Department of Chemistry University of Texas at Austin
|
|
- Randolf Carroll
- 5 years ago
- Views:
Transcription
1 Electrochemical Cells II Supplemetal Worksheet All the electrochemical cells o this worksheet are the same oes o the first Electrochemical Cells worksheet. To make the work o this worksheet easier, refer to the work you did o the previous Electrochemical Cells worksheet. Experimetal Observatios of Electrochemical Cells 1. Cosider the voltaic cell that cotais stadard Co 2+ /Co ad Au 3+ /Au electrodes. The followig experimetal observatios were oted: (1) Metallic gold plates out o oe electrode ad the gold io cocetratio decreases aroud that electrode, ad (2) The mass of the cobalt electrode decreases ad the cobalt (II) io cocetratio icreases aroud that electrode. a. Recall the diagram, overall balaced redox reactio, ad the stadard cell potetial for this cell? KEY <Co(s) Co 2+ (aq) Au 3+ (aq) Au(s)> E cell = E cathode - E aode = 1.50 V (-0.28 V) = 1.78 V b. What is the stadard reactio free eergy for this cell? ΔGr = -FE = - ( = kj mol rx 6 mol e ) 1 mol rx (96,485 C 1 mol e ) (1.78 J C ) = J mol rx
2 c. Calculate the equilibrium costat for the overall redox reactio of this cell at 25 C. Because we are lookig for K at 25 C, we ca use the equatio logk = E So, K = 10 E = K = = 5.14* This is a very large K, this reflects the spotaeous ature of this reactio. d. Calculate the emf at 25 C of this cell i which the cocetratio of Co 2+ ios is 0.30 mol/l ad that of the Au 3+ ios is mol/l. Here we use the Nerst Equatio. Sice we are fidig the emf at 25 C we ca use this versio of the Nerst Equatio: Ecell = E cell log Q = E cell log [Co2+ ] [Au 3+ ] 2 = 1.78 V log [0.30]3 6 [0.0010] 2 = 1.74 V e. Assume you use this cell as a battery to power oe of your electric devices that draws 1 ma of curret. If you ra the battery at a costat 1 ma for 3000 hours, how may grams of Co would be cosumed? To figure this problem out, we will do a series of coversios: curret ad time charge moles of e- moles of Co grams of Co curret ad time charge: charge = curret * time = C/s * (3000 hrs *60 mi/hr * 60 s/mi) = C charge moles of e-: C * 1 mol e 96,485 C moles of e- moles of Co: mol e- * moles of Co grams of Co: mol Co * 3.30 g Co would be cosumed = mol e- 1 mol Co 2 mol e 58.9 g Co 1 mol Co = mol Co = 3.30 g Co
3 2. Cosider the electrolysis of molte calcium chloride with iert electrodes. The followig experimetal observatios were oted: (1) Bubbles of pale gree chlorie gas are produced at oe electrode, ad (2) Silvery white molte metallic calcium is produced at the other electrode. a. Recall the diagram, overall balaced redox reactio, ad the stadard cell potetial for this cell? <Pt(s) Cl - (aq) Cl2(g) Ca 2+ (aq) Ca(s) Pt(s)> E cell = E cathode - E aode = V (1.36 V) = V b. What is the stadard reactio free eergy for this cell? ΔGr 2 mol e = -FE = - ( ) 1 mol rx (96,485 C ) ( 4.12 J ) = kj 1 mol e C mol rx c. Calculate the equilibrium costat for the overall redox reactio of this cell at 25 C. Because we are lookig for K at 25 C, we ca use the equatio logk = E So, K = 10 E = K = 10 2 ( 4.12) = 3.76* This is a very small K, this reflects the o-spotaeous ature of this reactio
