Page 1. Spring 2002 Final Exam Review Palmer Graves, Instructor MULTIPLE CHOICE
|
|
- Scott Malone
- 6 years ago
- Views:
Transcription
1 Page 1 MULTIPLE CHOICE 1. Which one of the following exhibits dipole-dipole attraction between molecules? a) XeF b) AsH c) CO d) BCl e) Cl 2. What is the predominant intermolecular force in AsH? a) London-dispersion forces b) ion-dipole attraction c) ionic bonding d) dipole-dipole attraction e) hydrogen-bonding 3. Hydrogen bonding is a special case of. a) London-dispersion forces b) ion-dipole attraction c) dipole-dipole attractions d) none of these e) ion-ion interactions 4. The heat of fusion of water is 6.01 kj/mol. The heat capacity of liquid water is 75.2 J/mol-K. The conversion of 50.0 g of ice at 0.0 C to liquid water at 22.0 C requires kj of heat. a) b) 21.3 c) 17.2 d) e) Insufficient data is given.
2 Page 2 5. The phase diagram of a substance is given below. The region that corresponds to the solid phase is. a) w b) x c) y d) z e) x and y 6. What is the molarity of an aqueous sodium chloride solution that is 13.0% sodium chloride by mass and that has a density of 1.10 g/ml? a) 143 b) 2.45 c) 2.56 d) 2.23 e) Which produces the greatest number of ions when one mole dissolves in water? a) NaCl b) NH NO c) NH Cl d) Na SO e) sucrose 8. In the reaction 2NO 2NO + O at 300 C, [NO ] drops from to M in 100 s. The rate of appearance of O for this period is M/s. a) b) c) d) e)
3 Page 3 9. Given the data below for the reaction yy + zz products the rate law is rate =. Experiment Initial Number [Y]/M [Z]/M Rate (M/s) a) k[y][z] b) k[y] [Z] c) k[y] [Z] d) k[y][z] e) k[y] [Z] 10. The rate constant for a particular reaction is M s at 150 C, and M s at 200 C. What is the energy of activation for this reaction at 250 C? a) 132 b) 56 c) 99 d) 71 e) The reaction 2NO 2NO + O follows second-order kinetics. At 300 C, [NO ] drops from to M in 100 s. Use of the integrated form of the proper rate equation affords a value of L/mol s for the rate constant k. a) b) 0.65 c) 0.81 d) 1.2 e) The reaction CH -N C CH -C N is a first-order reaction. At C, k = s. If [CH -N C] is M, [CH -N C] in M after s is a) b) c) d) e) The activation energy of a reaction whose rate constant increases by a factor of 10.0 when the temperature is increased from 303 K to 333 K is kj. a) 30 b) 33 c) 46 d) 64 e) 89
4 Page At a certain temperature, a flask at equilibrium contains M HCl, M Cl, and M H. What is the value of K c for the equilibrium: 2 HCl(g) Cl (g) + H (g)? a) b) 11.0 c) d) e) The value of K c for the equilibrium H (g) + I (g) 2 HI(g) is 794 at 25 C. At this temperature, what is the value of K c for 1/2 H (g) + 1/2 I (g) HI(g)? a) 397 b) c) 28 d) 1588 e) Consider the reaction shown below: N O (g) 2NO (g) Determine the value of the equilibrium constant for this reaction if an initial concentration of N O (g) of mol/l is reduced to mol/l at equilibrium. There is no NO (g) present at the start of the reaction. a) 0.87 b) 13 c) 0.22 d) e) For the vapor-phase reaction 2AZ A + Z K c = 16 at 523 K. If mol AZ is introduced into an evacuated 1.00 L vessel at 523 K, then at equilibrium [Z ] is M. a) b) c) d) 0.24 e) Consider the following reaction at equilibrium: 2NH (g) N (g) + 3H (g) H = kj Adding N (g) to the system at equilibrium will. a) decrease the concentration of NH (g) at equilibrium b) decrease the concentration of H (g) at equilibrium c) increase the value of the equilibrium constant d) cause the reaction to shift to the right e) remove all of the H (g)
5 Page What is the ph of a M solution of barium hydroxide? a) b) c) 1.82 d) e) What is the ph of an aqueous solution at 25 C in which [OH ] is M? a) b) c) d) e) Calculate the concentration (in M) of hydronium ions in a solution at 25 C with a poh of a) b) c) d) e) The ph of a M NaOH solution at 25 C is. a) 1.96 b) 4.51 c) d) e) The [H ] and ph of a M HNO solution at 25 C are M and, respectively a) , b) , c) 0.021, d) 0.021, e) , Of the following, is a weak acid. a) HF b) HCl c) HBr d) HNO e) HClO 25. HZ is a weak acid. An aqueous solution of HZ is prepared by dissolving mol of HZ in sufficient water to yield 1.00 L of solution. The ph of the solution was 4.93 at 25 C. The K a of HZ is. a) b) c) d) e)
