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UH / English / ENGI 1331 / dan burleson uh

dan burleson uh

dan burleson uh

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School: University of Houston
Department: English
Course: Computing for Engineers
Professor: Daniel burleson
Term: Fall 2016
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Cost: 50
Description: Houston Community College System Departmental SAMPLE Final Examination Chemistry 1412B       Cortisone (steroid)- reduces swelling and decreases the body's immune response Final Sample Exam 1412B 1 PART I (2 points each) Multiple choice - Please DO NOT write or mark on this paper
Uploaded: 06/26/2017
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 Houston Community College System Departmental  SAMPLE  Final Examination Chemistry 1412B     Cortisone (steroid)- reduces swelling and decreases the body's immune response


What is the equilibrium constant for 4 HI(g) ↔ 2 H2(g) + 2 I2(g) under the saWe also discuss several other topics like gsu grade distribution
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Final Sample Exam 1412B 1PART I (2 points each) Multiple choice - Please DO NOT write or mark on this paper. Write your correct answer  on scantron. 1. In the reaction, HSO4- + HS- ↔ H2S + SO42- , which one of the sets below constitutes a conjugate (acid-  base) pair?  A) HSO4-, HS- B) HSO4- , H2S C) H2S , HS- D) HS-, SO42-  2. Which one of the species below is insoluble in water?  A) ZnSO4 B) PbCrO4 C) AgNO3 D) NaC2H3O2  3. A glucose solution is prepared by dissolving 5.10 g of glucose, C6H12O6, in 110.5 g of water. What is the   molality of the glucose solution?    A) 0.283 m B) 0.000256 m C) 0.245 m D) 0.256 m  4. What is the expected freezing point of a solution that contains 25.0g of fructose, C6H12O6, in 250.0g of   water? Ki = 1.86 °C m-1  A) -0.10°C B) +0.10°C C) -1.03°C D) +1.86°C 5. Which of the following reactions accompanied by an increase in entropy?  A) ZnS(s) + 3/2 O2(g) → ZnO(s) + SO2(g) B) CH4(g) + H2O(g) → CO(g) + 3H2(g)  C) BaO(s) + CO2(g) → BaCO3(s) D) Na2CO3(s) + CO2(g) + H2O(g) → 2 NaHCO3(s) 6. The nuclear particle which is described by the representation, 11 X, is called:   A) alpha particle B) electron C) neutron D) proton  7. Butene, C4H8, is a hydrocarbon with one bond. How many noncyclic isomers can be drawn?  A) 1 B) 2 C) 3 D) 4  8. If the OH- ion concentration in an aqueous solution at 25.0 oC is measured as 3.4 x 10-3 M, then the pH is?    A) 2.47 B) 7.22 C) 8.24 D) 11.53   9. A galvanic cell has two electrodes. Which statement below is correct?  A) Reduction takes place at the anode, which is positively charged.  B) Reduction takes place at the anode, which is negatively charged.  C) Reduction takes place at the cathode, which is positively charged.  D) Reduction takes place at the cathode, which is negatively charged. 10. If a reaction involves a single reactant is first order with a rate constant of 4.50× 10-2 s-1, how much   time is required for 75.0% of the initial quantity of reactant to be used up? 2 A) 16.7 seconds B) 30.8 seconds C) 23.1 seconds D) 25.3 seconds  11. For the reaction, 2XO + O2  2 XO2, some data obtained from measurements of the initial rate of   reaction at varying concentrations is given below.  Run # [XO] [O2] rate, mmol L-1 s-1  1 0.010 0.010 2.5  2 0.010 0.020 5.0  3 0.030 0.020 45.0  The rate law is therefore:    A) rate = k[XO]2[O2] B) rate = k[XO] [O2] C) rate = k[XO] [O2]2 D) rate = k[XO]2 [O2]2    12. Which one of the following is the strongest acid?  