Chemistry 12. Chemistry 12 AUGUST 2005 AUGUST Course Code = CH. Course Code = CH. Student Instructions
|
|
- Vivien Barker
- 6 years ago
- Views:
Transcription
1 MINISTRY USE ONLY Place Personal Education Number (PEN) here. Chemistry 12 AUGUST 2005 Course Code = C Chemistry 12 AUGUST 2005 Course Code = C 1. Place the stickers with your Personal Education Number (PEN) in the allotted spaces above. Under no circumstance is your name or identification, other than your Personal Education Number, to appear on this booklet. 2. Ensure that in addition to this examination booklet, you have a Data Booklet and an Examination Response Form. Follow the directions on the front of the Response Form. 3. Disqualification from the examination will result if you bring books, paper, notes or unauthorized electronic devices into the examination room. Student Instructions 4. When instructed to open this booklet, check the numbering of the pages to ensure that they are numbered in sequence from page one to the last page, which is identified by END OF EXAMINATION. 5. At the end of the examination, place your Response Form inside the front cover of this booklet and return the booklet and your Response Form to the supervisor.
2 MINISTRY USE ONLY Question (.5) NR Question (.5) NR Place Personal Education Number (PEN) here. Question (.5) NR Question (.5) NR Chemistry 12 AUGUST 2005 Course Code = C Question (.5) NR Question (.5) NR Question (.5) NR Question (.5) NR Version
3 GENERAL INSTRUCTIONS 1. Aside from an approved calculator, electronic devices, including dictionaries and pagers, are not permitted in the examination room. 2. All multiplechoice answers must be entered on the Response Form using an B pencil. Multiplechoice answers entered in this examination booklet will not be marked. 3. For each of the writtenresponse questions, write your answer in the space provided in this booklet. 4. Ensure that you use language and content appropriate to the purpose and audience of this examination. Failure to comply may result in your paper being awarded a zero. 5. This examination is designed to be completed in two hours. Students may, however, take up to 30 minutes of additional time to finish.
4 CEMISTRY 12 PROVINCIAL EXAMINATION 1. This examination consists of two parts: Value Suggested Time PART A: 60 multiplechoice questions PART B: 8 writtenresponse questions Total: 90 marks 120 minutes 2. The following tables can be found in the separate Data Booklet: Periodic Table of the Elements Atomic Masses of the Elements Names, Formulae, and Charges of Some Common Ions Solubility of Common Compounds in Water Solubility Product Constants at 25 C Relative Strengths of BrønstedLowry Acids and Bases AcidBase Indicators Standard Reduction Potentials of alfcells No other reference materials or tables are allowed. 3. A calculator is essential for the Chemistry 12 Provincial Examination. The calculator must be a handheld device designed primarily for mathematical computations involving logarithmic and trigonometric functions and may be capable of performing graphing functions. Computers, calculators with a QWERTY keyboard or symbolic manipulation abilities, and electronic writing pads will not be allowed. Students must not bring any external devices (peripherals) to support calculators such as manuals, printed or electronic cards, printers, memory expansion chips or cards, CDROMs, libraries or external keyboards. Students may have more than one calculator available during the examination, of which one may be a scientific calculator. Calculators may not be shared and must not have the ability to either transmit or receive electronic signals. In addition to an approved calculator, students will be allowed to use rulers, compasses, and protractors during the examination. Calculators must not have any information programmed into memory that would not be acceptable in paper form. Specifically, calculators must not have any builtin notes, definitions, or libraries. There is no requirement to clear memories at the beginning of the examination but the use of calculators with builtin notes is equivalent to the use of notes in paper form. Any student deemed to have cheated on a provincial examination will receive a 0 on that examination and will be permanently disqualified from the Provincial Examination Scholarship Program.
5 PART A: MULTIPLE COICE Value: 60 marks INSTRUCTIONS: Suggested Time: 80 minutes For each question, select the best answer and record your choice on the Response Form provided. Using an B pencil, completely fill in the circle that has the letter corresponding to your answer. 1. Which of the following could not be units for reaction rate? A. sec 1 B. gml C. M min D. C hour 2. Which of the following represents the typical mathematical relationship between reaction rate and time? A. B. Rate Rate Time Time C. D. Rate Rate Time Time 2005 Province of British Columbia. All rights reserved. Page 1
6 3. Consider the following reaction: Zn( s) + 2Cl( aq) Æ ZnCl2( aq) + 2( g) In two different experiments, equal moles of Zn and equal volumes of Cl are reacted. After 2 minutes, the volume of 2 produced is recorded as follows: Zn Temp [ Cl] Volume 2 ml ( ) Experiment 1 strip 10 C M Experiment 2 powdered 15 C 30. M 73. Which of the following factors explains why the rate in Experiment 1 is different than the rate in Experiment 2? A. [ Cl] B. temperature C. nature of reactants D. surface area of Zn Page Province of British Columbia. All rights reserved.
7 2005 Province of British Columbia. All rights reserved. Page 3 4. Consider the following reaction: Br C + O Æ Br + O C Which of the following could be true of the activated complex? Structure PE (relative to reactants) A. Br C O È Î 2 lower B. Br C O È Î lower C. Br C O È Î 2 higher D. Br C O È Î higher
8 5. Consider the following PE diagram: 600 PE (kj) Progress of the reaction Which of the following is true for the forward reaction? D Ea ( kj) A B C D Which of the following would have a positive value for D? I. the evaporation of water II. the burning of a match III. the explosive reaction between 2 and O 2 IV. a chemical cold pack A. III only B. IV only C. I and IV D. II and III Page Province of British Columbia. All rights reserved.
