Chem. 1B Midterm 2 Version B Feb. 24, 2016
|
|
|
- Catherine Pope
- 5 years ago
- Views:
Transcription
1 Chem. B Midterm 2 Version B Feb. 24, 206 First initial of last name Name: Print Neatly. You will lose point if I cannot read your name or perm number. Perm 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. On fundamental and short answer problems you must show your work in order to receive credit for the problem. If your cell phone goes off during the exam you will have your exam removed from you. Fundamentals (of 36 possible) ( )+( ) = Problem (of 6 possible) Problem 2 (of 8 possible) Multiple Choice (of 30 possible) Midterm Total (of 00 possible)
2 Fundamental Questions Each of these fundamental chemistry questions is worth 6 points. You must show work to get credit. Little to no partial credit will be awarded. Make sure to include the correct units on your answers. a) 4 pts A chemistry graduate student is studying the rate of this reaction: 2H3PO4(aq) P2O5(aq) + 3H2O(aq) He fills a reaction vessel with H3PO4 and measures its concentration as the reaction proceeds: Use this data to answer the following questions. Write the rate law for this reaction. (You must show your work to get credit) rate = k Time (minutes) [H3PO4] M M M M M Time (m) [H3PO4] ln[h3po4] The graph of t vs [H 3 PO 4 ] is a straight line therefore, rate=k[h3po4]2 b) 2 pts. Calculate the value of the rate constant k. Round your answers to 2 significant digits. Also be sure your answer has the correct unit symbol. = kt + therefore the slope equal k [A] [A] 0 slope = rise run = M M = 5.8 L 40. m 0 m m Or L s 2) 6 pts What mass of I2 from KI can be produced in.0 h with a current of 5 A? n = It (5 A) F = (.0 h( 96,486 C 2I - I 2 + 2e - 60 m s h )(60 m )) = 0.56 e 0.56 e ( I 2 2 e ) ( g I 2 I 2 ) = 7 g I 2 [H 3 PO 4 ] 3) 6 pts Balance N2H4(aq) + CO3 2- (aq) N2(g) + CO(g) in basic conditions N2H4 N2 + 4H + + 4e - CO H + + 2e - CO + 2H2O N2H4 N2 + 4H + + 4e - 2(CO H + + 2e - CO + 2H2O) N2H4 +2CO H + N2 + 2CO + 4H2O N2H4 +2CO H + + 4OH - N2 + 2CO + 4H2O + 4OH - N2H4(aq) + 2CO3 2- (aq) N2(g) + 2CO(g) + 4OH - (aq) 2
3 4) 6 pts Which of the reaction profiles represents the effect of a catalyst on the rate of reaction? A is the catalysized reaction. 5) 6 pts Draw the following galvanic cell: Pb(s) + Cl2(g) Pb 2+ (aq) + 2Cl - (aq) Calculate E, show the direction of electron flow and the direction of ion migration through the salt bridge, and identify the cathode and anode. Pb Pb e - E = 0.3 V Cl2 + 2e - 2Cl - E =.36 V Cl2(g) + Pb(s) Pb 2+ (aq) + 2Cl - (aq) E =.49 V 6) 6 pts In the first-order reaction A 2B, when the initial concentration of A was M it took 95 s for the concentration to drop to M. How much more time would be needed for the concentration to drop by an additional M. st Order ln[a] = kt + ln[a] o Determine k ln( M) = k(95 s) + ln( M) k = s Determine time ln( M) = (0.002 )t + ln( M) s t = 65s 3
4 Short Answer Questions Each of the following short answer questions are worth the noted points. Partial credit will be given. You must show your work to get credit. Make sure to include proper units on your answer. a) 6 pts Calculate the voltage of the following cell at 298 K Zn(s) Zn 2+ (aq).7 M Ag + (aq) 2.4 M Ag(s) Reaction of Interest Zn Zn e - E = 0.76 V 2(Ag + + e - Ag) E = 0.80 V Zn(s) + 2Ag + (aq) Zn 2+ (aq) + 2Ag(s) E =.56V E = E RT nf ln(q) = E RT nf ln ] ([Zn2+ [Ag + ] 2) E =.56V (8.345 K )(298K) (2)(96,485 C ) ln ( ) =.58 V b) 0 pts What is the voltage for the same cell at 800 K Zn(s) Zn 2+ (aq).7 M Ag + (aq) 2.4 M Ag(s) Hint: Assume ΔH and ΔS are temperature independent. = 42 S Zn K, S Ag = 43 K, S Ag + = 73, K ΔH f(ag+ ) = 05 k Find ΔG at 800 K G = H T S Find ΔH H rxn = H f (Zn 2+ ) + 2 H f (Ag) H f (Zn) 2 H f (Ag + ) H rxn = 53 k + 2(0 k ) 0 k Find ΔS S rxn = S Zn S Ag S Zn 2S Ag + 2(05 k S rxn = 2 + 2(43 ) K K 42 2 (73 ) = 24 K K G = H T S = 363,000 (800K) ( 24 G = 92,000 G = nfe E = G nf 92,000 = (2)(96,485 C ) = V E = 0.995V (8.345 K )(800K) (2)(96,485 C ) ln ( ) =.04 V ) = 363 k K ) K 4
