H 2 O (l) to raise its temperature from 19.5ºC to 37.5ºC? For H 2 O (l), specific heat = J/gºC. kj
3 9. A 50.0 L carboy of M HCl (aq) is needed for a general chemistry lab experiment. Determine the volume (in ml) of 12.0 M HCl (aq) that needs to be diluted to make this solution. ml 10. Using the half-reaction method, balance the following redox reaction which occurs in acidic solution: oxidation half reaction: HSO 3 (aq) + MnO 4 (aq) Mn 2+ (aq) + HSO 4 (aq) reduction half reaction: net ionic equation: 11. Give the oxidation number of: Br in NaBrO 2 C in KHC 2 O 4 F in CF If copper metal is dissolved in acid, the resulting solution is in color. 13. If 10.0 g N 2 (g) and 10.0 g Cl 2 (g) are mixed, determine the mole fraction of Cl 2. χ Cl2 = / 43 Part II (42 points): Multiple Choice. Indicate the one best answer for each of the following on your Scan-Tron sheet g of solid NaBr is dissolved in water resulting in ml of solution. Determine the molarity of this solution. a M b M c M d M e M 2. Nitrogen triiodide is extremely sensitive; touching it with a feather causes it to decompose. Calculate the standard enthalpy change for this reaction using the given standard enthalpies of formation: 2 NI 3 (s) N 2 (g) + 3 I 2 (g) Hº f (in kj/mol): a. 156 kj b kj c. 291 kj d kj e. 417 kj 3. Which one of the following is an acidic oxide? a. Na 2 CO 3 b. CaO c. NH 3 d. SO 3 e. KOH
4 4. Determine the volume of M NaOH (aq) required to reach the stoichiometric point in the titration of ml of M HCl (aq). a ml b ml c ml d ml e ml 5. Consider the following gas phase reaction that takes place at constant temperature and volume: 2 X (g) + 3 Z (g) X 2 Z 3 (g) If atm X (g) and atm Z (g) are combined and allowed to react, identify the limiting reactant, and the pressure exerted by X 2 Z 3 when the reaction is complete. a. X; atm b. X; atm c. Z; atm d. Z; atm e. there is not enough information to answer 6. Hydrogen peroxide, H 2 O 2, is used as an antiseptic. It can be prepared in a process described by the following chemical equation: H 2 (g) + O 2 (g) H 2 O 2 (l). Determine H for this reaction using the following information: 2 H 2 O 2 (l) 2 H 2 O (l) + O 2 (g); H = 196 kj 2 H 2 (g) + O 2 (g) 2 H 2 O (l); H = 572 kj a. 768 kj b. 188 kj c kj d kj e. +90 kj 7. A gas mixture contains 1.0 mol neon, 2.0 mol argon, and 3.0 mol krypton in a 10.0 L tank at 0 C. Determine the partial pressure of neon. a atm b. 230 atm c. 2.2 atm d. 13 atm e atm 8. Determine the volume (in L at STP) of hydrogen gas that can theoretically be formed when 1.00 mol sodium metal is allowed to react with 2.00 mol water: 2 Na (s) + 2 H 2 O (l) 2 NaOH (aq) + H 2 (g) a L b L c L d L e L 9. Which one of the following is an expected product in the reaction of Mg(OH) 2 (aq) and HNO 3 (aq)? a. H 2 O (l) b. Mg (s) c. NO 2 (g) d. O 2 (g) e. MgO (s) 10. Which one of the following substances, when dissolved in water, forms a strong electrolyte solution? a. Cu (s) b. NH 3 (g) c. HC 2 H 3 O 2 (aq) d. HBr (g) e. CH 3 OH (l)
5 11. Which one of the following gas samples has the greatest rate of diffusion? a. H 2 at 20 C b. H 2 at 100 C c. Ar at 20 C d. Ar at 100 C e. these all have the same rate of diffusion 12. Ammonia is produced industrially using the following reaction: N 2 (g) + 3 H 2 (g) 2 NH 3 (g); H = 92 kj. Determine the quantity (in kj) of heat associated with the production of 24 kg NH 3 (g). And, is this heat released or absorbed? a. 5.4 kj; absorbed b. 65,000 kj; released c. 44 kj; released d. 92 kj; absorbed e. 130,000 kj; released 13. Which one of the following statements about the kinetic molecular theory is false? a. Most of the volume in a gas sample is empty space. b. As the temperature is decreased for a gas sample, the forces of particle collisions will increase. c. As the temperature of a gas sample increases, the kinetic energy & the rms speed of the particles increases. d. Gas molecules move in straight lines at very high speeds until their direction is changed by collisions with the container walls or other gas particles. e. Gas molecules can effuse through small holes in porous barriers because they are in constant, random motion. 14. A student made the following statements about thermochemistry. Which one of these statements is false? a. For an endothermic change, heat is transferred from the surroundings to the system. b. For the system in an exothermic process, q final < q initial. c. The sign of H for an exothermic reaction is negative. d. When work is done on a system by its surroundings, the sign of w is negative. e. When a reaciton is multiplied by a certain factor, n, the value of H for that reaction must also be multiplied by n. / 42 Part III (15 points): Problems. Work all of the following problems. Show all work; work with units in all steps; report all answers with appropriate units and significant figures. Partial credit will not be given if I cannot follow your work. 1. A pure sample of a very dense, radioactive gas has a mass of 10.6 g and exerts a pressure of 716 mmhg in a ml flask at 13 C. Determine the molar mass of this gas (include units).
6 2. Calculate the temperature (in C) at which the molecules in a sample of hydrogen gas have an rms speed of 675 m/s. C ml of a solution containing CaCl 2 is mixed with an excess of Na 3 PO 4. A precipitation reaction occurs; 2.51 g of dried precipitate is recovered. Determine the molar concentration of Ca 2+ ions in the original solution. [Ca 2+ ] = M / 15
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