9 7. Which of the following represents the value for the activation energy of the forward reaction in an equilibrium system? A. E = E + ( D) a( forward) a( reverse) B. E = E ( D) a( forward) a( reverse) C. E = ( D) E a( forward) a( reverse) D. E = ( D) E a( forward) a( reverse) 8. Consider the following equilibrium: CaCO3( s) Æ CaO( s) + CO2( g) In which of the flasks will this equilibrium be established? Flask 1 Flask 2 Flask 3 Flask 4 CO 2 (g) CO 2 (g) CaCO 3 (s) CaO(s) CaCO 3 (s) CaO(s) A. 1, 2, 3 only B. 1, 2, 4 only C. 1, 3, 4 only D. 3, 4 only 9. Which of the following forward reactions demonstrates decreasing enthalpy and increasing entropy?? 1 A. g( l) + O ( g) Æ go( s) D = kj ? B. 2Cl( g) Æ ( g) + Cl ( g) D = + 185kJ 2 2? C. 2gO( s) Æ 2g( l) + O ( g) D = + 182kJ? D. 2SO ( g) Æ 2SO ( g) + O ( g) D = 200 kj Province of British Columbia. All rights reserved. Page 5
10 Use the following equilibrium system to answer questions 10 to 12. 4N ( g) + 3O ( g) Æ 2N ( g) + 6 O( l) D = 1530kJ Which of the following would cause the amount of N 3 at equilibrium to increase? A. an increase in [ O 2 ] B. a decrease in volume C. a decrease in temperature D. an increase in temperature 11. What happens when O 2 is added to the above system? Equilibrium [ N 2 ] A. no shift unchanged B. shifts right decreases C. shifts right increases D. shifts left increases 12. If some O 2 is injected into the system, what happens to the forward and reverse reaction rates during the shift to reestablish equilibrium? Forward Reaction Rate Reverse Reaction Rate A. increases decreases B. decreases decreases C. increases increases D. decreases increases Page Province of British Columbia. All rights reserved.
11 13. Consider the equilibrium expression K eq1 for reaction 1: 1 SO ( g) + O ( g) Æ SO ( g) and the equilibrium expression K eq2 for reaction 2: 2SO ( g) Æ O ( g) + 2SO ( g) ow is K eq2 related to K eq1? A. K = K eq2 eq1 = ( ) 2 B. K K eq2 eq C. K D. K eq2 eq2 = Ê Ë Á 1 ˆ K eq1 = Ê Ë Á 1 ˆ K eq Which of the following describes how a K eq value is related to the relative concentrations of reactants and products? K eq value Relative Concentration I. large [ products] > [ reactants] II. large [ reactants] > [ products] III. small [ products] > [ reactants] IV. small [ reactants] > [ products] A. I only B. IV only C. I and IV only D. II and III only 2005 Province of British Columbia. All rights reserved. Page 7
12 15. Consider the following equilibrium system: N2( g) + O2( g) Æ 2NO( g) Under certain conditions, K eq = When conditions are changed, Keq becomes Which of the following could account for this? A. [ N 2 ] was changed. B. A catalyst was added. C. Pressure was changed. D. Temperature was changed. 16. Consider the following equilibrium system: 2Sg ( ) Æ 2 ( g) + S ( g) At equilibrium, a 20. L reaction vessel contained mol 2S, mol 2 and mol S 2. What is the value of K eq? A B C D Consider the following equilibrium equation: CaCO3( s) Æ CaO( s) + CO2( g) Keq = 010. Initially, g CaCO 3 were placed in a 20. L container. What mass of CO 2 will be present at equilibrium? A g CO2 B. 88. gco2 C. 15gCO2 D. 22. g CO2 Page Province of British Columbia. All rights reserved.
13 18. The solubility of a solute is best determined from which type of solution? A. a saturated solution B. any solution at 25 C C. an unsaturated solution D. a supersaturated solution 19. What will be the [ Cl ] when equal volumes of 010. M NaCl and 020. M AlCl 3 are combined? A M B M C M D M 20. Which equation represents the reaction between 0. 2MNa2CO 3 and 0. 2M Ba( NO3 ) 2? A. Na ( aq) + NO ( aq) Æ NaNO ( s) B. Ba ( aq) + CO ( aq) Æ BaCO ( s) C. Na CO ( s) Æ Na ( aq) + CO ( aq) D. Ba( NO ) ( aq) + Na CO ( aq) Æ BaCO ( aq) + 2NaNO ( s) Which of the following solutions could be used to separate the anions SO 4 2 and CO 3 2 from each other by precipitation? A. NaNO3 ( aq) B. AgNO3 ( aq) C. Fe( NO3 ) 3 ( aq) D. Ba( NO3 ) 2 ( aq) 2005 Province of British Columbia. All rights reserved. Page 9
14 22. Which pair of ions would be suitable for removing the cations responsible for hard water? A. + and Cl B. NO 3 and I C. S 2 2 and SO 4 2 D. CO 3 3 and PO What is the K sp expression for Zn( O) 2? sp = [ ][ ] sp = [ ] [ ] sp = 2 [ + ][ 2 2 ] sp = [ + ] + [ ] A. K Zn O B. K Zn O C. K Zn O 2 2 D. K Zn 2 O 24. Which compound will have the lowest solubility? A. BeS B. FeS C. ZnS D. Cs 2 S 25. A solution is found to have an initial Pb 2 + What will be observed as the ions interact? [ ] of M and a Br [ ] of M. Observation Reason A. precipitate Trial K > K B. precipitate Trial K < K C. no precipitate Trial K > K D. no precipitate Trial K < K sp sp sp sp sp sp sp sp Page Province of British Columbia. All rights reserved.