5 2a) 8 pts The reaction 5Br - (aq) + BrO3 - (aq) + 6H + (aq) 3Br2(l) + 3H2O(l) Is expected to obey the mechanism k BrO3 - (aq)+h + (aq) HBrO3(aq) fast equilibrium k k 2 HBrO3(aq)+H + (aq) H2BrO3 + (aq) fast equilibrium k 2 Br - (aq)+h2bro3 + (aq) k 3 (Br-BrO2)(aq)+H2O(l) (Br-BrO2)(aq)+4H + (aq)+4br - (aq) products Write the rate law for this reaction. slow fast rate = k 3 [Br ][H 2 BrO 3 + ] H2BrO3 + is an intermediate therefore, needs to be eliminated from the rate law. Use equilibrium to eliminate the intermediate. k 2 [HBrO 3 ][H + ] = k 2 [H 2 BrO 3 + ] [H 2 BrO 3 + ] = k 2[HBrO 3 ][H + ] k 2 rate = k 3k 2 [Br ][HBrO 3 ][H + ] k 2 HBrO3 is an intermediate therefore, needs to be eliminated from the rate law. Use equilibrium to eliminate the intermediate. k [BrO 3 ][H + ] = k [HBrO 3 ] [HBrO 3 ] = k [BrO 3 ][H + ] k rate = k 3k 2 k [Br ][BrO 3 ][H + ] 2 k k 2 = k[br ][BrO 3 ][H + ] 2 2b) 0 pts Does this mechanism fit with the following experimental data? You must find the experimental rate law to get credit. [Br - ]o (M) [BrO3 - ]o (M) [H + ]o (M) Initial Rate( ) General Rate Law: rate = k[br ] x [BrO 3 ] y [H + ] z From experiments and 2 when the concentration of Br - is double the rate goes up by a factor of 2 therefore st order with respect to Br - From experiments and 3 when the concentration of H + is double the rate goes up by a factor of 4 therefore, 2 nd order with respect to H + From experiments and 4 2 L s = k(.0 M)(.0 M)y (.0 M) 2 36 L s = k(.0 M)(2.0 M)y (.0 M) = (0.50) y y=.6 rate = k[br ][BrO 3 ].6 [H + ] 2 No the mechanism is not consistent. Ls 5
6 Multiple Choice Questions On the ParScore form you need to fill in your answers, perm number, test version, and name. Failure to do any of these things will result in the loss of point. Your perm number is placed and bubbled in under the ID number. Do not skip boxes or put in a hyphen; unused boxes should be left blank. Bubble in your test version (B) under the test form. Note: Your ParScore forms will not be returned to you, therefore, for your records, you may want to mark your answers on this sheet. Each multiple choice question is worth 5 points. Identify the choice that best completes the statement or answers the question. Reaction E (volts) Na + + e Na 2.7 Al e Al.66 Fe e Fe 0.44 Co e Co 0.28 Cu e Cu Ag + + e Ag Cl2 + 2e 2Cl +.36 F2 + 2e 2F Which of the following would be the best reducing agent? a. Na + b. Al 3+ c. F2 d. Al e. F 2. The equilibrium constant for the following general reaction is 0. at 25 C. Calculate E for the cell. X2(s) + Y + (aq) X 2+ (aq) + Y(s) (unbalanced) a V b V c V d V 6
7 3. What time is required to plate a metal tray (24.0 cm x 2.0 cm) with a coating (thickness cm) of silver (density = 0.54 ) using a current of 7.65 A? Neglect the amount of silver required to coat the edges. Helpful Information: The reaction of interest is Ag + + e - Ag and MAg = 07.9 a. 30 s b. 708 s c. 92 s d. 420 s 4. The rate constant for a reaction increases from 0.0 to 00. when the temperature is increased from 35 K to 43 K. What is the activation energy for the reaction in? a b. 8.8 c..0 d In which of the following cases must E be equal to zero? I. In any cell at equilibrium II. In a concentration cell III. E can never be equal to zero. a. II only b. III c. I and II d. I only 6. What reaction occurs at the anode and at the cathode when electrolysis of aqueous MgI2 occurs? Assume standard conditions. Helpful information: I2 + 2e - 2I- E = 0.54 V Mg e - Mg E = V Anode/Cathode a. Water/Magnesium b. Water/Water c. Magnesium/Water d. Iodine/Magnesium 7
