Houston Community College System Departmental SAMPLE Final Exam Chemistry 1412A

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1 Houston Community College System Departmental SAMPLE Final Exam Chemistry 1412A 1

2 Final Sample Exam 1412A PART I (2 points each) Multiple choice - Please DO NOT write or mark on this paper. Write your correct answer on scantron. 1. In which colligative property (ies) does the value decrease as more solute is added? A. boiling point B. freezing point C. vapor pressure D. freezing point and vapor pressure 2. What is the molarity of a solution prepared by dissolving 25.2 g CaCO 3 in 600. ml of a water solution? A M B M C M D M 3. What is the freezing point of an aqueous glucose solution that has 25.0 g of glucose, C 6 H 12 O 6, per g H 2 O (K f = 1.86 C /m)? A B C D What is the osmotic pressure in atm produced by a 1.20 M glucose (C 6 H 12 O 6 ) solution at 25 C? A B C D The vapor pressure of pure ethanol at 60 C is 349 mm Hg. Calculate vapor pressure in mm Hg at 60 C for a solution prepared by dissolving 10.0 mol of naphthalene (nonvolatile) in 90.0 mol of ethanol? A. 600 B. 314 C D For first-order reactions the rate constant, k, has the units A. M s -1 B. M -1 s -1 C. M -2 s -1 D. s For second-order reactions the slope of a plot of 1/[A] versus time is A. k B. k/[a] 0 C. kt D. -k 8. If the reaction 2A + 3D products is first-order in A and second- order in D, then the rate law will have the form rate = A. k[a] 2 [D] 3 B. k[a][d] C. k[a] 2 [D] 2 D. k[a][d] 2 9. In the first-order reaction A products the initial concentration of A is 1.56 M and the concentration is M after 48.0 min. What is the value of the rate constant, k, in min -1? A x 10-2 B x 10-2 C x 10-2 D x

3 10. Consider the reaction 2HI(g) H 2 (g) + I 2 (g). What is the value of the equilibrium constant, K c, if at equilibrium, [H 2 ] = 6.50 x 10-7 M, [I 2 ] = 1.06 x 10-5 M, and [HI] = 1.87 x 10-5 M? A x 10-7 B x 10-2 C x D Given the following mechanism, determine which of the species below is a catalyst? I) C + ClO 2 ClO + CO II) CO + ClO 2 CO 2 + ClO III) ClO + O 2 ClO 2 + O IV) ClO + O ClO 2 A. ClO 2 B. CO 2 C. O D. CO 12. For the system CaO(s) + CO 2 (g) CaCO 3 (s) the equilibrium constant expression for K eq is A. [CO 2 ] B. 1 / [CO 2 ] C. [CaO] [CO 2 ] / [CaCO 3 ] D. [CaCO 3 ] / [CaO] [CO 2 ] 13. The value of K p for the reaction 2NO 2 (g) N 2 O 4 (g) is 1.52 at 319 K. What is the value of K p at this temperature for the reaction N 2 O 4 (g) 2NO 2 (g)? A B C x 10-4 D Which of the following is true for the cell shown here? Zn (s) Zn 2+ (aq) Cr 3+ (aq) Cr (s) A. the electrons flow from cathode to the anode B. the electrons flow from the zinc to the chromium C. the electrons flow from the chromium to the zinc D. the zinc is reduced 15. How many electrons are transferred in the following reaction? 2ClO H I - 5I 2 + Cl 2 + 6H 2 O A. 10 B. 12 C. 5 D A voltaic cell has an E 0 value of V. The reaction : A. is not spontaneous B. has K =1 C. has a negative G 0 D. has G 0 = Which energy conversion below takes place in a galvanic cell? A. electrical to chemical B. chemical to electrical C. mechanical to chemical D. electrical to mechanical 18. The value of K c for the reaction C(s) + CO 2 (g) 2CO(g) is 1.6. What is the equilibrium concentration of CO if the equilibrium concentration of CO 2 is 0.50 M? A B C D Consider the reaction below: 2SO 3 (g) 2SO 2 (g) + O 2 (g), H = +198 kj All of the following changes would shift the equilibrium to the left except one. Which one would not cause the equilibrium to shift to the left? A. removing some SO 3 B. decreasing the temperature C. increasing the container volume D. adding some SO 2 3