15 26. Which relationship can be used to calculate the maximum Ba 2 + solution of Na 3PO4? 2 + Ksp A. [ Ba ] = 3 [ PO4 ] B. Ba C. Ba 2 + [ ] = 2 + [ ] = K PO 3 2 sp 3 [ 4 ] K PO sp 3 [ 4 ] [ ] = [ ] sp 4 D. Ba K PO [ ] that can exist in a 27. What is produced when C3N2 acts as a base in water? A. C3N + B. C3N3 + C. C3N2 D. C2N2 28. What species will form when + ions are in the presence of O 2 molecules? A. O + B. + O 2 + C. O 3 + D. O What is the conjugate acid of the base AsO 4 2? A. AsO B. 2AsO4 C. 2AsO4 D. AsO Province of British Columbia. All rights reserved. Page 11
16 30. Which solution will have the greatest electrical conductivity? A M Cl B M RbO C M K3PO4 D. 20. M C612O6 31. The following equilibrium favours the formation of products: N O + C N Æ C N + N O Which species is the strongest acid? + A. N3O B. N O 2 C. C3N2 + D. C3N3 32. Which of the following solutions would have the greatest [ O ]? A. 01. M CO 3 B M PO 4 C. 01. M 2PO 4 D. 01. M 2BO Given that the ionization of water is endothermic, which of the following is true if temperature is decreased? K w Reason A. decreases equilibrium shifts left B. decreases equilibrium shifts right C. increases equilibrium shifts left D. increases equilibrium shifts right Page Province of British Columbia. All rights reserved.
17 34. Which of the following would be a typical p of soda pop? A. 10. B. 32. C. 68. D What is the [ KO] in a KO solution that has a p = ? A M B M C. 20. M D M What is the [ O 3 ] in 070. M CN? A M B M C M D M 37. The S 2 ion is a relatively strong base with an equilibrium constant of What is the K a value for S? A B C D Province of British Columbia. All rights reserved. Page 13
18 38. Which of the following is true as a result of the predominant hydrolysis of NaCO 3? Solution Reason A. basic K > K B. basic K > K C. acidic K > K D. acidic K > K a b a b b a b a 39. A salt forms in the reaction between F( aq) and NaO( aq). What is the net ionic equation for the hydrolysis of this salt? + A. NaF( aq) Æ Na ( aq) + F ( aq) + B. F( aq) + O( l) Æ O ( aq) + F ( aq) 2 3 C. F ( aq) + O( ) Æ F( aq) + O ( aq) 2 l D. F( aq) + NaO( aq) Æ NaF( aq) + 2O( l) 40. What is the K a for the indicator that is yellow in its basic form and blue in its acid form? A B C D What term is used to describe the point at which a chemical indicator changes colour? A. titration point B. transition point C. equivalence point D. stoichiometric point Page Province of British Columbia. All rights reserved.
19 42. When ml samples of the strong acid SO following results were obtained: 2 4 were titrated with 025. M NaO the Titration Volume of NaO( aq) ml ml mL What is the concentration of the SO 2 4 sample? A M B M C M D M 43. Which of the following equations describes the predominant reaction that occurs at the equivalence point of a titration between C3 COO( aq) and NaO( aq)? + A. ( aq) + O ( aq) Æ O( ) 2 l B. C COO ( aq) + O( l) Æ C COO( aq) + O ( aq) C. C3COO( aq) + NaO( aq) Æ NaC3COO( aq) + 2O( l) D. ( aq) + CCOO ( aq) + Na ( aq) + O ( aq) Æ Na ( aq) + C COO ( aq) + O( ) l 2005 Province of British Columbia. All rights reserved. Page 15
20 Use the following equilibrium equation and data to answer questions 44 and CN( aq) + O( l) Æ O ( aq) + CN ( aq) M M M 44. Why is the solution above not considered to be a true buffer solution? A. excessive [ CN] B. + excessive O 3 [ ] [ ] C. insufficient CN D. insufficient [ CN] 45. What could be added to 1. 0L of this solution in order for it to behave as a true buffer? A. 10. mol Cl B. 10. mol CN C. 10. mol 3O + D. 10. mol NaCN 46. Which of the following equations correctly represents the reaction of a metallic oxide with water? A. KO 2 + O 2 Æ 2KO B. SO3 + 2O Æ2SO4 C. Na2O + 2O Æ Na2O2 + 2 D. NaO + O Æ Na + 2 O 2 2 Page Province of British Columbia. All rights reserved.
21 47. Identify the substance that is oxidized in the following equation: A. Br 2 B. SO 2 C. O 2 D. Na2SO4 Br + SO + Na SO + 2 O Æ 2 SO + 2NaBr What is the reducing agent in the following equation? Fe + 2I Æ 2Fe + I 2 A. I 2 B. I C. Fe 2 + D. Fe What is the oxidation number of C in the CO ion? A. 1 3 B. 2 3 C. 1 D A solution of Ag( NO 3 ) 2 (an unusual form of silver) reacts with gold metal while a solution of AgNO 3 does not react with gold. What is the order of oxidizing agents when arranged from strongest to weakest? A. Ag, Au, Ag B. Au, Ag, Ag C. Ag, Au, Ag D. Ag, Ag, Au Province of British Columbia. All rights reserved. Page 17
22 51. Which of the following best describes what happens when lead solid is placed in a 1. 0M solution of Cu( NO 3 ) 2? A. Bubbles form on the lead. B. No changes are observed. C. Copper solid forms on the lead and the solution changes colour. D. The mass of lead solid increases and the solution does not change colour. 52. Consider the following redox reaction: 2KClO + 2 C O Æ 2ClO + 2CO + K C O + 2 O What is the oxidation halfreaction? A. 2e + C O Æ 2 + 2CO B. CO Æ 2 + 2CO + 2e + C. 2 + ClO3 Æ ClO2 + 2O + e D. e + + ClO Æ ClO + O 53. A g sample of impure NaI is analyzed by titration with M CuSO 4 solution according to the following equation: 2 + 4I + 2Cu Æ 2CuI + I 2 ow many moles of NaI are present in the sample if the titration requires ml of CuSO 4 solution? A mol B mol C mol D mol Page Province of British Columbia. All rights reserved.