Chem. 1B Midterm 2 Version B March 3, 2017
First initial of last name Chem. 1B Midterm 2 Version B March 3, 2017 Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the exam
Chem. 1B Midterm 2 Version A March 3, 2017
First initial of last name Chem. 1B Midterm 2 Version A March 3, 2017 Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the exam
Chem. 1B Midterm 2 Version A
Chem. 1B Midterm 2 Version A First letter of last name 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.
Chem. 1B Midterm 2 Version A
Chem. B Midterm Version A Name Student Number All wor must be shown on the eam for partial credit. Points will be taen off for incorrect or no units and for the incorrect number of significant figures.
Chem. 1B Midterm 1 Version B February 3, 2017
First initial of last name Chem. 1B Midterm 1 Version B February 3, 2017 Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the
Chem. 1B Midterm 1 Version A February 3, 2017
First initial of last name Chem. 1B Midterm 1 Version A February 3, 2017 Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the
Chem. 1B Final Practice Test 2 Solutions
First letter of last name Chem. 1B Final Practice Test 2 Solutions Name Print Neatly. You will lose 1 point if I cannot read your name or perm number. Student Number If you are sitting next to someone
Chem. 1B Midterm 1 Practice Test 2
First letter of last name Chem. 1B Midterm 1 Practice Test 2 Name Print Neatly. You will lose 1 point if I cannot read your name or perm number. Student Number If you are sitting next to someone with the
Chem. 1B Midterm 1 Version A February 9, 2018
First initial of last name Chem. 1B Midterm 1 Version A February 9, 2018 Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the
Chem. 1A Midterm 1 Version A October 19, 2018
First initial of last name Chem. 1A Midterm 1 Version A October 19, 2018 Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the
Chem. 1A Midterm 1 Version A October 20, 2017
First initial of last name Chem. 1A Midterm 1 Version A October 20, 2017 Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the
Chem. 1A Midterm 1 Version B October 20, 2017
First initial of last name Chem. 1A Midterm 1 Version B October 20, 2017 Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the
Chem. 1B Midterm 1 Version A Jan. 29, 2016
Chem. 1B Midterm 1 Version A Jan. 29, 2016 First initial of last name Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the exam
Chem. 1A Midterm 2 Version A November 9, 2018
First initial of last name Chem. 1A Midterm 2 Version A November 9, 2018 Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the
Chem. 1B Midterm 1 Version B February 1, 2019
First initial of last name Chem. 1B Midterm 1 Version B February 1, 2019 Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the
Chem. 1B Midterm 1 Practice Test 1
First letter of last name Chem. 1B Midterm 1 Practice Test 1 Name Print Neatly. You will lose 1 point if I cannot read your name or perm number. Student Number If you are sitting next to someone with the
Chem. 1B Final Practice First letter of last name
Chem. 1B Final Practice First letter of last name 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.
Chem. 1A Midterm 1 Version A October 14, 2016
Chem. 1A Midterm 1 Version A October 14, 2016 First initial of last name Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the
Chem. 1A Midterm 1 Version B October 14, 2016
Chem. 1A Midterm 1 Version B October 14, 2016 First initial of last name Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the
Chem. 1B Final Practice
Chem. 1B Final Practice Name Student Number All work must be shown on the exam for partial credit. Points will be taken off for incorrect or no units and for the incorrect number of significant figures.