4 20. Calculate the ph of a solution if its [OH ] = M and indicate whether the solution is acidic, basic, or neutral. A. 3.15, acidic B. 17.2, basic C. 10.8, basic D. 11, basic 21. Which one of the conjugate bases of the following Brønsted-Lowry acids are incorrect? A. ClO - for HClO B. HS - for H 2 S C. H 2 SO 4 for HSO 4 - D. NH 3 for NH Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral. Find the incorrect answer. A. KNO 3 ( neutral) B. NaC 2 H 3 O 2 ( basic) C. KClO (acidic) D. NaCN (basic) 23. Calculate the ph of a buffer that is 0.20 M in formic acid and 0.15 M in sodium formate (K a = 1.8 x 10-4 ). A. 2.4 x 10-4 B C D If X is the solubility of a salt in moles per liter, which one of the following K sp expressions is incorrect? A. Ag 2 S, K sp = 4X 3 B. AgCl, K sp = X 2 C. BaSO 4, K sp = 4 X 2 D. Cu(OH) 2, K sp = 4X For each of the following processes, predict whether entropy, S, is positive or negative: (i) 2K(s) + Br 2 (l) 2KBr(s), (ii) 2MnO 2 (s) 2MnO(s) + O 2 (g) A. (i) positive, (ii) positive B. (i) negative, (ii) positive D. (i) positive, (ii) negative D. (i) negative, (ii) negative 26. Using the given values of S ( J/mol.K), calculate the value of S for the reaction, C 2 H 4 (g) + H 2 (g) C 2 H 6 (g) S 0 = A J/ K B J/ K C J/ K D J/ K 27. Consider a galvanic cell based on the reaction below, what is the coefficient of Fe 3+ in the balanced equation in acidic solution? Fe 2+ + Cr 2 O 7 2- Fe 3+ + Cr 3+ A. 1 B. 2 C. 3 D The standard reduction potentials for the following half reactions are given as follows; Cr e - Cr (s) Br 2 + 2e - 2Br - E 0 = V E 0 = V What is the E 0 for a voltaic cell using these reactions? A V B V C V D V 4

5 29. Which of the following represents positron? A. 1 1 H B. 0-1 e C e D. 4 2 He 30. Which of the following balanced equation is labeled incorrectly? A. Beta decay, U Np e B. Alpha Bombardment, Na He Al n C. Electron capture, 7 4 Be + 0-1e 7 3 Li D. All are correctly labeled 31. Which of the following pairs is incorrect? A. ethane - C 2 H 6 B. hexane - C 6 H 14 C. decane - C 10 H 22 D. heptane - C 7 H Which of the following is general formula for alkene with n-carbon atoms? A. C n H n B. C n H 2n+2 C. C n H 2n D. C n H 2n Classify the following molecule; CH 3 -CH 2 - C= O OCH 3 A. ester B. aldehyde C. ketone D. carboxylic acid 34. What is the correct IUPAC name the following compound; Cl CH 2 CH 3 C=C H 3 C Cl A. cis-2-chloro-3-chloro-2-pentene B. 2,3-dichloro-1-methylbutene C. trans-2,3-dichloro-2-pentene D. 1-chloro-2-methylbutene 35. Which of the following is correct condensed formula for isopropanol A. CH 3 - CH 2 -CH 2 OH B. CH 3 -CH -CH 3 CH 3 OH C. CH 3 - C -CH 2 OH D. CH 3 - H 2 C = CH-OH CH 3 5

6 Part II-( 5 points each) Name: Show work- Please write your complete work in space provided. Partial credit will be given. 1. A solution is prepared by dissolving 6.00 g of an unknown nonelectrolyte in enough water to make 1.00 L of solution. The osmotic pressure of this solution is atm at 25.0 C. What is the molecular weight of the unknown solute (R = L atm/k mol)? 2. Initial rate data were obtained for the following reaction: A(g) + 2B(g) C(g) + D(g) initial initial initial Experiment [A], mol/l [B], mol/l rate,ms What are the rate law and k value for the reaction? 3. If the ph of a solution is 6.30, what are the molar concentrations of H + (aq), OH (aq), and poh in the solution? 6

7 4. A 50.0-mL sample of 0.50 M acetic acid, CH 3 COOH, is titrated with a M NaOH solution. Calculate the ph after 25.0 ml of the base have been added (K a = 1.8 x 10 5 ). 5. If a constant current of 5.0 amperes is passed through a cell containing Cr 3+ for 1.0 hour, how many grams of Cr will plate out on to the cathode? (the atomic mass of Cr is and 1 Faraday = coulombs) 6.The half-life of Sr-90 1s 28.1 years. How long will it take a 10.0 g sample of Sr-90 to decompose to 0.10 g? 7