6 Page The ph of a 0.15 M aqueous solution of HOAc at 25 C is. The K a for HOAc is a) 5.57 b) 7.35 c) 2.78 d) 9.18 e) The ph of a 0.10 M solution of a weak base is What is the K b for this base? a) b) c) d) e) Calculate the poh of a M aqueous sodium cyanide solution at 25 C (for CN, K b = ). a) 9.31 b) c) 5.20 d) 1.08 e) A solution containing which one of the following pairs of substances will be a buffer solution? a) NaI, HI b) KBr, HBr c) RbCl, HCl d) CsF, HF e) none of these 30. Calculate the ph of a solution prepared by dissolving 0.37 mol of formic acid (HCO H) and 0.23 mol of sodium formate (NaCO H) in 1.00 L of solution. K a = for formic acid. a) 2.09 b) c) 3.54 d) 2.30 e) Consider the titration of ml of M HClO with M KOH. The H O concentration after addition of 10.0 ml of KOH is M. a) b) c) d) e) Consider the titration of 25.0 ml of M HClO with M KOH. The H O concentration after addition of 66.2 ml of KOH is M. a) b) c) d) e) 0.273
7 Page The ph of a solution prepared by mixing 45 ml of M KOH with 65 ml of M HCl is. a) 1.31 b) 2.92 c) 0.74 d) 1.97 e) What is the molarity of an HOAc solution if 25.5 ml of this solution required 37.5 ml of M NaOH to reach the equivalence point? a) b) c) d) e) The ph at the equivalence point of an HOAc solution if 25.5 ml of this solution required 37.5 ml of M NaOH to reach the equivalence point is closest to. a) 4 b) 7 c) 9 d) 12 e) ml of M HF is titrated with M NaOH. What is the ph when ml of base have been added? (K a for HF is ) a) b) c) d) e) Given the following table of K s p values, determine which compound listed has the smallest solubility. compound K s p CdCO Cd(OH) AgI Fe(OH) 4 10 ZnCO a) ZnCO b) Cd(OH) c) CdCO d) AgI e) Fe(OH) 38. Calculate the molar solubility of silver carbonate (K s p = ). a) b) c) d) e)
8 Page Given the following table of thermodynamic data, substance H f S I (g) kj/mol J/mol-K I (s) determine the normal sublimation point (in C) of iodine. a) b) c) d) e) Some standard entropies (at 25 C in J/mol K) are given: Ca (aq) -55.2, F (aq) -9.6, CaF (s) S for the reaction CaF (s) Ca (aq) + 2F (aq) at 25 C in J/K is. a) b) c) -5.5 d) e) Given the following table of thermodynamic data, substance S C H (g) J/mol-K C H (g) C H (g) H (g) determine the S (in J/mol-K) for the reaction: C H (g) + H (g) C H (g) a) b) c) d) e)
9 Page Consider the following table of thermodynamic data. All values are tabulated for 25 C. Substance G (kj/mol) S (J/mol K) f C H (g) C H (g) C H (g) H (g) H O(g) C H OH(l) What is the value of H (in kj) for the reaction described below? Assume the reaction is performed at 25 C. a) -173 b) 236 c) -311 d) -248 e) 149 C H (g) + 2H (g) C H (g) 43. Consider the following table of thermodynamic data. Substance G (kj/mol) S (J/mol K) f NO(g) NO (g) NOCl(g) N O(g) Determine the value of G (kj) for the following reaction taking place at 25 C. 2NO(g) + O (g) 2NO (g) a) b) c) d) e) insufficient information is given 44. Consider the following reaction at 25 C. C(s) + H O(g) CO(g) + H (g) G = 91.2 kj H = kj What is the value of S (J/K) for this reaction at 25 C? a) -135 b) 1.6 c) -1.6 d) 135 e) 223
10 Page Determine the value of G (kj) for the following reaction using data from the table below. 2H O(g) + O (g) 2H O (g) Substance G (kj/mol) f a) -246 b) 666 c) 246 d) -666 e) More data are needed. H O(g) -228 H O (g) Consider the reaction: Ag (aq) + Cl (aq) AgCl(s) Given the following table of thermodynamic data, substance H f S Ag (aq) kj/mol J/mol-K Cl (aq) AgCl(s) determine the value of G (in kj/mol) for the reaction at 25 C. a) b) c) d) e) Consider the following reaction. A + B C This reaction will always be spontaneous if H is and S is. a) +, + b) -, - c) -, + d) +, - e) +, The equilibrium constant for a reaction is 0.48 at 25 C. What is the value of G (kj) at this temperature? (R = J/K mol) a) 1.8 b) -4.2 c) d) 4.2 e) More information is needed. (c) 2000 Prentice-Hall, Inc. All rights reserved.