Chem 1C Midterm 2 Practice Test 1
Chem 1C Midterm 2 Practice Test 1 First initial of last name Name Perm Number All work must be shown on the exam for partial credit. Points will be taken off for incorrect or missing units. Calculators
Chem. 1A Midterm 2 Version A November 9, 2016
Chem. 1A Midterm 2 ersion A November 9, 2016 First initial of last name Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the exam
Chem. 1A Midterm 2 Version B November 9, 2016
Chem. 1A Midterm 2 ersion B November 9, 2016 First initial of last name Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the exam
Chem. 1C Midterm 2 Version B May 17, 2017
First initial of last name Chem. 1C Midterm 2 Version B May 17, 2017 Name: rint Neatly. You will lose 1 point if I cannot read your name or perm number. erm Number: All work must be shown on the exam for
Chem. 1C Midterm 2 Version B May 11, 2016
Chem. 1C Midterm 2 Version B May 11, 2016 First initial of last name Name: Print Neatly. You will lose 1 point if I cannot read your name or perm number. Perm Number: All work must be shown on the exam
Chem. 1A Midterm 2 Version A
Chem. 1A Midterm 2 Version A Name Student Number All work must be shown on the exam for partial credit. Points will be taken off for incorrect or no units and for the incorrect number of significant figures.
Chem. 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.
CHEMISTRY - CLUTCH CH.18 - ELECTROCHEMISTRY.
!! www.clutchprep.com CONCEPT: OXIDATION-REDUCTION REACTIONS Chemists use some important terminology to describe the movement of electrons. In reactions we have the movement of electrons from one reactant
25. A typical galvanic cell diagram is:
Unit VI(6)-III: Electrochemistry Chapter 17 Assigned Problems Answers Exercises Galvanic Cells, Cell Potentials, Standard Reduction Potentials, and Free Energy 25. A typical galvanic cell diagram is: The
Chem. 1C Midterm 1 Version B April 26, 2017
First initial of last name Chem. C Midterm Version B April 6, 07 Name: Print Neatly. You will lose point if I cannot read your name or perm number. Perm Number: All work must be shown on the exam for partial
Chem. 1C Midterm 1 Version A April 26, 2017
First initial of last name Chem. C Midterm Version A April 6, 07 Name: Print Neatly. You will lose point if I cannot read your name or perm number. Perm Number: All work must be shown on the exam for partial
Chem. 1A Final Practice Test 2
Chem. 1A Final Practice Test 2 All work must be shown on the exam for partial credit. Points will be taken off for incorrect or missing units. Calculators are allowed. Cell phones may not be used as calculators.
Chapter 18 problems (with solutions)
Chapter 18 problems (with solutions) 1) Assign oxidation numbers for the following species (for review see section 9.4) a) H2SO3 H = +1 S = +4 O = -2 b) Ca(ClO3)2 Ca = +2 Cl = +5 O = -2 c) C2H4 C = -2
Chapter 18 Electrochemistry. Electrochemical Cells
Chapter 18 Electrochemistry Chapter 18 1 Electrochemical Cells Electrochemical Cells are of two basic types: Galvanic Cells a spontaneous chemical reaction generates an electric current Electrolytic Cells
Chem. 1A Midterm 2 Practice Test 2
Chem. 1A Midterm 2 Practice Test 2 All work must be shown on the exam for partial credit. Points will be taken off for incorrect or missing units. Calculators are allowed. Cell phones may not be used as
CHEM J-8 June /01(a)
CHEM1001 2012-J-8 June 2012 22/01(a) A galvanic cell has the following cell reaction: D(s) + 2Zn 2+ (aq) 2Zn(s) + D 4+ (aq) Write the overall cell reaction in shorthand cell notation. E = 0.18 V 8 D(s)
Chem. 1C Midterm 1 Practice Test 2
Chem. 1C Midterm 1 Practice Test 2 First initial of last name 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
Oxidation-reduction (redox) reactions
Oxidation-reduction (redox) reactions Reactions in which there are changes in oxidation state (oxidation number) between reactants and products 2 MnO 4- + 10 Br - + 16 H + 2 Mn 2+ + 5 Br 2 + 8 H 2 O One
Bubble in A, B or C as the test form code at the top right of your answer sheet. Bubble in your Section Number also. VERSION X
CHM 2046 Practice Exam 3 Bubble in A, B or C as the test form code at the top right of your answer sheet. Bubble in your Section Number also. VERSION X 1. A reaction has ΔH = -75.0 kj and ΔS = -245 J/K.