8 CHEMISTRY FINAL CHEM 1412A EXAM(answers) Part I -Multiple Choice Questions (2 points each) 1. D 2. A 3. D 4. A 5. B 6. D 7. A 8. D 9. D 10. B 11. A 12. B 13. D 14. B 15. A 16. C 17. B 18. C 19. C 20. C 21. C 22. C 23. B 24.C 25. B 26. A 27. D 28. A 29. C 30. D 31. D 32. C 33. A 34. C 35. B Part II Show work 1. (0.750 atm) π = MRT and M = π /RT = = M ( L-atm/mol-K)(298K) n mass unk mass unk (6.00 g) M = n = MxV = MW unk = = = 196 g/mol V MW unk MxV (0.0307M)(1.00L) OR: (g) ( R) (T) (6.00) (0.0821) ( 298) MW = = = 196 g/mol π V (0.750) ( 1.00) 2. EXP 1 & 2: Concentration of A is doubled, concentration of B is kept constant, initial rate increases by a factor of 4. That means that the reaction is second order in A. EXP 1 & 3: Concentration of A is kept constant, concentration of B is doubled, initial rate increases by a factor of 2. That means that the reaction is first order in B. Rate = k [A] 2 [B] EXP 1: 0.45 Ms -1 = k (0.15M) 2 (0.10M) k = 200 M -2 s ph = 6.30 [H + ] = antilog (-6.30) = 5.01 x 10-7 M poh = = 7.70 [OH - ] = antilog(-7.70) = 1.90 x 10-8 M OR: [H + ] = 10 ph = = 5.01 x 10-7 M, poh = = 7.70 [OH - ] = 10 poh = = = 1.90 x 10-8 M 4. mol CH3COOH = 0.50Mx0.050L = 0.025mol, mol NaOH = 0.15Mx0.025L = 3.75x10-3 mol CH 3 COOH(aq) + NaOH(aq) NaC 2 H 3 O 2 (aq) + H 2 O(l) Initial: (0.025 mol) (3.75x10-3 mol) 0 0 Change: -(3.75x10-3 mol) -(3.75x10-3 mol) (3.75x10-3 mol) (3.75x10-3 mol) Final: (2.13x10-2 mol) 0 (3.75x10-3 mol) (3.75x10-3 mol) CH 3 COOH(aq) + H 2 O(l) CH 3 COO - (aq) + H 3 O + (l) (2.13x10-2 mol) M CH3COOH = = 0.283M (0.075L) [CH 3 COO - ] ph= pk a + log = 3.98 (3.75x10-3 mol) [CH 3 COOH] M CH3COO = = 0.05M (0.075L) OR: M a = M(acid) = ( MaVa/Vtot) = (0.50)(0.05)/0.075 = 0.33 M Mb = M(base) = (MbVb/Vtot) = (0.15)(0.025)/0.075 = 0.05 M PK a = -logk a = -log (1.85x10 5 ) = 4.73 For weak acid strong base ; PH = PK a + log [Mb] / [Ma - Mb] = log [0.05] / [ ] = = Charge = (5.0Amp)(3600sec) = 18,000C Moles of e - = 18,000C x (1 mol e - /96485C) = mol e - = mol Cr mol Cr = g Cr OR : Mass ( g Cr) = ( M/n) ( It/F) = ( 52/3) (5x3600/96485) = g Cr 6. k =( 0.693/28.1yr) = 2.47 x 10-2 yr -1 ln[0.10] = -(2.47 x 10-2 yr -1 )(t) + ln[10.0] t = 186 yr. OR: t = (3.32)(t½ ) ln ( m o / m n ), t = ( 3.32) ( 28.1) log ( 10.0/0.10), t = 186 yr. 8

9 Houston Community College System Departmental SAMPLE Final Exam Chemistry 1412B Cortisone (steroid)- reduces swelling and decreases the body's immune response 9