11 ANSWER KEY FOR TEST UNTITLED Page 1 1. b 2. d 3. c 4. b 5. a 6. b 7. d 8. a 9. b 10. d 11. e 12. a 13. d 14. b 15. c 16. a Chapter: 11 QUESTION: 9 Chapter: 11 QUESTION: 10 Chapter: 11 QUESTION: 27 Chapter: 11 QUESTION: 50 Chapter: 11 QUESTION: 74 Chapter: 13 QUESTION: 71 Chapter: 13 QUESTION: 91 Chapter: 14 QUESTION: 3 Chapter: 14 QUESTION: 29 Chapter: 14 QUESTION: 42 Chapter: 14 QUESTION: 45 Chapter: 14 QUESTION: 46 Chapter: 14 QUESTION: 78 Chapter: 15 QUESTION: 24 Chapter: 15 QUESTION: 31 Chapter: 15 QUESTION: 61
12 ANSWER KEY FOR TEST UNTITLED Page b 18. b 19. a 20. c 21. b 22. c 23. c 24. a 25. b 26. c 27. b 28. c 29. d 30. c 31. a 32. b Chapter: 15 QUESTION: 67 Chapter: 15 QUESTION: 74 Chapter: 16 QUESTION: 18 Chapter: 16 QUESTION: 23 Chapter: 16 QUESTION: 30 Chapter: 16 QUESTION: 40 Chapter: 16 QUESTION: 47 Chapter: 16 QUESTION: 58 Chapter: 16 QUESTION: 60 Chapter: 16 QUESTION: 67 Chapter: 16 QUESTION: 87 Chapter: 16 QUESTION: 97 Chapter: 17 QUESTION: 14 Chapter: 17 QUESTION: 24 Chapter: 17 QUESTION: 49 Chapter: 17 QUESTION: 50
13 ANSWER KEY FOR TEST UNTITLED Page d 34. c 35. c 36. e 37. e 38. a 39. c 40. d 41. a 42. c 43. a 44. d 45. c 46. c 47. c Chapter: 17 QUESTION: 59 Chapter: 17 QUESTION: 61 Chapter: 17 QUESTION: 62 Chapter: 17 QUESTION: 73 Chapter: 17 QUESTION: 82 Chapter: 17 QUESTION: 89 Chapter: 19 QUESTION: 19 Chapter: 19 QUESTION: 40 Chapter: 19 QUESTION: 43 Chapter: 19 QUESTION: 54 Chapter: 19 QUESTION: 55 Chapter: 19 QUESTION: 58 Chapter: 19 QUESTION: 60 Chapter: 19 QUESTION: 64 Chapter: 19 QUESTION: 72
14 ANSWER KEY FOR TEST UNTITLED Page a Chapter: 19 QUESTION: 83 (c) 2000 Prentice-Hall, Inc. All rights reserved.
1. Rank the following elements in order of increasing atomic radius: P, Al, Cl, F, S
Useful constants and other information: R = 0.0821 LCatm/KCmole R = 8.314 J/KCmole h = 6.626 x 10-34 JCs 1 atm = 760 torr Specific heat of H 2 O(l) = 4.184 J/gC C 1 cal = 4.184 J c = 3 x 10 8 m/s PART
More informationE) Buffer capacity is the amount of acid that can be added until all of the base is used up.
Chem 124 Spring 2016 Exam 3 VERSION 1 Name make sure you fill in your version number in the TN box on the side of your scantron sheet 1) Which of the following solutions is a good buffer system? A) a solution
More informationph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin)
JASPERSE CHEM 210 PRACTICE TEST 3 VERSION 2 Ch. 17: Additional Aqueous Equilibria Ch. 18: Thermodynamics: Directionality of Chemical Reactions Key Equations: For weak acids alone in water: [H + ] = K a
More information(for tutoring, homework help, or help with online classes)
www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. chem10b 17.2-5 Of the following solutions, which has the greatest buffering capacity? A. 0.821 M HF and 0.909 M NaF
More informationCHEM 102 Final Mock Exam
CHEM 102 Final Mock Exam 1. A system releases 300 J of heat and does 650 J of work on the surroundings. What is the change in internal energy of the system? a. -950 J b. 350 J c. 950 J d. -350 J 2. Which
More informationX212F Which of the following is a weak base in aqueous solution? A) H 2 CO 3 B) B(OH) 3 C) N 2 H 4 D) LiOH E) Ba(OH) 2
PX212SP14 Practice Exam II / Spring 2014 1. Which of the following statements are characteristic of acids? 1. They are proton donors. 2. They react with bases to produce a salt and water. 3. They taste
More informationChemistry 1A Fall 2013 MWF 9:30 Final Test Form A
Chemistry 1A Fall 2013 MWF 9:30 Final Test Form A 1. How many moles of P 4 molecules are in 141.4 g of phosphorus? A) 4.566 mol B) 1.752 x10 4 mol C) 1.141 mol D) 2.348 x 10 1 mol E) 1.414 x 10 1 mol 2.
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More informationDougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria
Dougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria This is a PRACTICE TEST. Complete ALL questions. Answers will be provided so that you may check your work. I strongly
More informationChapter 19 Chemical Thermodynamics
Chapter 19. Chemical Thermodynamics Sample Exercise 19.2 (p. 819) Elemental mercury is a silver liquid at room temperature. Its normal freezing point is -38.9 o C, and its molar enthalpy of fusion is H
More informationCh 8 Practice Problems
Ch 8 Practice Problems 1. What combination of substances will give a buffered solution that has a ph of 5.05? Assume each pair of substances is dissolved in 5.0 L of water. (K a for NH 4 = 5.6 10 10 ;
More informationHEMISTRY 110 EXAM 3 April 6, 2011 FORM A When the path is blocked, back up and see more of the way. 1. A 250 L vessel is evacuated and then connected to a 50.0 L bulb with compressed nitrogen. The pressure
More informationCHEM Dr. Babb s Sections Exam #4 Review Sheet
CHEM 116 - Dr. Babb s Sections Exam #4 Review Sheet 158. Explain using the HC 2 H 3 O 2 /NaC 2 H 3 O 2 buffer system how a buffer maintains a relatively constant ph when small quantity of acid (HCl) or
More information10. Calculate the mass percent nitrogen in (NH 4 ) 2 CO 3 (molar mass = g/mol). a % c % e % b % d % f. 96.