Guide to Chapter 18. Electrochemistry
Guide to Chapter 18. Electrochemistry We will spend three lecture days on this chapter. During the first class meeting we will review oxidation and reduction. We will introduce balancing redox equations
CHM 152 Exam 4 Review Ch KEY
CHM 152 Exam 4 Review Ch. 18 19 KEY 1. Predict whether the entropy change will be positive or negative for the following: a. H 2 O (g) H 2 O (l) S - b. C 6 H 12 O 6 (s) 2C 2 H 5 OH(l) + 2CO 2 (g) S +_
Chem. 1A Final Practice Test 1
Chem. 1A Final Practice Test 1 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.
Electrochemical Cells
Electrochemistry Electrochemical Cells The Voltaic Cell Electrochemical Cell = device that generates electricity through redox rxns 1 Voltaic (Galvanic) Cell An electrochemical cell that produces an electrical
Homework #3 Chapter 11 Electrochemistry
Homework #3 Chapter 11 Electrochemistry Chapter 4 83. a) Oxidation ½ Reaction Fe + HCl HFeCl 4 Fe + 4HCl HFeCl 4 Fe + 4HCl HFeCl 4 + 3H + Fe + 4HCl HFeCl 4 + 3H + + 3e Reduction ½ Reaction H 2 2H + H 2
CHEM 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)
BCIT 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
CHM 2046 Practice Final Exam
CHM 2046 Practice Final Exam IMPORTANT: Bubble in A, B or C as the test form code at the top right of your answer sheet AND also bubble in your Section Number and UFID on the left side of your answer sheet.
Chemistry 102 Chapter 19 OXIDATION-REDUCTION REACTIONS
OXIDATION-REDUCTION REACTIONS Some of the most important reaction in chemistry are oxidation-reduction (redox) reactions. In these reactions, electrons transfer from one reactant to the other. The rusting
ELECTROCHEMISTRY OXIDATION-REDUCTION
ELECTROCHEMISTRY Electrochemistry involves the relationship between electrical energy and chemical energy. OXIDATION-REDUCTION REACTIONS SPONTANEOUS REACTIONS Can extract electrical energy from these.
Electrochemical System
Electrochemical System Topic Outcomes Week Topic Topic Outcomes 8-10 Electrochemical systems It is expected that students are able to: Electrochemical system and its thermodynamics Chemical reactions in
Chapter 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
CH Practice Exam #2
CH1810 - Practice Exam #2 Part I - Multiple Choice - Choose the best answer and place the letter corresponding to the answer in the space provided. 1. Consider the following reaction and its equilibrium
Chem. 1A Midterm 1 Practice Test 2
Chem. 1A Midterm 1 Practice Test 2 All work must be shown on the exam for partial credit. Points will be taken off for incorrect or missing units. Calculators are allowed. Cell phones may not be used as
Chemistry 112, Fall 2006, Section 1 (Garman and Heuck) Final Exam A (100 points) 19 Dec 2006
Chemistry 112, Fall 2006, Section 1 (Garman and Heuck) (100 points) 19 Dec 2006 Name: YOU MUST: Put your name and student ID on the bubble sheet correctly. Put the exam version on the bubble sheet on the
Chemistry 223 Spring 2012 Oregon State University Exam 2 May 24, 2012 Drs. Nafshun, Watson, Richardson
Chemistry 223 Spring 2012 Oregon State University Exam 2 May 24, 2012 Drs. Nafshun, Watson, Richardson Instructions: You should have with you several number two pencils, an eraser, your 3" x 5" note card,
DO NOT OPEN UNTIL INSTRUCTED TO DO SO. CHEM 111 Dr. McCorkle Exam #3A KEY. While you wait, please complete the following information:
DO NOT OPEN UNTIL INSTRUCTED TO DO SO CHEM 111 Dr. McCorkle Exam #3A KEY While you wait, please complete the following information: Name: Student ID: Turn off cellphones and stow them away. No headphones,
18.3 Electrolysis. Dr. Fred Omega Garces. Chemistry 201. Driving a non-spontaneous Oxidation-Reduction Reaction. Miramar College.