A) HClO (Ka = 3.0 x 10-8) B) HF (Ka = 6.8 x 10-4)  C) HNO2 (Ka = 4.5 x 10-4) D) HCN (Ka = 4.9 x 10-10) 13. Using the standard entropy values:  H2(g), So = + 130.6 J mol-1 K-1 I2(s), So = + 116.12 J mol-1 K-1 HI(g), So = + 206.5 J mol-1 K-1  Calculate the standard entropy change, ∆So, for the reaction: H2(g) + I2(g) → 2 HI(g)  A) -40.8 J B) +40.8 J C) -165.3 J D) +165.3 J  14. Consider the following reaction at equilibrium:  2NH3(g)  N2(g) + 3H2(g) ΔH° = + 92.4 kJ  Adding H2(g) to the system at equilibrium will ____________________  A) decrease the concentration of NH3(g) at equilibrium  B) remove all of the N2(g)  C) increase the value of the equilibrium constant  D) decrease the concentration of N2(g) at equilibrium 15. The equilibrium constant for the reaction, H2(g) + I2(g) ↔ 2 HI(g) is 54.9 at 699.0 K. What is the   equilibrium constant for 4 HI(g) ↔ 2 H2(g) + 2 I2(g) under the same condition?  A) 109.8 B) 9.11 x 10-3 C) 3.32 x 10-4 D) -109.8  16. A 0.400 M solution of an acid, HA, has a pH = 1.301. What is the value of the ionization constant, Ka, for   this acid?    A) 5.00 x 10-2 B) 1.25 x 10-3 C) 5.56 x 10-3 D) 6.25 x 10-3  317. What is the balanced form of the following unbalanced redox equation that takes  place in an   acidic medium? NO2-(aq) + Cr2O72-(aq) → Cr3+(aq) + NO3-(aq) A) NO2-(aq) + Cr2O72-(aq) + 8H+(aq) → 2Cr3+(aq) + NO3-(aq) + 4H2O(l) B) 3NO2-(aq) + Cr2O72-(aq) → 2Cr3+(aq) + 3NO3-(aq) + 4H2O(l) C) 3NO2-(aq) + Cr2O72-(aq) + 8H+(aq) → 2Cr3+(aq) + 3NO3-(aq) + 4H2O(l) D) 3NO2-(aq) + Cr2O72-(aq) + 16H+(aq) → 2Cr3+(aq) + 3NO3-(aq) + 8H2O(l) 18. A buffer solution is prepared by taking 0.250 moles of acetic acid ( pKa = 4.74) and 0.400 moles of sodium  acetate in sufficient water to make 1.800 liters of solution . Calculate the pH.  A) 4.95 B) 4.66 C) 4.86 D) 4.56  19. Oxidation refers to ______ electrons, reduction refers to ________ of electrons.  A) Gain; gain B) Loss; gain C) Neutralization; loss D) Gain; loss 20. 40.0 ml of 0.10 M HCl(aq) was added to 50.0 ml of 0.10 M NaOH(aq) and the mixture was stirred, then   tested with a pH meter. What pH should be obtained at 25.0 oC?  A) 1.95 B) 12.05 C) 7.00 D) 12.50  21. What element undergoes alpha decay to form lead-208 ( Pb)?  82  222 131  A) Radon (Rn) B) Xenon(Xe)  86 54  84 212  C) Krypton (Kr) D) Polonium (Po)  36 84   22. The solubility of silver oxalate, Ag2C2O4, in pure water is 2.06 x 10-4 moles per liter. Calculate the value of   Ksp for silver oxalate from this data.  A) 4.24 x 10-8 B) 8.49 x 10-8 C) 1.75 x 10-11 D) 3.50 x 10-11  23. Hydrocarbons containing a carbon-carbon triple bond are called _____________ .  A) alkanes B) alkenes C) alkynes D) cyclic alkanes  24. The half-life of cobalt-60 is 5.3 yr. How much of a 1.000-mg sample of cobalt-60 is left after a 10.6yr   priod? A) 0.250mg B) 0.100mg C) 0.990mg D) 0.125mg 25. Which of the following salts has a cation that can hydrolyze in water?  A) NaCl B) Ca(NO3)2 C) Ba(C2H3O2)2 D) NH4Cl 426. The unit of the rate constant for a second order reaction could be _______.  A) M-1 s-1 B) M C) M s-1 D) M2s-1 27. For the reaction: A(g) + 2B(g)  4C(g), ΔG° = 77.8 kJ. If the reaction mixture consists of 2.0 atm A,   4.0 atm B, and 2.5 atm C at 298 K, calculate the ΔG for this reaction mixture at 298 K. (R=8.314 J/molK).   A) 78.3 kJ B) 7.89 kJ C) –7.89 kJ D) -34.2 kJ 28. A galvanic cell is composed of these two half cells, with the standard reduction   potentials shown  Zn2+(aq) + 2e- ↔ Zn(s) -0.76 volt  Cd2+(aq) + 2e- ↔ Cd(s) -0.40 volt  What is the standard free energy for the cell reaction of this galvanic cell?  A) -69 KJ B) +69 KJ C) -224 KJ D) +224 KJ  29. The reaction 2H2O2  2H2O + O2 has the following mechanism? H2O2 + I–  H2O + IO– H2O + IO–  H2 + O2 + I–  The intermediates in the reaction are:   A) H2O and IO– B) H2O2 and I–  C) H2O2 and IO– D) IO– and I– 30. Name the following compound according to IUPAC system:  CH3  ⏐ CH3⎯CH⎯CH⎯CH2⎯CH3  ⏐ CH2CH3 A) 2,3-dimethylhexane B) 3-ethyl-2,4-dimethylheptane C) 3-ethyl-2-methylheptane D) None of the above 31. The system, H2 (g) + X2 (g) ↔ 2 HX(g) has a value of 24.4 for the constant, Kc. A system being tried   in a 3.00 liter reactor was charged with 0.150 moles of H2, 0.150 moles of X2 and, 0.600 moles of HX. The   catalyst was introduced using a remote unit, and the system was allowed to come to equilibrium. Which   statement below describes the situation?  