Chem 1721/1821: Final Exam Review Multiple Choice Problems 1. What is the molar mass of barium perchlorate, Ba(ClO 4 ) 2? a. 189.90 g/mol c. 272.24 g/mol e. 336.20 g/mol b. 240.24 g/mol d. 304.24 g/mol
More informationFor the entire exam, solutions are aqueous and T = 25 C unless stated otherwise. Questions 1 15 cover material from Exam 1.
For the entire exam, solutions are aqueous and T = 25 C unless stated otherwise. Questions 1 15 cover material from Exam 1. 1. What state of matter is described as follows? On the molecular level, the
More informationSlide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c
Slide 1 / 84 1 Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy A B C D E a only b only c only a and c b and c Slide 2 / 84 2 The internal energy of a system
More informationChemistry 122 Wrap-Up Review Kundell
Chapter 11 Chemistry 122 Wrap-Up Review Kundell 1. The enthalpy (heat) of vaporization for ethanol (C 2 H 5 OH) is 43.3 kj/mol. How much heat, in kilojoules, is required to vaporize 115 g of ethanol at
More informationCHEMpossible. Final Exam Review
CHEMpossible Final Exam Review 1. Given the following pair of reactions and their equilibrium constants: 2NO 2 (g) 2NO (g) + O 2 (g) K c = 15.5 2NO (g) + Cl 2 (g) 2 NOCl (g) K c = 3.20 10-3 Calculate a
More informationph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin) 1. Which of the following combinations would provide buffer solutions?
JASPERSE CHEM 210 PRACTICE TEST 3 VERSION 3 Ch. 17: Additional Aqueous Equilibria Ch. 18: Thermodynamics: Directionality of Chemical Reactions Key Equations: For weak acids alone in water: [H + ] = K a
More informationChem 1B, Test Review #2
1. The following kinetics data were obtained for the reaction: Expt.# 2NO(g) + Cl 2 (g) 2NOCl(g) [NO] 0 (mol/l) [Cl 2 ] 0 (mol/l) Initial Rate, (mol/l.s) 1 0.20 0.10 6.3 x 10 3 2 0.20 0.30 1.9 x 10 2 3
More informationCHE 107 FINAL EXAMINATION December 10, 2012
CHE 107 FINAL EXAMINATION December 10, 2012 University of Kentucky Department of Chemistry READ THESE DIRECTIONS CAREFULLY BEFORE STARTING THE EXAMINATION! It is extremely important that you fill in the
More informationChem Practice Exam Two (Chapters 19, 20 and 21)
Chem 203 - Practice Exam Two (Chapters 19, 20 and 21) 1. Consider the dissolution of MnS in water (K sp = 3.0 10 14 ). MnS(s) + H 2O(l) Mn 2+ (aq) + HS (aq) + OH (aq) How is the solubility of manganese(ii)
More informationAcid-Base Equilibria and Solubility Equilibria Chapter 17
PowerPoint Lecture Presentation by J. David Robertson University of Missouri Acid-Base Equilibria and Solubility Equilibria Chapter 17 The common ion effect is the shift in equilibrium caused by the addition
More informationEquilibri acido-base ed equilibri di solubilità. Capitolo 16
Equilibri acido-base ed equilibri di solubilità Capitolo 16 The common ion effect is the shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance.
More informationThermodynamics. 1. Which of the following processes causes an entropy decrease?