18.3 Electrolysis Driving a non-spontaneous Oxidation-Reduction Reaction Dr. Fred Omega Garces Chemistry 201 Miramar College 1 Electrolysis Voltaic Vs. Electrolytic Cells Voltaic Cell Energy is released
AP 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
Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions.
Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions. In electrochemical reactions, electrons are transferred from one species to another. Learning goals and
Review: Balancing Redox Reactions. Review: Balancing Redox Reactions
Review: Balancing Redox Reactions Determine which species is oxidized and which species is reduced Oxidation corresponds to an increase in the oxidation number of an element Reduction corresponds to a
a. Write the balanced equation for the reaction that occurs in this cell.
EXAM 3 PRACTICE Leaders: Deborah Course: CHEM 178 Instructor: Miller Date: 1. A voltaic cell is formed at room temperature (25 C) by a silver strip immersed into an aqueous 1.0 M Ag + solution (E o red
Ch 11 Practice Problems
Ch 11 Practice Problems 1. How many electrons are transferred in the following reaction? 2Cr 2O 7 2- + 14H + + 6Cl 2Cr 3+ + 3Cl 2 + 7H 2O A) 2 B) 4 C) 6 D) 8 2. Which metal, Al or Ni, could reduce Zn 2+
CHAPTER 17 ELECTROCHEMISTRY
Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 17 ELECTROCHEMISTRY Day Plans for the day Assignment(s) for the day 17.1 Galvanic Cells Assignment
Name (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
CH 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
1022_3rd Exam_
1022_3rd Exam_1030521 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) For the following example, identify the following. H2O(l) H2O(g) A) a negative
Electrochemistry. The study of the interchange of chemical and electrical energy.
Electrochemistry The study of the interchange of chemical and electrical energy. Oxidation-reduction (redox) reaction: involves a transfer of electrons from the reducing agent to the oxidizing agent. oxidation:
Chemistry 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
40S 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
40S 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 MID-TERM EXAM TO BE BETTER PREPARED. To prepare
Assigning Oxidation Numbers
RULES Assigning Oxidation Numbers Examples 1. Each Uncombined Element has an 2Na + Cl 2 2NaCl oxidation number = 0 Na = 0 or written Na 0 Cl 2 = 0 or written Cl 0 Monatomic ions have an oxidation number
Study Guide for Module 17 Oxidation-Reduction Reactions and Electrochemistry
Chemistry 1020, Module 17 Name Study Guide for Module 17 Oxidation-Reduction Reactions and Electrochemistry Reading Assignment: Chapter 17 in Chemistry, 6th Edition by Zumdahl. Guide for Your Lecturer:
CHAPTER 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
Chemistry 102 Spring 2017 Discussion #13, Chapter 17 Student name TA name Section. Things you should know when you leave Discussion today: ( G o f
Chemistry 0 Spring 07 Discussion #3, Chapter 7 Student name TA name Section Things you should know when you leave Discussion today:. ΔSsys = ΔrS = Σ [ni (S )]product - Σ [nj (S )]reactants. ΔGº = -T ΔSnet
Electrochemistry. Chapter 18. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Electrochemistry Chapter 18 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Electrochemical processes are oxidation-reduction reactions in which: the energy
Name (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
Electrochemistry. 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
Chapter 19: Oxidation - Reduction Reactions
Chapter 19: Oxidation - Reduction Reactions 19-1 Oxidation and Reduction I. Oxidation States A. The oxidation rules (as summarized by Mr. Allan) 1. In compounds, hydrogen has an oxidation # of +1. In compounds,
Electrochemistry. To use principles of electrochemistry to understand the properties of electrochemical cells and electrolysis.