23 Use the following cell diagram for questions 54 to 56. electrons Volts inert electrode 1.0 M KNO3 Cd 1.0 M g(no 3 ) M Cd(NO3 )2 g(l) 54. Which of the following is the correct anode halfcell reaction? 2 + A. Cd + 2e Æ Cd 2 + B. g + 2e Æ g 2 + C. g Æ g + 2e 2 + D. Cd Æ Cd + 2e 55. Which of the following describes the change in mass of the g( l) and the movement of nitrate ions? Mass of g( l) Nitrate Ions A. increases towards the Cd electrode B. decreases towards the Cd electrode C. increases towards the inert electrode D. decreases towards the inert electrode 56. If the standard cell voltage is 125. V, what is the reduction halfcell potential for Cd? A V B V C V D V 2005 Province of British Columbia. All rights reserved. Page 19
24 57. Consider the following electrochemical cell: 2 (g) Pt (inert) Porous Barrier Cu 1.0 M Cl 1.0 M CuSO 4 Which of the following could be used to confirm the ion migration through the porous barrier? A. adding phenolphthalein to the copper halfcell B. adding phenolphthalein to the hydrogen halfcell C. adding barium nitrate solution to the copper halfcell D. adding barium nitrate solution to the hydrogen halfcell 58. Which of the following is an example of corrosion? A. copper spontaneously oxidizing B. sulphur spontaneously oxidizing C. copper nonspontaneously oxidizing D. sulphur nonspontaneously oxidizing Page Province of British Columbia. All rights reserved.
25 59. A student brought an old silver medal to the Chemistry Lab to plate it with copper. e set up a cell like the one in the following diagram: Object 1 Object 2 Medal 1.0 M CuSO 4 Which of the following combinations should produce the best result? Object 1 Electron Flow Object 2 A. AC power supply towards the medal Ag B. DC power supply towards the medal copper C. DC power supply from the medal copper D. voltmeter from the medal Pt 60. Which of the following occurs when a solution of NiSO 4 is electrolyzed using inert carbon electrodes? A. The cathode dissolves. B. ydrogen gas is produced. C. The p of the solution decreases. D. The Ni 2 + concentration increases. This is the end of the multiplechoice section. Answer the remaining questions directly in this examination booklet Province of British Columbia. All rights reserved. Page 21
26 PART B: WRITTEN RESPONSE Value: 30 marks INSTRUCTIONS: Suggested Time: 40 minutes You are expected to communicate your knowledge and understanding of chemical principles in a clear and logical manner. Your steps and assumptions leading to a solution must be written in the spaces below the questions. Answers must include units where appropriate and be given to the correct number of significant figures. For questions involving calculations, full marks will NOT be given for providing only an answer. 1. Consider the following reaction mechanism: Step 1 Cl2 Æ 2Cl (fast) Step 2 Cl + CO Æ COCl (slow) Step 3 COCl + Cl2 Æ COCl2 + Cl (fast) Identify a reaction intermediate in the reaction mechanism and write the equation for the overall reaction. Explain why increasing the CO but increasing the Cl 2 Reaction Intermediate: Overall Reaction Equation: Explanation: [ ] will increase the reaction rate, [ ] will not. (5 marks) Page Province of British Columbia. All rights reserved.
27 2. Consider the following equilibrium: CO( g) + O( g) Æ CO ( g) + ( g) K = eq 46. Initially, 050. mol CO, 050. mol 2O, 0. 62mol CO 2 and 0. 62mol 2 are placed in a 10. L container, and the reaction proceeds towards products. Calculate the equilibrium [ 2 ]. (3 marks) 3. A solution is prepared by mixing equal moles of Ba( NO 3 ) 2, K2SO4 and BaS and precipitation occurs. Identify the precipitate(s) and write the net ionic equation(s) for the reaction(s). (3 marks) Precipitate(s): Net Ionic Equation(s): 2005 Province of British Columbia. All rights reserved. Page 23
28 4. Write balanced equations to show water acting as an acid with C3C2N2, then water acting as a base with 2 O 2. (4 marks) As an acid: As a base: 5. Calculate the initial concentration of a solution of N 3 which has a p = and Kb = Begin by writing the equation for the predominant reaction. (5 marks) Page Province of British Columbia. All rights reserved.
29 6. A sample of the strong acid Cl( aq) is titrated with a sample of N3 ( aq), a weak base. Write the formula, complete ionic and net ionic equations for the titration reaction. (3 marks) 7. In an unusual compound, IPO 4, iodine exists as Iodine(III). The compound decomposes as follows: 3 IPO Æ I + IO + PO ( acidic) Balance this redox equation in acidic solution. (4 marks) 2005 Province of British Columbia. All rights reserved. Page 25
30 8. In separate electrolysis experiments, 10. M NaCl, 10. M KNO 3, 10. M Li2SO 4, and 10. M Cs3PO 4 all produced the same gas at their cathodes. Write the equation for the formation of this gas and explain why this same reaction occurs in all four cases. (3 marks) END OF EXAMINATION Page Province of British Columbia. All rights reserved.
PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS
INSERT STUDENT I.D. NUMBER (PEN) STICKER IN THIS SPACE JUNE 1998 PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS 1. Insert the stickers with your Student I.D. Number (PEN)
More informationChemistry 12 AUGUST Course Code = CH. Student Instructions
MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry 12 2001 Ministry of Education AUGUST 2001 Course
More informationPROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS
INSERT STUDENT I.D. NUMBER (PEN) STICKER IN THIS SPACE APRIL 1996 PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS 1. Insert the stickers with your Student I.D. Number (PEN)
More informationChemistry 12 JANUARY Course Code = CH. Student Instructions
MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry 12 2002 Ministry of Education JANUARY 2002 Course
More informationChemistry 12 APRIL Course Code = CH. Student Instructions
MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry 12 2002 Ministry of Education APRIL 2002 Course Code
More informationCHEMISTRY 12 JUNE 2000 STUDENT INSTRUCTIONS
Insert Personal Education Number (PEN) here. Insert only pre-printed PEN label here. STUDENT INSTRUCTIONS 1. Insert the stickers with your Personal Education Number (PEN) in the allotted spaces above.