Thermodynamics 1. Which of the following processes causes an entropy decrease? A. boiling water to form steam B. dissolution of solid KCl in water C. mixing of two gases in one container D. beach erosion
More informationTest #3 Last Name First Name November 13, atm = 760 mm Hg
Form G Chemistry 1442-001 Name (please print) Test #3 Last Name First Name November 13, 2003 Instructions: 1. This exam consists of 25 questions. 2. No scratch paper is allowed. You may do the work in
More informationANSWERS CIRCLE CORRECT SECTION
CHEMISTRY 162 - EXAM I June 08, 2009 Name: SIGN: RU ID Number Choose the one best answer for each question and write the letter preceding it in the appropriate space on this answer sheet. Only the answer
More informationIntermolecular Forces 2 nd Semester Review Questions and Problems
Intermolecular Forces 2 nd Semester Review Questions and Problems 1. Complete the following table: Molecule Lewis Structure Molecule Shape Polar/Nonpolar CS 2 H 3 O + CdBr 2 CHI 3 2. What makes the dipole
More informationChemistry Lab Equilibrium Practice Test
Chemistry Lab Equilibrium Practice Test Basic Concepts of Equilibrium and Le Chatelier s Principle 1. Which statement is correct about a system at equilibrium? (A) The forward and reverse reactions occur
More informationCHEMISTRY Midterm #2 October 26, Pb(NO 3 ) 2 + Na 2 SO 4 PbSO 4 + 2NaNO 3
CHEMISTRY 123-02 Midterm #2 October 26, 2004 The total number of points in this exam is 100. The total exam time is 50 min. Good luck! PART I: MULTIPLE CHOICE (Each multiple choice question has a 2-point
More information7. A solution has the following concentrations: [Cl - ] = 1.5 x 10-1 M [Br - ] = 5.0 x 10-4 M
Solubility, Ksp Worksheet 1 1. How many milliliters of 0.20 M AlCl 3 solution would be necessary to precipitate all of the Ag + from 45ml of a 0.20 M AgNO 3 solution? AlCl 3(aq) + 3AgNO 3(aq) Al(NO 3)
More information4. [7 points] Which of the following reagents would decrease the solubility of AgCl(s)? NaOH HCl NH 3 NaCN
1. [7 points] It takes 0.098 g of silver iodate, AgIO 3, to make 1.00-L of a saturated solution saturated at 25 C. What is the value of the solubility product, K sp? a. 3.5 10 4 b. 1.2 10 7 c. 9.8 10 2
More informationCHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A
CHEMISTRY 110 EXAM 3 NOVEMER 12, 2012 FORM A 1. Consider a balloon filled with 5 L of an ideal gas at 20 C. If the temperature of the balloon is increased by 70 C and the external pressure acting on the
More information2. Which of the following liquids would have the highest viscosity at 25 C? A) CH 3 OCH 3 B) CH 2 Cl 2 C) C 2 H 5 OH D) CH 3 Br E) HOCH 2 CH 2 OH
CHEF124 Mid Term Revision (Trimester 3, 2012/13) 1. Identify the dominant (strongest) type of intermolecular force present in (a) RbCl(s) ionic (b) NH 3 (l) - hydrogen bonding (c) Cl 2 (l) dispersion (d)
More informationB 2 Fe(s) O 2(g) Fe 2 O 3 (s) H f = -824 kj mol 1 Iron reacts with oxygen to produce iron(iii) oxide as represented above. A 75.
1 2004 B 2 Fe(s) + 3 2 O 2(g) Fe 2 O 3 (s) H f = -824 kj mol 1 Iron reacts with oxygen to produce iron(iii) oxide as represented above. A 75.0 g sample of Fe(s) is mixed with 11.5 L of O 2 (g) at 2.66
More information2. Write a balanced chemical equation which corresponds to the following equilibrium constant expression.
Practice Problems for Chem 1B Exam 1 Chapter 14: Chemical Equilibrium 1. Which of the following statements is/are CORRECT? 1. For a chemical system, if the reaction quotient (Q) is greater than K, products
More informationCHEM 212 Practice Exam 2 1
CHEM 212 Practice Exam 2 1 1. In the following reaction NH 4 + (aq) + H 2 O(l) NH 3 (aq) + H 3 O + (aq) a. NH 4 + is an acid and NH 3 is its b. H 2 O is an acid and H 3 O + is its c. NH 4 + is an acid
More informationAP Chemistry 1st Semester Final Review Name:
AP Chemistry 1st Semester Final Review Name: 2015-2016 1. Which of the following contains only sigma (s) bonds? 5. H2O(g) + CO(g) H2(g) + CO2(g) A) CO2 B) C3H6 C) CH3Cl D) N2O3 E) SiO2 2. What is the equilibrium
More informationGeneral Chemistry Study Guide
General Chemistry 1311 Study Guide Name : Louise K number: Date: Oct 02006 Instructor: Jingbo Louise Liu kfjll00@tamuk.edu 1 Chapter 04 & 05 (10 questions required and 5 questions for extra credit) Credited
More informationChapter How many grams of a 23.4% by mass NaF solution is needed if you want to have 1.33 moles of NaF?
Chapter 13 1. Which of the following compounds is a strong electrolyte? a. NH 4Cl b. NaCl c. NaC 2H 3O 2 d. HCl e. All of the above 2. A solution that is 13.58% by mass of sugar contains 13.75 grams of
More informationPage 1. Exam 2 Review Summer A 2002 MULTIPLE CHOICE. 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l)
Page 1 MULTIPLE CHOICE 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l) The coefficient of HCl(aq) in the balanced reaction is. a) 1 b) 2 c) 3 d) 4 e) 0 2. Given the information
More informationEquilibrium Practice Test
Equilibrium Practice Test Name: ANSWERS Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. (20 marks) 60 /60 1. Equilibrium happens when. a. opposing
More information1442 Final Review website: Chapter 13 Properties of Solutions
1442 Final Review website: http://dipowell1.home.mindspring.com Chapter 13 Properties of Solutions Useful Information: R = 0.08206 L. atm/mol. K = 8.314 J/mol. K 1 atm = 760 torr = 760 mm Hg P soln = (P
More informationChapter 8: Phenomena. Chapter 8: Applications of Aqueous Equilibrium
Chapter 8: Phenomena ph ph ph ph 14 12 10 8 6 4 2 0 14 12 10 8 6 4 2 0 Phenomena: Buffers are sometimes defined as: a solution that resists changes in ph when an acid base is added to it. This definition
More informationph = pk a + log 10 {[base]/[acid]}
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9 ) ( F - 32) F = ( 9 / 5 )( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
More information1002_2nd Exam_
1002_2nd Exam_1010418 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) How will addition of sodium acetate to an acetic acid solution affect the
More informationBROOKLYN COLLEGE. FINAL EXAMINATION IN CHEMISTRY 1. Fall, Paul Cohen, instructor.