4 d. How may hours are required to plate g of metallic calcium from 1.00 M CaCl2 (aq) by usig a curret of 3.00 A? To figure this problem out, we will do a series of coversios: grams of Ca moles of Ca moles of e- charge charge ad curret time grams of Ca moles of Ca: 12 g Ca * 1 mol Ca moles of Ca moles of e-: mol Ca * 40.1 g Ca 2 mol e = mol Ca 1 mol Ca moles of e- charge: mol e- * 96,485 C 1 mol e = C charge ad curret time: time = charge = C curret 3 C/s = mol e- = s * 1 hr = 5.4 hr 3600 s It would require 5.4 hours to plate g of metallic calcium from 1.00 M CaCl2 (aq) by usig a curret of 3.00 A. e. Determie the volume (i liters, at STP) of chlorie gas that ca be produced i this cell by usig a curret of 7.30 ma for 2.11 hours. To figure this problem out, we will do a series of coversios: curret ad time charge moles of e- moles of Co liters of Cl2 curret ad time charge: charge = curret * time = C/s * (2.11 hrs *60 mi/hr * 60 s/mi) = C charge moles of e-: C * 1 mol e 96,485 C = mol e- moles of e- moles of Cl2: mol e- * 1 mol Cl 2 = mol Cl2 2 mol e moles of Cl2 liters of Cl2: mol Cl2 * 22.4 L Cl 2at STP = L Cl2 = 1 mol Cl 2 at STP 6.44 ml Cl ml Cl2 would be produced
5 Short Had Notatio of Electrochemical Cells 3. Cosider the followig cell <Ni(s) Ni 2+ (aq) Ag + (aq) Ag(s)> a. Recall the diagram, overall balaced redox reactio, ad the stadard cell potetial for this cell? E cell = E cathode - E aode = 0.80 V (-0.23 V) = 1.03 V b. What is the stadard reactio free eergy for this cell? ΔGr 2 mol e = -FE = - ( ) 1 mol rx (96,485 C ) (1.03 J ) = kj 1 mol e C mol rx c. Calculate the equilibrium costat for the overall redox reactio of this cell at 25 C. Because we are lookig for K at 25 C, we ca use the equatio logk = E So, K = 10 E = K = = 7.18*10 34 This is a very large K, this reflects the spotaeous ature of this reactio.
6 d. What is the cocetratio of Ni 2+ ios if the emf at 25 C of this cell is V ad the cocetratio of Ag + ios is mol/l? Here we use the Nerst Equatio. Sice we are fidig the emf at 25 C we ca use this versio of the Nerst Equatio: Ecell = E cell log Q Ecell - E cell = log [Ni2+ ] [Ag + ] (E cell - Ecell) = log [Ni2+ ] 10 [Ag + ] (E cell Ecell) = [Ni2+ ] [Ag + ] 2 [Ni 2+ ] = [Ag + ] (E cell Ecell) = [ mol/l] (1.03V 1.1V) = 1.2 * 10-4 M e. How may hours would it take for this galvaic cell to plate g of metallic silver from 1.00 M solutios of Ni 2+ (aq) ad Ag + (aq) assumig it produces a costat curret of 2.25 A? To figure this problem out, we will do a series of coversios: grams of Ag moles of Ag moles of e- charge charge ad curret time grams of Ag moles of Ag: 30.0 g Ag * moles of Ag moles of e-: mol Ag * 1 mol Ag g Ag 1 mol e 1 mol Ca = mol Ag moles of e- charge: mol e- * 96,485 C 1 mol e = C charge ad curret time: time = charge = C curret 2.25 C/s = mol e- 1 hr = s * = 3.3 hr 3600 s It would require 3.3 hours to plate g of metallic silver from 1.00 M solutios of Ni 2+ (aq) ad Ag + (aq) assumig it produces a costat curret of 2.25 A.