Electrochemistry Objectives: To use principles of electrochemistry to understand the properties of electrochemical cells and electrolysis. Background: Part I: Galvanic Cells: A Galvanic cell is a device
CHEMISTRY 102 FALL 2003 FINAL EXAM FORM C S DR. KEENEY-KENNICUTT PART 1
NAME CHEMISTRY 102 FALL 2003 FINAL EXAM FORM C S 515-524 DR. KEENEY-KENNICUTT Directions: (1) Put your name and signature on the free response part of the exam where indicated. (2) Choose the best answer
17.1 Redox Chemistry Revisited
Chapter Outline 17.1 Redox Chemistry Revisited 17.2 Electrochemical Cells 17.3 Standard Potentials 17.4 Chemical Energy and Electrical Work 17.5 A Reference Point: The Standard Hydrogen Electrode 17.6
ph = pk a + log 10{[base]/[acid]}
![ph = pk a + log 10{[base]/[acid]}](/thumbs/90/103664826.jpg "ph = 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
Chapter 18. Electrochemistry
Chapter 18 Electrochemistry Section 17.1 Spontaneous Processes and Entropy Section 17.1 http://www.bozemanscience.com/ap-chemistry/ Spontaneous Processes and Entropy Section 17.1 Spontaneous Processes
Wksht 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
Oxidation refers to any process in which the oxidation number of an atom becomes more positive
Lecture Notes 3 rd Series: Electrochemistry Oxidation number or states When atoms gain or lose electrons they are said to change their oxidation number or oxidation state. If an element has gained electrons
Chemistry 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
Electrochemistry. Galvanic Cell. Page 1. Applications of Redox
Electrochemistry Applications of Redox Review Oxidation reduction reactions involve a transfer of electrons. OIL- RIG Oxidation Involves Loss Reduction Involves Gain LEO-GER Lose Electrons Oxidation Gain
CHEMISTRY 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
Chapter 20 Electrochemistry
Chapter 20 Electrochemistry Learning goals and key skills: Identify oxidation, reduction, oxidizing agent, and reducing agent in a chemical equation Complete and balance redox equations using the method
CHEM 116 Electrochemical Cells
CHEM 116 Electrochemical Cells Lecture 22 Prof. Sevian Today s agenda Big picture of electrochemistry Redox reactions and oxidation numbers (last lecture) Charge flow in electrochemical cells and diagramming
Chapter Electrical work is given by a. w elec = Qε b. w elec = -QΔε c. w elec = -Q/Δε d. w elec = -Δε/Q e. none of these Answer: b
Exam 4 practice test, Fall 2005, Williams, 12/9, chapter 14 questions added. 12/12, some comments and revisions to chapter 14 questions. 12/14 some more comments and revisions, to chapter 13 questions.
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.
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
Electrochem: It s Got Potential!
Electrochem: It s Got Potential! Presented by: Denise DeMartino Westlake High School, Eanes ISD Pre-AP, AP, and Advanced Placement are registered trademarks of the College Board, which was not involved
CHEM 112 Final Exam (New Material) Practice Test Solutions
CHEM 112 Final Exam (New Material) Practice Test Solutions 1D Another electrolysis problem. This time we re solving for mass, which almost always means solving for number of moles and then converting to
Electrochemistry. Electrochemistry. Preliminary Concepts. More Preliminary Concepts. Daniell Cell. Electrochemical Cells
Electrochemistry Electrochemistry CHEM 102 T. Hughbanks Applications: Batteries Corrosion Industrial production of chemicals such as Cl 2, NaOH, F 2 and Al Biological electron transfer reactions Preliminary
8. Relax and do well.
CHEM 1515 Exam II John II. Gelder October 14, 1993 Name TA's Name Lab Section INSTRUCTIONS: 1. This examination consists of a total of 8 different pages. The last two pages include a periodic table, a
Chapter 20. Electrochemistry
Chapter 20. Electrochemistry 20.1 Oxidation-Reduction Reactions Oxidation-reduction reactions = chemical reactions in which the oxidation state of one or more substance changes (redox reactions). Recall:
Part One: Introduction. a. Chemical reactions produced by electric current. (electrolysis)
CHAPTER 19: ELECTROCHEMISTRY Part One: Introduction A. Terminology. 1. Electrochemistry deals with: a. Chemical reactions produced by electric current. (electrolysis) b. Production of electric current
Electrochemistry objectives
Electrochemistry objectives 1) Understand how a voltaic and electrolytic cell work 2) Be able to tell which substance is being oxidized and reduced and where it is occuring the anode or cathode 3) Students
Electrochemical Cells
CH302 LaBrake and Vanden Bout Electrochemical Cells Experimental Observations of Electrochemical Cells 1. Consider the voltaic cell that contains standard Co 2+ /Co and Au 3+ /Au electrodes. The following