Name BROOKLYN COLLEGE. FINAL EXAMINATION IN CHEMISTRY 1. Fall, 2008. Paul Cohen, instructor. Formulas: Write the chemical formula for each of the following: Al 2 (S0 4 ) 3 1. Aluminum sulfate Ni(OH) 2
More informationCHM151 Quiz Pts Fall 2013 Name: Due at time of final exam. Provide explanations for your answers.
CHM151 Quiz 12 100 Pts Fall 2013 Name: Due at time of final exam. Provide explanations for your answers. 1. Which one of the following substances is expected to have the lowest melting point? A) BrI B)
More informationName period AP Unit 8: equilibrium
Name period AP Unit 8: equilibrium 1. What is equilibrium? Rate of the forward reaction equals the rate of the reverse reaction 2. How can you tell when equilibrium has been reached? The concentrations
More informationA) sublimation. B) liquefaction. C) evaporation. D) condensation. E) freezing. 11. Below is a phase diagram for a substance.
PX0411-1112 1. Which of the following statements concerning liquids is incorrect? A) The volume of a liquid changes very little with pressure. B) Liquids are relatively incompressible. C) Liquid molecules
More information2. (12 pts) Write the reactions that correspond to the following enthalpy changes: a) H f o for solid aluminum oxide.
1. (6 pts) Given the following data at 25 o C: 2 O 3 (g) > 3 O 2 (g) H o = 427 kj O 2 (g) > 2 O (g) H o = 495 kj NO (g) + O 3 (g) > NO 2 (g) + O 2 (g) H o = 199 kj Calculate H o for the following reaction
More information3. Which of the following compounds is soluble? The solubility rules are listed on page 8.
1. Classify the following reaction. Sb 2 O 3 + 3 Fe 2 Sb + 3 FeO a) Combination reaction b) Decomposition reaction c) Neutralization reaction d) Single-replacement reaction e) Double-replacement reaction
More informationChem 128, Exam III April 23, 2004
I. (35 points) A. (10 points) Consider an aqueous solution of PbI 2 with solid lead(ii) iodide present. K sp =8.4x10 9. 1. Write a balanced net ionic equation for the equilibrium established between the
More informationCh 9 Practice Problems
Ch 9 Practice Problems 1. One mole of an ideal gas is expanded from a volume of 1.50 L to a volume of 10.18 L against a constant external pressure of 1.03 atm. Calculate the work. (1 L atm = 101.3 J) A)
More informationAP Chemistry. 4. Which atom in its ground state has the most unpaired electrons? a. Ge b. As c. Se d. Br e. Ga
Name AP Chemistry Take Home Quiz Due Thursday, 1/9/2014 Bubble the correct answer on your scantron for each of the following. 1. Barium sulfate is LEAST soluble in a 0.01-molar solution of which of the
More informationCh 10 Practice Problems
Ch 10 Practice Problems 1. Which of the following result(s) in an increase in the entropy of the system? I. (See diagram.) II. Br 2(g) Br 2(l) III. NaBr(s) Na + (aq) + Br (aq) IV. O 2(298 K) O 2(373 K)
More informationQuiz name: Equilibria + Acids/Bases
Name: Quiz name: Equilibria + Acids/Bases Date: 1. 2. At 450 C, 2.0 moles each of H 2(g), I 2(g), and HI are combined in a 1.0 L rigid container. The value of K c at 450 C is 50. Which of the following
More informationAP Chemistry. CHAPTER 17- Buffers and Ksp 17.1 The Common Ion Effect Buffered Solutions. Composition and Action of Buffered Solutions
AP Chemistry CHAPTER 17- Buffers and Ksp 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak electrolyte.
More information5. What is the percent ionization of a 1.4 M HC 2 H 3 O 2 solution (K a = ) at 25 C? A) 0.50% B) 0.36% C) 0.30% D) 0.18% E) 2.
Name: Date: 1. For which of the following equilibria does K c correspond to an acid-ionization constant, K a? A) NH 3 (aq) + H 3 O + (aq) NH 4 + (aq) + H 2 O(l) B) NH 4 + (aq) + H 2 O(l) NH 3 (aq) + H
More informationCH302 Spring 2009 Practice Exam 1 (a fairly easy exam to test basic concepts)
CH302 Spring 2009 Practice Exam 1 (a fairly easy exam to test basic concepts) 1) Complete the following statement: We can expect vapor pressure when the molecules of a liquid are held together by intermolecular
More informationCHM 2046 Final Exam Review: Chapters 11 18
Chapter 11 1. Which of the following has the lowest boiling point? a. NH 3 b. CH 3 Cl c. NaCl d. CO 2 e. CH 3 CH 2 CH 2 CH 2 CH 3 2. Which of the following has the lowest vapor pressure? a. CH 3 F b. CH
More informationAP Study Questions
Name: Class: Date: AP 17.1-17.2 Study Questions True/False Indicate whether the statement is true or false. 1. The extent of ionization of a weak electrolyte is increased by adding to the solution a strong
More informationChem 210 Jasperse Final Exam- Version 1 Note: See the very last page to see the formulas that will be provided with the final exam.
