Chemistry 1A - Fall 1995 - Pines - Midterm 3

Chemistry 1A - Fall 1995 - Pines - Midterm 3 - Chemistry 1A...

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Unformatted text preview: Chemistry 1A Midterm Exam III Nov 15, 1995 Professor Pines (Closed Book, 100 minutes, 100 points) Page 1 of 8 Name:_______________________________ Lab TA_____________________________ SID: ____________________________ Discussion TA _______________________ The following formulae and data may be useful: For aA + bB ⇔ cC + dD : ∆ E = q + w Q = [ C]c [ D]d [ A]a[ B]b At equilibrium, Q = K pH =pKa - log [HA]/[A-] R=8.314JK-1mole-1 Photon: E = h υ, λυ = c °( products) − ∑ ∆H f ° (reactants ) Wave-Particle Duality: ∆ H° = ∑ ∆H f λp=h ∆ G° = ∑ ∆G f ° ( products) − ∑ ∆G f °( reactants) S° = ∑ S°( products) − ∑ S° ( reactants) ∆ h = 6.626 x 10-34 J s c = 3.0 x 108 m.s-1 ∆ G° = ∆H ° − T ∆S° = − RT ln K = − nF ∆ε ° Thermodynamic Properties Substance ∆Hf° (kJ mol-1) S° (J K-1mol-1) Substance ∆Hf° (kJ mol-1) S° (J K-1mol-1) O2 0 205.03 H2SO4 -814.0 156.9 FeS2 -178.2 52.93 H2O(l) -285.8 69.91 Fe2O3 -824.2 87.4 NaCl - 411.15 72.13 Standard Reduction Potentials Half-Reaction ε°(V) Half-Reaction ε°(V) MnO4-+ 8 H++ 5 e- ∅ Mn2+ + 4 H2O +1.49 Sn2+ + 2 e- ∅ Sn (s) -0.14 Cl2 (g) + 2 e- ∅ 2 Cl- +1.36 Fe2+ + 2 e- ∅ Fe (s) -0.41 O2 (g) + 4 H++ 4 e- ∅ 2 H2O +1.23 Zn2+ + 2 e- ∅ Zn (s) -0.76 Cu2+ + 2 e- ∅ Cu (s) +0.34 2 H2O + 2 e- ∅ H2 (g) + 2 OH- -0.83 2H+ + 2 e- ∅ H2(g) 0 Na+ + e- ∅ Na (s) -2.711 Write your name on all 7 pages. This test consists of two parts: Multiple choice and Problems requiring a longer answer. For the multiple choice section, mark one correct answer for each question AND use a #2 pencil to bubble in one correct answer on your Scantron™ form for each question. • Budget your time. Anticipate spending about 50 minutes on each part. • Be sure to leave sufficient time to transfer your multiple choice answers to the Scantron™ form. (for Administrative use only) MC3 2 Total E3 MC2 3 Total E2 1 4 Name_____________________ Page 2 of 2 Part I: Multiple Choice, 3 points each, 54 points total MARK THE CORRECT ANSWER ON YOUR EXAM AND SHADE IN THE BUBBLE OF THE CORRECT ANSWER FOR EACH QUESTION WITH A #2 PENCIL ON YOUR SCANTRON™ FORM. 1.) The answer to question 1 is A. Bubble in A on your Scantron™ form. 2.) Consider the endothermic reaction N2O4 (g) 2NO2 (g) in a sealed vessel. If K1 is the equilibrium constant at 300 K, and K2 is the equilibrium constant at 400 K, which of the following must be true? A) K1 = K2 B) K1 = K2-1 C) K1K2 = Kw D) K1 < K2 E) K2 < K1 3.) What conditions favor the yield of ammonia (NH3) at equilibrium, given the following exothermic reaction: N2 (g) + 3H2 (g) A) High Temperature B) Low Pressure 4.) D) Open Container E) Thermal Insulation B) =3 C) Between 3 and 4 D) = 4 E) > 4 An HAc (weak acid) solution with pH = 3 is diluted by a factor of 10 with water. The new pH is: A) <3 6.) C) High Pressure An HCl (strong acid) solution with pH=3 is diluted by a factor of 10 with water. The new pH is: A) <3 5.) 2NH3 (g) B) =3 C) Between 3 and 4 D) = 4 E) > 4 A sealed can half full of soda expands on a warm day. The reaction below is: CO2 (aq) A) isothermal B) exothermic CO2 (g) C) endothermic D) basic E) acidic 7.) An electrically conducting solution of Ba(OH)2 (a soluble salt) is titrated with H2SO4 until the conductance is at a minimum. (Ksp for BaSO4 = 1.1x10-10) At this point: A) [Ba2+]=[SO42-] B) [Ba2+]<[SO42-] C)[SO42-]<[Ba2+] D) [H3O+]<[OH-] E) [OH-]<[H3O+] Name_____________________ Page 3 of 3 -8 mole speck of AgCl (K = 1.6 x 10-10) is added to 1.0 L of H O. What is [Ag+] in the 8.) A 1.0 x 10 sp 2 resulting solution? A) 1.0 x 10-16 M 9.) B) 1.6 x 10-10 M C) 1.0 x 10-8 M D) 1.3 x 10-5 M E) 1.0 x 10-4 M Under what conditions will a reaction with ∆H° > 0 and ∆S° < 0 be spontaneous? A) High T B) Low T C) All T D) No T E) Can’t determine 10.) It snows in the winter (low temperature) but it rains in the summer (high temperature). This implies that for the formation of snow (H2O (l) H2O (s)): A) H°>0, ∆S°>0 B) ∆H°<0, ∆S°>0 C) ∆H°>0, ∆S°<0 D) ∆H°<0, ∆S°<0 E) Can’t determine 11.) A balloon, containing an ideal gas at 25 °C and 2 atm, adiabatically (q=0) expands to twice its original volume against an external pressure of 1 atm; the final temperature is: Ideal Gas V=X at 25°C A) < 25 °C B) = 25 °C Pext=1atm C) > 25 ° Ideal Gas V=2X D) = -RlnKp E) Can’t determine 12.) An ideal gas at 25 °C and 2 atm adiabatically (q=0) expands into a vacuum to twice its original volume, the final temperature is: Ideal Gas V = X Vacuum at 25C A) < 25 °C B) = 25 °C Ideal Gas V = 