More informationChemistry 12. Resource Exam B. Exam Booklet
Chemistry 12 Resource Exam B Exam Booklet Contents: 21 pages Examination: 2 hours 50 multiple-choice questions in the Exam Booklet Additional Time Permitted: 60 minutes Province of British Columbia PART
More informationChemistry 12 August 2005 Provincial Examination
Chemistry 12 August 2005 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 August 2003 Provincial Examination
Chemistry 1 August 003 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationSCH4U: EXAM REVIEW. 2. Which of the following has a standard enthalpy of formation of 0 kj mol -1 at 25ºC and 1.00 atm?
SCH4U_08-09 SCH4U: EXAM REVIEW 1. The heat of a reaction is equal to: a. enthalpy (products) + enthalpy (reactants) b. enthalpy (reactants) enthalpy (products) c. enthalpy (products) enthalpy (reactants)
More informationAcids and Bases Part One Monster Review. Which of the following are general properties of bases in aqueous solution?
Chemistry 1 Acids and Bases Part One onster Review 1 Which of following are general properties of bases in ueous solution? feel slippery and increase [ O ] turn litmus red and accept a proton conduct electricity
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 informationChemistry 12 June 2003 Provincial Examination
Chemistry 12 June 2003 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationELECTROCHEMISTRY. Electrons are transferred from Al to Cu 2+. We can re write this equation as two separate half reactions:
ELECTROCHEMISTRY A. INTRODUCTION 1. Electrochemistry is the branch of chemistry which is concerned with the conversion of chemical energy to electrical energy, and vice versa. Electrochemical reactions
More informationBCIT Winter Chem Final Exam
BCIT Winter 2017 Chem 0012 Final Exam Name: Attempt all questions in this exam. Read each question carefully and give a complete answer in the space provided. Part marks given for wrong answers with partially
More informationSOLUBILITY REVIEW QUESTIONS
Solubility Problem Set 1 SOLUBILITY REVIEW QUESTIONS 1. What is the solubility of calcium sulphate in M, g/l, and g/100 ml? 2. What is the solubility of silver chromate? In a saturated solution of silver
More informationChemistry 112 Name Exam III Form A Section November 13,
Chemistry 112 Name Exam III Form A Section November 13, 2012 email IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white
More informationAP Questions: Electrochemistry
AP Questions: Electrochemistry I 2 + 2 S 2O 2-3 2 I - + S 4O 2-6 How many moles of I 2 was produced during the electrolysis? The hydrogen gas produced at the cathode during the electrolysis was collected
More information( ) SENIOR 4 CHEMISTRY FINAL PRACTICE REVIEW TEST VALUE: TOTAL 100 MARKS. Multiple Choice. Ca (PO ) 3Ca + 2PO. Name Student Number
SENIOR 4 CHEMISTRY FINAL PRACTICE REVIEW TEST Name Student Number Attending Phone Number Address NonAttending ANSWER EY VALUE: TOTAL 100 MARS PART A Multiple Choice 1. (c) Using the solubility chart i)
More informationName AP CHEM / / Collected Essays Chapter 17
Name AP CHEM / / Collected Essays Chapter 17 1980 - #2 M(s) + Cu 2+ (aq) M 2+ (aq) + Cu(s) For the reaction above, E = 0.740 volt at 25 C. (a) Determine the standard electrode potential for the reaction
More information] after equilibrium has been established?
Chemistry 1 Solubility Equilibrium onster Review 1. A saturated solution forms when a 0. 10 mol of salt is added to 10. L of water. The salt is A. Li S B. CuBr C. Zn( OH) ( ) D. NH CO 4. Consider the following
More informationCHAPTER 5 REVIEW. C. CO 2 D. Fe 2 O 3. A. Fe B. CO
CHAPTER 5 REVIEW 1. The following represents the process used to produce iron from iron III oxide: Fe 2 O 3 + 3CO 2Fe + 3CO 2 What is the reducing agent in this process? A. Fe B. CO C. CO 2 D. Fe 2 O 3
More informationChemistry 12 - Learning Outcomes
Chemistry 12 - Learning Outcomes A: Chapt 1. Reaction Kinetics - (Introduction) A1. give examples of reactions proceeding at different rates A2. describe rate in terms of some quantity (produced or consumed)
More informationWhich of the following units could be used to express reaction rate? Reaction Kinetics Monster Review
Chemistry 12 Reaction Kinetics Monster Review 1. Which of the following units could be used to express reaction rate? A. ml s B. ml g C. g ml D. ml mol 2. Consider the reaction: Zn( s) + 2HCl( aq) ZnCl2(
More informationBIG IDEAS. Reaction Kinetics Reactants must collide to react. Conditions surrounding a reaction determine its rate.
Area of Learning: SCIENCE Chemistry Grade 12 Ministry of Education BIG IDEAS Dynamic Equilibrium Solubility Equilibrium Acids and Bases Oxidation-Reduction Some chemical reactions are reversible and proceed
More informationChemistry 30 Review Test 3 Redox and Electrochemistry /55
Chemistry 30 Review Test 3 Redox and Electrochemistry /55 Part I Multiple choice / Numerical Response Answer the following multiple choice questions on the scantron sheet. Answer the numerical response
More informationReaction Kinetics Multiple Choice
Reaction Kinetics Multiple Choice January 1999 1. Consider the reaction: Ca (s) + 2H 2 O (l) Ca(OH) 2 (aq) + H 2 (g) At a certain temperature, 2.50 g Ca reacts completely in 30.0 seconds. The rate of consumption
More informationChemistry 12 April 2003 Provincial Examination
Chemistry 12 April 2003 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 January 2002 Provincial Examination
Chemistry 12 January 2002 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
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 informationChemistry 12 June 2000 Provincial Examination
Chemistry 1 June 000 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationConcentration 0. 5 M solutions 1. 0 M solutions. Rates Fast Slow. Which factor would account for the faster reaction rate in Experiment 1?