10 Final Sample Exam 1412B PART 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, HSO HS - H 2 S + SO 4 2-, which one of the sets below constitutes a conjugate (acidbase) pair? A) HSO 4 -, HS - B) HSO 4 -, H 2 S C) H 2 S, HS - D) HS -, SO Which one of the species below is insoluble in water? A) ZnSO 4 B) PbCrO 4 C) AgNO 3 D) NaC 2 H 3 O 2 3. A glucose solution is prepared by dissolving 5.10 g of glucose, C 6 H 12 O 6, in g of water. What is the molality of the glucose solution? A) m B) m C) m D) m 4. What is the expected freezing point of a solution that contains 25.0g of fructose, C 6 H 12 O 6, in 250.0g of water? K i = 1.86 C m -1 A) C B) C C) C D) C 5. Which of the following reactions accompanied by an increase in entropy? A) ZnS(s) + 3/2 O 2 (g) ZnO(s) + SO 2 (g) B) CH 4 (g) + H 2 O(g) CO(g) + 3H 2 (g) C) BaO(s) + CO 2 (g) BaCO 3 (s) D) Na 2 CO 3 (s) + CO 2 (g) + H 2 O(g) 2 NaHCO 3 (s) 6. The nuclear particle which is described by the representation, 1 1 X, is called: A) alpha particle B) electron C) neutron D) proton 7. Butene, C 4 H 8, 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 o C is measured as 3.4 x 10-3 M, then the ph is? A) 2.47 B) 7.22 C) 8.24 D) 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

11 10. If a reaction involves a single reactant is first order with a rate constant of s -1, how much time is required for 75.0% of the initial quantity of reactant to be used up? A) 16.7 seconds B) 30.8 seconds C) 23.1 seconds D) 25.3 seconds 11. For the reaction, 2XO + O 2 2 XO 2, some data obtained from measurements of the initial rate of reaction at varying concentrations is given below. The rate law is therefore: Run # [XO] [O 2 ] rate, mmol L -1 s A) rate = k[xo] 2 [O 2 ] B) rate = k[xo] [O 2 ] C) rate = k[xo] [O 2 ] 2 D) rate = k[xo] 2 [O 2 ] Which one of the following is the strongest acid? A) HClO (K a = 3.0 x 10-8 ) B) HF (K a = 6.8 x 10-4 ) C) HNO 2 (K a = 4.5 x 10-4 ) D) HCN (K a = 4.9 x ) 13. Using the standard entropy values: H 2 (g), S o = J mol -1 K -1 I 2 (s), S o = J mol -1 K -1 HI(g), S o = J mol -1 K -1 Calculate the standard entropy change, S o, for the reaction: H 2 (g) + I 2 (g) 2 HI(g) A) J B) J C) J D) J 14. Consider the following reaction at equilibrium: 2NH 3 (g) N 2 (g) + 3H 2 (g) H = kj Adding H 2 (g) to the system at equilibrium will A) decrease the concentration of NH 3 (g) at equilibrium B) remove all of the N 2 (g) C) increase the value of the equilibrium constant D) decrease the concentration of N 2 (g) at equilibrium 15. The equilibrium constant for the reaction, H 2 (g) + I 2 (g) 2 HI(g) is 54.9 at K. What is the equilibrium constant for 4 HI(g) 2 H 2 (g) + 2 I 2 (g) under the same condition? A) B) 9.11 x 10-3 C) 3.32 x 10-4 D) A M solution of an acid, HA, has a ph = 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

12 17. What is the balanced form of the following unbalanced redox equation that takes place in an acidic medium? NO2 - (aq) + Cr2O7 2- (aq) Cr 3+ (aq) + NO3 - (aq) A) NO2 - (aq) + Cr2O7 2- (aq) + 8H + (aq) 2Cr 3+ (aq) + NO3 - (aq) + 4H2O(l) B) 3NO2 - (aq) + Cr2O7 2- (aq) 2Cr 3+ (aq) + 3NO3 - (aq) + 4H2O(l) C) 3NO2 - (aq) + Cr2O7 2- (aq) + 8H + (aq) 2Cr 3+ (aq) + 3NO3 - (aq) + 4H2O(l) D) 3NO2 - (aq) + Cr2O7 2- (aq) + 16H + (aq) 2Cr 3+ (aq) + 3NO3 - (aq) + 8H2O(l) 18. A buffer solution is prepared by taking moles of acetic acid ( pka = 4.74) and moles of sodium acetate in sufficient water to make liters of solution. Calculate the ph. A) 4.95 B) 4.66 C) 4.86 D) Oxidation refers to electrons, reduction refers to of electrons. A) Gain; gain B) Loss; gain C) Neutralization; loss D) Gain; loss 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 o C? A) 1.95 B) C) 7.00 D) What element undergoes alpha decay to form lead-208 ( Pb)? A) Radon (Rn) B) Xenon(Xe) C) Krypton (Kr) D) Polonium (Po) The solubility of silver oxalate, Ag 2 C 2 O 4, in pure water is 2.06 x 10-4 moles per liter. Calculate the value of K sp for silver oxalate from this data. A) 4.24 x 10-8 B) 8.49 x 10-8 C) 1.75 x D) 3.50 x 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 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(NO 3 ) 2 C) Ba(C 2 H 3 O 2 ) 2 D) NH 4 Cl 12