A) the reaction goes to the right, Q ‹ K B) the reaction goes to the left, Q ‹ K     C) the reaction goes to the right, Q › K D) the reaction goes to the left, Q › K  32. A solution is made by mixing 138.2 grams of ethanol, C2H6O, (46.069 g mol-1), 103.6 gram of water   (18.015 g mol-1), and 80.11 grams of methanol, CH4O, (32.0042 g mol-1). What is the mole fraction of   methanol in the mixture?  A) 0.02504 B) 0.2224 C) 0.2493 D) 0.3333  533. A Lewis base is defined as a substance that  A) acts as a proton donor B) increases [H+] when placed in H2O  C) decreases [OH–] when placed in H2O D) acts as a electron pair donor 34. The standard reduction potentials for the following half reactions are given as follows;  Cr+3 +3e-  Cr(s) E0 = - 0.73 V  Br2(aq) + 2e-  2Br- E0 = + 1.09 V  What is the E0 for this cell?  A) 1.82 V B) 0.36 C) 4.75 V D) 1.79 V 35. Classify the following molecule: O  CH3- CH2- CH2- C O -CH3 A) ester B) aldehyde C) ketone D) carboxylic acid     6Name :__________________________ Part II-( 5 points each) Show work- Please write your complete work in space provided. Partial credit will be given. 1. Solution made by dissolving 6.73 grams of toluic acid in 110 grams of benzene ( f.p. = 5.45oC, Kf = 5.07   oC/m) gave a freezing point of 3.00 oC. What is the calculated molecular weight of toluic acid form this   data?  2. The gas phase decomposition of HI, HI(g) → 1/2H2(g) + 1/2I2(g) , has the rate equation,   -∆ [HI] / ∆t = K[HI]2 where K=30.0 L/mol. min at 443°C. How much time does it take for the   concentration of HI to drop from 0.010 mol/L to 0.0050 mol/L at 443°C? 3. Ka for hypochlorous acid, HClO, is 3.0x10-8.  a. Calculate the pH after addition of 15.0 ml of 0.100 M NaOH to 40.0 ml of 0.100 M HClO.  b. Identify the pH at half equivalent point. 74. Assuming that the value of ∆H and ∆S do not change with temperature, and using the following data,  CaO(s), ∆Hfo = -635.5 KJ mol-1, So = +40.0 J mol-1 K-1  CaCO3(s), ∆Hfo = -1207 KJ mol-1, So = +92.9 J mol-1 K-1  CO2(g), ∆Hfo = -394 KJ mol-1, So = +213.6 J mol-1 K-1  Calculate the value for the free energy change, ∆Gofor the reaction,  CaCO3(s) → CaO(s) + CO2(g) at 815 Co 5. Aluminum metal is oxidized in aqueous base with water serving as the oxidizing agent.  Al(s) + H2O(1) → Al(OH)4- + H2(g) (basic solution)     Write a balanced equation for this reaction in basic solution. 6. Refer to the following half-reactions below;   MnO4- + 8H+ + 5e-  Mn2+ + 4H2O E0 = 1.51 V  Cr2O72- + 14H+ + 6e-  2Cr3+ + 7H2O E0 = 1.33 V  Calculate the value of equilibrium constant at 25 0C for this reaction?  8CHEMISTRY FINAL CHEM 1412B EXAM(answers) PART - I 1. C 2. B 3. D 4. C 5. B 6. D 7. C 8. D 9. C 10. B 11. A 12. B 13. D 14. D 15. C  16. D 17. C 18. A 19. B 20. B 21. D 22. D 23. C 24. A 25. D 26. A 27. A 28. A 29. A 30. D  31. A32. B 33. D 34. A 35. A    PART - II 1. ∆Tf = kf x m = kf x (n/kg) = (kf x m)/(Mxkg); M = (kf x m)/(∆Tf x kg) M = 136.15 g/mol   2. t = (1/k) x ((1/[A]t ) – (1/[A]o))  t = (1/30) x ((1/0.005) – (1/0.01))  t = 3.33 min. 3. a. pH = pKa + log((1.5x10-3)/(2.5x10-3))   pH = 7.30  b. At ½ equivalent point pH = pKa   pH = 7.52 4. ∆Ho = 177.5 kJ  ∆So = 160.7 J  ∆Go = ∆Ho - T∆So  ∆Go = 177.5 kJ - 1088.15 x 160.7 x 10-3 kJ   ∆Go = 2.634 kJ  5. 2Al + 6H2O + 2OH-  2Al(OH) 4- + 3H2 6. ∆G = ∆Go + RT Ln Q   E = Eo – (RT/nF)Ln Q   E = Eo – (0.0592/n)Log Q  at equilibrium, E= 0, and Q = Keq.  Log Keq. = n Eo /0.0592 = 30 x (151 – 1.33)/0.0592  Log Keq. = 91.2;  Keq. = 1.58x1091   9
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