72. Consider the following experimental results: Experiment 1 Experiment 2 2+ - - 4 2 2 4 aq Reactants Fe ( aq) + MnO4 ( aq) MnO ( aq) + H C O ( ) Temperature 20 C 40 C Concentration 0. 5 M solutions 1.
More informationChemistry 12 January 2000 Provincial Examination
Chemistry 2 January 2000 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 12 Provincial Exam Workbook Unit 03: Solubility Equilibrium. Multiple Choice Questions
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 1 / 7 Chemistry 1 Provincial Exam Workbook Unit 0: Solubility Equilibrium Multiple Choice Questions 1. Which of the following would be true
More informationSolubility Multiple Choice. January Which of the following units could be used to describe solubility? A. g/s B. g/l C. M/L D.
Solubility Multiple Choice January 1999 14. Which of the following units could be used to describe solubility? A. g/s B. g/l C. M/L D. mol/s 15. Consider the following anions: When 10.0mL of 0.20M Pb(NO3)
More informationChemistry 12 August 2002 Provincial Examination
Chemistry 12 August 2002 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationCHEMISTRY 13 Electrochemistry Supplementary Problems
1. When the redox equation CHEMISTRY 13 Electrochemistry Supplementary Problems MnO 4 (aq) + H + (aq) + H 3 AsO 3 (aq) Mn 2+ (aq) + H 3 AsO 4 (aq) + H 2 O(l) is properly balanced, the coefficients will
More information8. Draw Lewis structures and determine molecular geometry based on VSEPR Theory
Chemistry Grade 12 Outcomes 1 Quantum Chemistry and Atomic Structure Unit I 1. Perform calculations on wavelength, frequency and energy. 2. Have an understanding of the electromagnetic spectrum. 3. Relate
More information(c) dilute solution of glucose (d) chloroform 12 Which one of the following represents the same net reaction as the electrolysis of aqueous H2SO4
1 Electrolysis is the process in which a chemical reaction takes place at the expense of (a) chemical energy (b) electrical energy (c) heat energy (d) none of these 2 Standard hydrogen electrode has an
More informationCHEM 12 Unit 3 Review package (solubility)
CHEM 12 Unit 3 Review package (solubility) 1. Which of the following combinations would form an ionic solid? A. Metalloid - metal B. Metal non-metal C. Metalloid metalloid D. Non-metal non-metal 2. Which
More information1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions)
Chemistry 12 Solubility Equilibrium II Name: Date: Block: 1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions) Forming a Precipitate Example: A solution may contain the ions Ca
More informationAP Chemistry: Electrochemistry Multiple Choice Answers
AP Chemistry: Electrochemistry Multiple Choice Answers 14. Questions 14-17 The spontaneous reaction that occurs when the cell in the picture operates is as follows: 2Ag + + Cd (s) à 2 Ag (s) + Cd 2+ (A)
More informationElectrochemistry. A. Na B. Ba C. S D. N E. Al. 2. What is the oxidation state of Xe in XeO 4? A +8 B +6 C +4 D +2 E 0
Electrochemistry 1. Element M reacts with oxygen to from an oxide with the formula MO. When MO is dissolved in water, the resulting solution is basic. Element M is most likely: A. Na B. Ba C. S D. N E.
More informationChemistry 12 June 1998 Provincial Examination
Chemistry 12 June 1998 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationSolubility & Equilibrium Unit Review
Solubility & Equilibrium Unit Review This review is worth 3 marks of your total test marks. It must be completed on test day. 3 marks will be given to students who have fully completed this review with
More informationChapter Test B. Chapter: Chemical Equilibrium. following equilibrium system? 2CO(g) O 2 (g) ^ 2CO 2 (g)
Assessment Chapter Test B Chapter: Chemical Equilibrium PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. What is
More informationChemistry 12 April 1998 Provincial Examination
Chemistry 12 April 1998 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
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 informationSection A: Summary Notes
ELECTROCHEMICAL CELLS 25 AUGUST 2015 Section A: Summary Notes Important definitions: Oxidation: the loss of electrons by a substance during a chemical reaction Reduction: the gain of electrons by a substance
More informationWksht 4.2 Aqueous Equilibria II
Wksht 4.2 Aqueous Equilibria II Date: 10/16/17 1. Label the type of titration each graph represents and whether their equivalence point ph values would be greater than, equal to, or less than 7. WA being
More information40S CHEMISTRY FINAL EXAM PROBLEM REVIEW SHEET:
40S CHEMISTRY FINAL EXAM PROBLEM REVIEW SHEET: **THIS IS NOT A COMPLETE REVIEW. CONTINUE TO READ ALL COURSE NOTES, GO OVER ALL WORKSHEETS, HANDOUTS, AND THE UNIT TESTS TO BE BETTER PREPARED. To prepare
More informationCHEMISTRY 102 FALL 2010 FINAL EXAM FORM C Section 502 DR. KEENEY-KENNICUTT PART 1
NAME (Block Print) CHEMISTRY 102 FALL 2010 FINAL EXAM FORM C Section 502 DR. KEENEY-KENNICUTT Directions: (1) Put your name on PART 1 and your name and signature on PART 2 of the exam where indicated.
More informationCHEMISTRY 12 SYLLABUS Online 2010
CHEMISTRY 12 SYLLABUS Online 2010 Mr. Lockwood Email: plockwood@sd43.bc.ca Personal: https://my43.sd43.bc.ca/schools/pinetreesecondary/classes/plockwood/default.aspx UserName: Password: WebCT: http://bb.etc.bc.ca/webct/entrypageins.dowebct
More informationUNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12)
I. Multiple Choice UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) 1) Which one of the following would form an ionic solution when dissolved in water? A. I 2 C. Ca(NO 3 ) 2 B. CH 3 OH D.