Chem 210 Jasperse Final Exam- Version 1 Note: See the very last page to see the formulas that will be provided with the final exam. 1 1. Which of the following liquids would have the highest vapor pressure,
More informationName: Score: /100. Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each
Name: Score: /100 Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each 1. Which of the following contains the greatest number of moles of O? A) 2.3 mol H 2 O
More informationFORMULA SHEET (tear off)
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9) ( F - 32) F = ( 9 / 5)( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
More informationName: Score: /100. Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each
Name: Score: /100 Part I. Multiple choice. Write the letter of the correct answer for each problem. 3 points each 1. Which of the following contains the greatest number of moles of O? A) 2.3 mol H 2 O
More informationSolubility Equilibria
Chapter 17 SOLUBILITY EQUILIBRIA (Part II) Dr. Al Saadi 1 Solubility Equilibria The concept of chemical equilibrium helps to predict how much of a specific ionic compound (salt) will dissolve in water.
More informationExam 2 Sections Covered: 14.6, 14.8, 14.9, 14.10, 14.11, Useful Info to be provided on exam: K K [A ] [HA] [A ] [B] [BH ] [H ]=
Chem 101B Study Questions Name: Chapters 14,15,16 Review Tuesday 3/21/2017 Due on Exam Thursday 3/23/2017 (Exam 3 Date) This is a homework assignment. Please show your work for full credit. If you do work
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More informationAcid-Base Equilibria and Solubility Equilibria
ACIDS-BASES COMMON ION EFFECT SOLUBILITY OF SALTS Acid-Base Equilibria and Solubility Equilibria Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 2 The common
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which one of the following is the weakest acid? 1) A) HF (Ka = 6.8 10-4) B) HNO2 (Ka
More informationName Date Class ACID-BASE THEORIES
19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary
More informationFORMULA SHEET (tear off)
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9) ( F - 32) F = ( 9 / 5)( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More informationAcid-Base Equilibria and Solubility Equilibria
Acid-Base Equilibria and Solubility Equilibria Acid-Base Equilibria and Solubility Equilibria Homogeneous versus Heterogeneous Solution Equilibria (17.1) Buffer Solutions (17.2) A Closer Look at Acid-Base
More informationCH 223 Sample Exam Exam II Name: Lab Section:
Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. Which of the following equations is the solubility
More informationIllinois JETS Academic Challenge Chemistry Test (District) Useful Information. PV = nrt R = L atm mol -1 K -1.
Useful Information PV = nrt R = 0.08206 L atm mol -1 K -1 Q = m x T x s 1 atm = 760 torr Avogadro's number = 6.022 x 10 23 K = C + 273 ph = -log [H + ] 1 1 E = (-R H ) - n 2 n 2 f i R H = 2.18 x 10-18
More informationQuestions 1 13 cover material from Exam 1
Questions 1 13 cover material from Exam 1 1. Which intermolecular forces are present in H Te(l)? A. dispersion only C. dispersion, dipole-dipole, and hydrogen bonding B. dispersion and dipole-dipole D.
More informationAP Chemistry Big Idea Review
Name: AP Chemistry Big Idea Review Background The AP Chemistry curriculum is based on 6 Big Ideas and many Learning Objectives associated with each Big Idea. This review will cover all of the Big Ideas
More informationFORMULA SHEET (tear off)
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9) ( F - 32) F = ( 9 / 5)( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
More information6. Place the following elements in order of increasing atomic radii: Mg, Na, Rb, Cl.
CH141 Practice Problems/Practice Final Exam Page 1 of 12 Name: 1. What is the SO 4 2- concentration of a solution prepared by dissolving 3.00 g of Na 2 SO 4 in 1.00 L of water? 2. What is the hybridization
More informationQuestions 1 15 cover Exam 1 material
Questions 1 15 cover Exam 1 material 1. Which molecule cannot hydrogen bond to another molecule of itself? A. CH3OH C. CH3CH3 B. CH3NH2 D. HF 2. Concerning surface tension, which of the following is incorrect?
More informationChem. 1A Final. Name. Student Number
Chem. 1A Final Name Student Number All work must be shown on the exam for partial credit. Points will be taken off for incorrect or no units. Calculators are allowed. Cell phones may not be used for calculators.
More information2. What mass of an aqueous 22.9% sodium chloride solution contains 99.5 g of water?
CHEM 1412 MIDTERM EXAM (100 pts total) ANSWER KEY Student s Name PART A (20 multiple choice questions, 3 pts each): 1. The solubility of a gas in a liquid can always be increased by: a) decreasing the
More informationACIDS, BASES, AND SALTS
ACIDS, BASES, AND SALTS Chapter Quiz Choose the best answer and write its letter on the line. 1. A solution in which the hydroxide-ion concentration is 1 10 2 is a. acidic. c. neutral. b. basic. d. none
More information3. [7 points] Which of the following slightly soluble salts has the largest molar solubility in aqueous solution?