13 26. 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) M 2 s For the reaction: A(g) + 2B(g) 4C(g), G = 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 G 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) kj 28. A galvanic cell is composed of these two half cells, with the standard reduction potentials shown Zn 2+ (aq) + 2e - Zn(s) volt Cd 2+ (aq) + 2e - Cd(s) 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 2H 2 O 2 2H 2 O + O 2 has the following mechanism? H 2 O 2 + I H 2 O + IO H 2 O + IO H 2 + O 2 + I The intermediates in the reaction are: A) H 2 O and IO B) H 2 O 2 and I C) H 2 O 2 and IO D) IO and I 30. Name the following compound according to IUPAC system: CH 3 CH 3 CH CH CH 2 CH 3 CH 2 CH 3 A) 2,3-dimethylhexane B) 3-ethyl-2,4-dimethylheptane C) 3-ethyl-2-methylheptane D) None of the above 31. The system, H 2 (g) + X 2 (g) 2 HX(g) has a value of 24.4 for the constant, K c. A system being tried in a 3.00 liter reactor was charged with moles of H 2, moles of X 2 and, 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 grams of ethanol, C 2 H 6 O, ( g mol -1 ), gram of water ( g mol -1 ), and grams of methanol, CH 4 O, ( g mol -1 ). What is the mole fraction of methanol in the mixture? A) B) C) D)

14 33. A Lewis base is defined as a substance that A) acts as a proton donor B) increases [H + ] when placed in H 2 O C) decreases [OH ] when placed in H 2 O 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) E 0 = V Br 2(aq) + 2e - 2Br - E 0 = V What is the E 0 for this cell? A) 1.82 V B) 0.36 C) 4.75 V D) 1.79 V 35. Classify the following molecule: O CH 3 - CH 2 - CH 2 - C O -CH 3 A) ester B) aldehyde C) ketone D) carboxylic acid 14

15 Part II-( 5 points each) Name : 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. = 5.45 o C, K f = 5.07 o C/m) gave a freezing point of 3.00 o C. What is the calculated molecular weight of toluic acid form this data? 2. The gas phase decomposition of HI, HI(g) 1/2H 2 (g) + 1/2I 2 (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 mol/l to mol/l at 443 C? 3. K a for hypochlorous acid, HClO, is 3.0x10-8. a. Calculate the ph after addition of 15.0 ml of M NaOH to 40.0 ml of M HClO. b. Identify the ph at half equivalent point. 15

16 4. Assuming that the value of H and S do not change with temperature, and using the following data, CaO(s), H f o = KJ mol -1, S o = J mol -1 K -1 CaCO 3 (s), H f o = KJ mol -1, S o = J mol -1 K -1 CO 2 (g), H f o = -394 KJ mol -1, S o = J mol -1 K -1 Calculate the value for the free energy change, G o for the reaction, CaCO 3 (s) CaO(s) + CO 2 (g) at 815 C o 5. Aluminum metal is oxidized in aqueous base with water serving as the oxidizing agent. Al(s) + H 2 O(1) Al(OH) H 2 (g) (basic solution) Write a balanced equation for this reaction in basic solution. 6. Refer to the following half-reactions below; MnO H + + 5e - Mn H 2 O Cr 2 O H + + 6e - 2Cr H 2 O E 0 = 1.51 V E 0 = 1.33 V Calculate the value of equilibrium constant at 25 0 C for this reaction? 16

17 CHEMISTRY 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. A 32. B 33. D 34. A 35. A PART - II 1. T f = k f x m = k f x (n/kg) = (k f x m)/(mxkg); M = (k f x m)/( T f x kg) M = 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 = H o = kj S o = J G o = H o - T S o G o = kj x x 10-3 kj G o = kj 5. 2Al + 6H 2 O + 2OH - 2Al(OH) H 2 6. G = G o + RT Ln Q E = E o (RT/nF)Ln Q E = E o (0.0592/n)Log Q at equilibrium, E= 0, and Q = Keq. Log Keq. = n E o / = 30 x ( )/ Log Keq. = 91.2; Keq. = 1.58x

Houston Community College System Departmental Final Examination Chemistry CHEM 1412 Final

Houston Community College System Departmental Final Examination Chemistry 1412 CHEM 1412 Final 1 PART I (2 points each) CHEM 1412 FINAL EXAM Version F-1/06A Multiple choice - scantron. Please DO NOT write