More informationDate Topics Problems Video(s) Due One Review tests, introduce red-ox, identify oxidizing and reducing agents
Chapter 20: Electrochemistry. Tentative Schedule Date Topics Problems Video(s) Due One Review tests, introduce redox, identify oxidizing and reducing agents Oxidation numbers / oxidizing and reducing agents
More informationCHEM J-14 June 2014
CHEM1101 2014-J-14 June 2014 An electrochemical cell consists of an Fe 2+ /Fe half cell with unknown [Fe 2+ ] and a Sn 2+ /Sn half-cell with [Sn 2+ ] = 1.10 M. The electromotive force (electrical potential)
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 information4. Which of the following equations represents an endothermic reaction?
Chem 12 Practice Kinetics Test 1. Consider the following reaction mechanism: step 1: M + X MX step 2: MX + A D + X The chemical species MX is a(n) A. catalyst B. inhibitor C. final product D. reaction
More informationChem 1120 Pretest 3 Sprin 2015
Name: Class: Date: Chem 1120 Pretest 3 Sprin 2015 Multiple Choice Identify the choice that best completes the statement or answers the question. Chapter 19 Values The following equilibrium constants will
More informationELECTROCHEMISTRY OXIDATION-REDUCTION
ELECTROCHEMISTRY Electrochemistry involves the relationship between electrical energy and chemical energy. OXIDATION-REDUCTION REACTIONS SPONTANEOUS REACTIONS Can extract electrical energy from these.
More informationAP* Electrochemistry Free Response Questions page 1
Galvanic (Voltaic) Cells 1988 Average score = 5.02 a) two points Sn ---> Sn 2+ + 2e Ag + + e ---> Ag AP* Electrochemistry Free Response Questions page 1 b) two points 2 Ag + + Sn ---> 2 Ag + Sn 2+ E =
More informationChem 12 Practice Solubility Test
Chem 12 Practice Solubility Test 1. Which combination of factors will affect the rate of the following reaction? Zn (s) + 2HCl ZnCl 2 + H 2(g) A. Temperature and surface area only B. Temperature and concentration
More informationREACTION RATES AND EQUILIBRIUM
Name Date Class 18 REACTION RATES AND EQUILIBRIUM SECTION 18.1 RATES OF REACTION (pages 541 547) This section explains what is meant by the rate of a chemical reaction. It also uses collision theory to
More informationA voltaic cell using the following reaction is in operation: 2 Ag + (lm) + Cd(s) 2 Ag(s) + Cd 2+ (l M)
0. Cu (s) + 2Ag + Cu 2+ + 2Ag (s) If the equilibrium constant for the reaction above is 3.7x10 15, which of the following correctly describes the standard voltage, E o and the standard free energy change,
More informationExam3Fall2009thermoelectro
Exam3Fall2009thermoelectro Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Thermodynamics can be used to determine all of the following EXCEPT
More informationChemistry 12 August 2008 Form A Provincial Examination Answer Key
Cognitive Processes K = Knowledge U = Understanding H = Higher Mental Processes Topics 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation Reduction
More informationChemistry 12 April 2004 Provincial Examination
Chemistry 12 April 2004 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationStudent Achievement. Chemistry 12
Student Achievement Chemistry 12 Key Elements: Reaction Kinetics Estimated Time: 14 16 hours By the end of this course, students will be able to explain the significance of reaction rates, demonstrate
More informationChemistry 12 April 2001 Provincial Examination
Chemistry 1 April 001 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationChemistry 40S. Final Exam Review Package. Multiple Choice Section
Chemistry 40S Final Exam Review Package Multiple Choice Section Aqueous Reactions 1. What is the net ionic equation when solutions of silver nitrate and sodium acetate are mixed? a. Na + (aq) + NO 3 -
More informationCHEMICAL REACTIONS. Introduction. Chemical Equations
CHEMICAL REACTIONS Chemistry I Chapter 7 1 Chemical Equations Their Job: Depict the kind of reactants and products and their relative amounts in a reaction. 4 Al (s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) The
More informationChapter 19: Electrochemistry
Chapter 19: Electrochemistry Overview of the Chapter review oxidation-reduction chemistry basics galvanic cells spontaneous chemical reaction generates a voltage set-up of galvanic cell & identification
More informationOxidation-Reduction Reactions and Introduction to Electrochemistry
ADVANCED PLACEMENT CHEMISTRY Oxidation-Reduction Reactions and Introduction to Electrochemistry Students will be able to: identify oxidation and reduction of chemical species; identify oxidants and reductants
More informationChapter 20. Electrochemistry Recommendation: Review Sec. 4.4 (oxidation-reduction reactions) in your textbook
Chapter 20. Electrochemistry Recommendation: Review Sec. 4.4 (oxidation-reduction reactions) in your textbook 20.1 Oxidation-Reduction Reactions Oxidation-reduction reactions = chemical reactions in which
More informationReview 7: Solubility Equilibria
Review 7: Solubility Equilibria Objectives: 1. Be able to write dissociation equations for ionic compounds dissolving in water. 2. Given Ksp, be able to determine the solubility of a substance in both
More informationUnit #8, Chapter 10 Outline Electrochemistry and Redox Reactions
Unit #8, Chapter 10 Outline Electrochemistry and Redox Reactions Lesson Topics Covered Homework Questions and Assignments 1 Introduction to Electrochemistry definitions 1. Read pages 462 467 2. On page
More informationhttp://redoxanswers.weebly.com REDOX LESSON LEARNING GOALS http://redoxanswers.weebly.com Lesson 1: Introduction to Redox Relate to examples of oxidation-reduction reactions in the real-world. Understand
More informationBonus Final Exam 3. 1 Calculate the heat of reaction,δh 0 rxn, for the following reaction as written at 298 K: g 2H 2 CH 4. g CF 4.