2X C) > 25 ° D) = -RlnKp E) Can’t determine 13.) A beam of blue light (400 nm) will eject electrons from an unknown metal surface while a beam of red light (700 nm) will not eject electrons. Will a beam of green light (475 nm) eject electrons from the same surface? A) No B) Sometimes C) Yes D) Only at high intensity E) Can’t determine Name_____________________ Page 4 of 4 14.) A photon of blue light with a wavelength of 400 nm splits into two identical infrared photons. Knowing that energy is conserved, what is the wavelength of each of these two photons? A) 200 nm 15.) D) 566 nm E) 800 nm B) Cl- C) Cu+2 D) O2 (g) E) Cl2 (g) Which of the following will be oxidized by Fe2+ but not by Na+ under standard conditions? A) Cl2 17.) C) 400 nm Which one of the following species is the strongest oxidizer under standard conditions? A) Mn2+ 16.) B) 283 nm C) Na+ B) Zn E) Cl- D) Sn Which of the following is a product of the reaction when NaCl is added to an acidic MnO4- solution? A) Cl2 B) Cl- C) Na D) H+ E) H2 18.) Aluminum (Al) produces H2 bubbles when immersed in HCl, mercury (Hg) does not. Which is the strongest reducer? A) Al3+ 19.) B) Al C) Hg D) Hg+ E) H2 Buried copper (Cu) pipes are often fitted with zinc (Zn) strips; why? A) To prevent oxidation of Cu B) To prevent reduction of Cu D) Zn is acid resistant C) Zn is shinier E) Zn is base resistant Name_____________________ Page 5 of 5 Part II: 4 Problems, 46 points total SHOW ALL OF YOUR WORK AND USE UNITS IN YOUR CALCULATIONS. PARTIAL CREDIT IS AVAILABLE, SO ATTEMPT EACH PART OF EACH QUESTION EVEN IF YOU WERE UNABLE TO DO THE PREVIOUS PART(S). (10 pts) 1.) Phosgene (COCl2) is a poisonous gas. At 425 K it will dissociate to establish the following equilibrium: COCl2 (g) CO (g) + Cl2 (g) K= 1.00 x 10-4 a.) Starting with pure COCl2 gas at PCOCl2 = 2.00 atm, when the system reaches equilibrium the total pressure (in atm) will be: (circle the correct answer) A) = 1.00 B) Between 1.00 and 2.00 C) = 2.00 D) Between 2.00 and 4.00 E) = 4.00 b.) Calculate the partial pressure of CO for the equilibrium system of part a.). Justify any assumptions made. PCO = _____________ c.) The container for the equilibrium system of part a.) is doubled in volume. When the system reaches the new equilibrium state the total pressure (in atm) will be: (circle the correct answer) A) = 1.00 B) Between 1.00 and 2.00 C) = 2.00 D) Between 2.00 and 4.00 E) = 4.00 d.) Calculate the partial pressure of CO for the new equilibrium system of part c.). Justify any assumptions made. PCO = _____________ Name_____________________ Page 6 of 6 (9pts) 2a.) Starting with a 1.0 liter solution of 1.0 M sodium acetate (Ac-), how many moles of HCl do you need to add to make a buffer with pH= 4.75? (For HAc pKa = 4.75 ). Show your work. Moles HCl = _____________ b.) To 1.0 L of buffer solution (pH=pKa) produced in part a.) 9.0 L of H2O are added, what is the new pH? Show your work. pH = _____________ c.) How many moles of acetic acid (HAc) must be added to H2O to make 1.0 L of a solution with pH = 4.75? Show your work. Moles HAc = _____________ Name_____________________ Page 7 of 7 (12pts) 3.) You make the following observation: • Addition of tin metal (Sn) to a solution of silver ions (Ag+) results in the formation of Ag and Sn2+. a.) Write a balanced equation for the net spontaneous reaction that describes this observation. b.) Will Ag reduce Sn2+? Explain. c.) For the standard cell Sn (s) | Sn2+ (1.0 M) || Ag+ (1.0 M) | Ag (s) when current flows, at which electrode, Sn or Ag, does oxidation occur? Explain in terms of electron flow for the operating cell. d.) In the operating cell in part c.), for each mole of anode (- electrode) that dissolves, how many moles of metal plate out onto the cathode (+ electrode)? Explain. Moles = _____________ Name_____________________ Page 8 of 8 (15 pts) 4.) A study of the ancient geology of the earth shows that rocks greater than 2 billion years old contain iron in the form of FeS2. In rocks less than 2 billion years old, iron appears mostly in the oxidized form Fe2O3 (hematite). 4FeS2 (s) + 8H2O (l) + 15O2 (g) 2Fe2O3 (s) + 8H2SO4 (l) a.) Calculate ∆H° for the above reaction. ∆H° = _____________ b.) Calculate ∆S° for the above reaction. ∆S° = _____________ c.) Over what temperature range is the reaction spontaneous? Show your calculations. From T = ___________ to ___________ ...
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This note was uploaded on 09/11/2009 for the course CHEM 1A taught by Professor Nitsche during the Spring '08 term at Berkeley.

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