1. [7 points] The solubility product expression for Pb 3 (PO 4 ) 2 (s) is (a) [3 Pb 2+ ] 3 [2 PO 4 3 ] 2 (b) [Pb 2+ ] 2 [PO 4 3 ] 3 (c) [3 Pb 2+ ] 3 [2 PO 4 3 ] 2 /[Zn 3 (PO 4 ) 2 ] (d) [3 Pb 2+ ][2 PO
More informationChemistry Grade : 11 Term-3/Final Exam Revision Sheet
Chemistry Grade : 11 Term-3/Final Exam Revision Sheet Exam Date: Tuesday 12/6/2018 CCS:Chem.6a,6b,6c,6d,6e,6f,7a,7b,7d,7c,7e,7f,1g Chapter(12):Solutions Sections:1,2,3 Textbook pages 378 to 408 Chapter(16):Reaction
More informationCreate assignment, 48975, Exam 2, Apr 05 at 9:07 am 1
Create assignment, 48975, Exam 2, Apr 05 at 9:07 am 1 This print-out should have 30 questions. Multiple-choice questions may continue on the next column or page find all choices before making your selection.
More informationChap. 4 AQUEOUS RXNS. O H δ+ 4.1 WATER AS A SOLVENT 4.2 AQUEOUS IONIC REACTIONS. Page 4-1. NaOH(aq) + HCl(g) NaCl(aq) +H 2 O
Chap. AQUEOUS RXNS.1 WATER AS A SOLVENT Describe solution composition in terms of molarity Describe strong and weak electrolyte solutions, including acids and bases Use ionic equations to describe neutralization
More informationOctober 19, 1999 Page 1. Chapter 4 Practice Worksheet Dr. Palmer Graves, Instructor MULTIPLE CHOICE
October 19, 1999 Page 1 MULTIPLE CHOICE Section 4.1 Some Ways that Chemical Reactions Occur 1. The reaction of HNO (aq) + KOH(aq) KNO (aq) + H O(l) is best classified as a(n) a) acid-base neutralization
More informationCHEMpossible. 101 Exam 2 Review
CHEMpossible 1. Circle each statement that applies to thermal energy and heat: a. Thermal energy is the average kinetic energy of its molecules due to their motion b. High thermal energy is reflected in
More informationANSWER KEY CHEMISTRY F14O4 FIRST EXAM 2/16/00 PROFESSOR J. MORROW EACH QUESTION IS WORTH 1O POINTS O. 16.
discard 1 2 ANSWER KEY CHEMISTRY F14O4 FIRST EXAM 2/16/00 PROFESSOR J. MORROW PRINT NAME, LAST: FIRST: I.D.# : EACH QUESTION IS WORTH 1O POINTS 1. 7. 13. 2. 8. 14. 3. 9. 15. 4. 1O. 16. 5. 11. 17. 6. 12.
More informationCHM 2046 Test #3 Review: Chapters , 15, & 16
Chapter 14 1. For the following reaction Kc = 0.513 at 500 K. N 2 O 4 (g) 2 NO 2 (g) If a reaction vessel initially contains an N 2 O 4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations
More informationTitration a solution of known concentration, called a standard solution
Acid-Base Titrations Titration is a form of analysis in which we measure the volume of material of known concentration sufficient to react with the substance being analyzed. Titration a solution of known
More information1. When the following reaction is balanced using smallest whole-number integers, what is the coefficient for oxygen?
Chemistry 11 Fall 2009 Examination #2 ANSWER KEY For the first portion of this exam, select the best answer choice for the questions below and mark the answers on your scantron. Then answer the free response
More information5.2 Energy. N Goalby chemrevise.org Lattice Enthalpy. Definitions of enthalpy changes
5.2 Energy 5.2.1 Lattice Enthalpy Definitions of enthalpy changes Enthalpy change of formation The standard enthalpy change of formation of a compound is the energy transferred when 1 mole of the compound
More informationSCH4U: Practice Exam
SCHU_07-08 SCHU: Practice Exam Energy in Chemistry 1. Which of the following correctly describes a reaction that absorbs heat from the surroundings? a. the reaction is endothermic b. H for this reaction
More informationFORMULA SHEET (tear off)
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9 ) ( F - 32) F = ( 9 / 5 )( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
More informationSample Questions for Exam 2. Chem 1310 A/B, Dr. Williams, Revised 10/27/ chapter
Sample Questions for Exam 2. Chem 1310 A/B, Dr. Williams, Revised 10/27/2005 -------chapter 6---------------- 1. Which of the following molecules is nonpolar? a. Br 2 b. BrCl c. HBr e. CO 2 e. all of these
More information3. The osmotic pressure of a ml solution of an unknown nonelectrolyte is 122 torr at 25 C. Determine the molarity of the solution.
1. Which of the following has a correct van t Hoff factor indicated? A. Al 2 (SO 4 ) 3, i = 5 C. CaBr 2, i = 2 B. Na 2 CO 3, i = 6 D. C 6 H 12 O 6, i = 3 2. Calculate the vapor pressure of a solution containing
More information