Bonus Final Exam 3 1 Calculate the heat of reaction,δh rxn, for the following reaction as written at 298 K: CH 4 2F 2 CF 4 2H 2 substance CH 4 CF 4 ΔH f kj/mol 75 68 (A) ΔH rxn 23 kj (B) ΔH rxn 914 kj
More informationChapter 19 ElectroChemistry
Chem 1046 General Chemistry by Ebbing and Gammon, 9th Edition George W.J. Kenney, Jr, Professor of Chemistry Last Update: 11July2009 Chapter 19 ElectroChemistry These Notes are to SUPPLIMENT the Text,
More informationChemistry 12 Provincial Workbook Unit 01: Reaction Kinetics. Multiple Choice Questions
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 01), P. 1 / 68 Chemistry 1 Provincial Workbook Unit 01: Reaction Kinetics Multiple Choice Questions 1. Which of the following describes what happens
More informationChem 110 General Principles of Chemistry
Chem 110 General Principles of Chemistry Chapter 3 (Page 88) Aqueous Reactions and Solution Stoichiometry In this chapter you will study chemical reactions that take place between substances that are dissolved
More informationWhich of the following factors will not alter the position of equilibrium?
86 N( g) + 3H $ ( g) NH3 ( g) Which of the following factors will not alter the position of uilibrium? A a pressure decrease B a temperature increase C the presence of a catalyst D the addition of more
More informationChemistry 3202 Pre-Public Examination May 2012 Name:
Chemistry 3202 Pre-Public Examination May 2012 Name: Section A: Multiple Choice This section contains 40 multiple choice covering concepts from the entire course. Please answer all multiple choice items
More informationChemistry 12 June 2002 Provincial Examination
Chemistry 1 June 00 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation Reduction
More informationElectrochemistry. Outline
Electrochemistry Outline 1. Oxidation Numbers 2. Voltaic Cells 3. Calculating emf or Standard Cell Potential using Half-Reactions 4. Relationships to Thermo, Equilibrium, and Q 5. Stoichiometry 6. Balancing
More informationChemistry 112 Name Exam III Form A Section April 2,
Chemistry 112 Name Exam III Form A Section April 2, 2013 email IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white cover
More informationChemistry 12 August 2007 Form A Provincial Examination Multiple-Choice Key
Chemistry 12 August 2007 Form A Provincial Examination Multiple-Choice Key Cognitive Processes K = Knowledge U = Understanding H = Higher Mental Processes Weightings 11% 78% 11% Question Types 50 = Multiple
More informationName (Print) Section # or TA. 1. You may use a crib sheet which you prepared in your own handwriting. This may be
Name (Print) Section # or TA 1. You may use a crib sheet which you prepared in your own handwriting. This may be one 8-1/2 by 11 inch sheet of paper with handwriting only on one side. 2. You may use a
More informationPHYSICAL SCIENCES: PAPER II
NATIONAL SENIOR CERTIFICATE EXAMINATION NOVEMBER 2014 PHYSICAL SCIENCES: PAPER II Time: 3 hours 200 marks PLEASE READ THE FOLLOWING INSTRUCTIONS CAREFULLY 1. This question paper consists of 14 pages, a
More informationUnit 4-1 Provincial Practice Questions Page 1
Page 1 Page 2 Page 3 Page 4 Page 5 1.00 Page 6 Page 7 Page 8 55. The conjugate base of HAsO 4 2 is A. H 3 O + B. 3 AsO 4 C. H 3 AsO 4 D. H 2 AsO 4 56. Consider the following acidbase equilibrium: HC 6
More information11-1 Notes. Chemical Reactions
11-1 Notes Chemical Reactions Chemical Reactions In a chemical reaction 1 or more substances (the reactants) change into 1 or more new substances (the products). Reactants are always written on the left
More informationSect 7.1 Chemical Systems in Balance HMWK: Read pages
SCH 4UI Unit 4 Chemical Systems and Equilibrium Chapter 7 Chemical Equilibrium Sect 7.1 Chemical Systems in Balance HMWK: Read pages 420-424 *Some reactions are reversible, ie not all reactions are as
More informationUnit 3: Solubility Equilibrium Topic B: Precipitation Reactions and Qualitative Analysis
1 In this topic we will examine: Unit 3: Solubility Equilibrium Topic B: Precipitation Reactions and Qualitative Analysis how to predict if a precipitate forms when solutions are mixed how to selectively
More informationChemistry 201: General Chemistry II - Lecture
Name Date Chemistry 201: General Chemistry II - Lecture Short-Answer Exam #3, 70 Points Total Form: A Read all directions carefully. Answers not conforming to the directions will be marked as incorrect!
More informationChemistry 12 Provincial Exam Workbook Unit 04: Acid Base Equilibria. Multiple Choice Questions
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P. 1 / 69 Chemistry 1 Provincial Exam Workbook Unit 0: Acid Base Equilibria Multiple Choice Questions 1. Calculate the volume of 0.00 M HNO needed
More information4. Using the data from Handout 5, what is the standard enthalpy of formation of N 2 O (g)? What does this mean?
EXTRA HOMEWORK 3A 1. In each of the following pairs, tell which has the higher entropy. (a) One mole of ice or one mole of liquid water (b) One mole of liquid propane or one mole of gaseous propane (c)
More informationCHAPTER 12. Practice exercises
CHAPTER 12 Practice exercises 12.1 2Al(s) + 3Cl 2 (g) 2AlCl 3 (aq) Aluminium is oxidised and is therefore the reducing agent. Chlorine is reduced and is therefore the oxidising agent. 12.3 First the oxidation
More information1. Which one of the following would form an ionic solution when dissolved in water? A. I2 C. Ca(NO3)2 B. CH3OH D. C12H22O11
Chemistry 12 Solubility Equilibrium Review Package Name: Date: Block: I. Multiple Choice 1. Which one of the following would form an ionic solution when dissolved in water? A. I2 C. Ca(NO3)2 B. CH3OH D.
More informationPart A: Multiple Choice (23 marks total)
Part A: Multiple Choice (23 marks total) Use the answer sheet found at the end of this examination to answer the multiple-choice questions in this section. Shade in the circle that corresponds to your
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 information