7 4. Cosider the followig cell <Pt(s) Ce 3+ (aq) Ce 4+ (aq) Cu 2+ (aq) Cu(s)> a. Recall the diagram, overall balaced redox reactio, ad the stadard cell potetial for this cell? E cell = E cathode - E aode = 0.34 V (1.70 V) = V b. What is the stadard reactio free eergy for this cell? ΔGr 2 mol e = -FE = - ( ) 1 mol rx (96,485 C ) ( 1.36 J ) = kj 1 mol e C mol rx c. Calculate the equilibrium costat for the overall redox reactio of this cell at 25 C. Because we are lookig for K at 25 C, we ca use the equatio logk = E So, K = 10 E = K = 10 2 ( 1.36) = 9.47*10-47 This is a very small K, this reflects the o-spotaeous ature of this reactio
8 d. What is the cocetratio of Ce 4+ ios if the emf at 25 C of this cell is 1.20 V, the cocetratio of Cu 2+ ios is 0.60 mol/l ad the cocetratio of Ce 3+ ios is 0.30 mol/l? Here we use the Nerst Equatio. Sice we are fidig the emf at 25 C we ca use this versio of the Nerst Equatio: Ecell = E cell log Q Ecell - E cell = [Ce log 4+ ] 2 [Cu 2+ ] [Ce 3+ ] (E cell - Ecell) = log [Ce 4+ ] 2 10 [Cu 2+ ] [Ce 3+ ] (E cell Ecell) [Ce = 4+ ] 2 [Cu 2+ ] [Ce 3+ ] 2 [Ce 4+ ] 2 = [Cu 2+ ] [Ce 3+ ] 2 10 [Ce 4+ ] = [Cu 2+ ] [Ce 3+ ] 2 10 (E cell Ecell) (E cell Ecell) = [0.60 mol/l] [0.30 mol/l] ( 1.36V ( 1.20 V)) = 4.56 * 10-4 M e. Determie the mass (i grams) of metal copper that ca be produced i this cell by usig a curret of 5.0 A for 2.7 days g Cu would be produced (see problem 1e for a similar explaatio for this problem)
9 Electrochemical Cell Diagrams 5. Cosider the followig cell: a. Recall the diagram, overall balaced redox reactio, ad the stadard cell potetial for this cell? <Cu(s) Cu 2+ (aq) Z 2+ (aq) Z(s)> E cell = E cathode - E aode = V (0.34 V) = V b. What is the stadard reactio free eergy for this cell? ΔGr = -FE = kj mol rx
10 c. Calculate the equilibrium costat for the overall redox reactio of this cell at 25 C. K = 5.96*10-38 This is a very small K, this reflects the o-spotaeous ature of this reactio. d. What is the potetial for this cell if the Cu 2+ cocetratio is 5.8 x 10-3 M ad the Z 2+ cocetratio is 1.3 x 10-1 M? Here we use the Nerst Equatio to fid that E = E logq = log [Z2+ ] 2 [Cu 2+ ] = log (0.13) 2 (0.0058) = -1.14V e. Determie the mass (i grams) of zic metal that ca be produced i this cell by usig a curret of 6.0 A for 1.5 days g Z would be produced (see problem 1e for a similar explaatio for this problem)
11 6. Cosider the followig cell: a. Recall the diagram, overall balaced redox reactio, ad the stadard cell potetial for this cell? <Z(s) Z 2+ (aq) Cu 2+ (aq) Cu(s)> E cell = E cathode - E aode = 0.34 V (-0.76 V) = 1.10 V b. What is the stadard reactio free eergy for this cell? ΔGr = -FE = kj mol rx
12 c. Calculate the equilibrium costat for the overall redox reactio of this cell at 25 C. K = 1.1*10 37 This is a very large K, this reflects the spotaeous ature of this reactio. d. Calculate the emf at 25 C of this cell i which the cocetratio of Cu 2+ ios is mol/l ad that of the Z 2+ ios is mol/l. Here we use the Nerst Equatio. Sice we are fidig the emf at 25 C we ca use this versio of the Nerst Equatio: Ecell = E cell log Q = E cell log [Z2+ ] [Cu 2+ ] = 1.15 V = 1.10 V log [0.0020] 2 [0.1250] e. How may hours would it take for this galvaic cell to plate g of metallic copper from 1.00 M solutios of Cu 2+ (aq) ad Z 2+ (aq) assumig it produces a costat curret of 5.0 A? It would require 2.53 hours to plate g of metallic copper from 1.00 M solutios of Cu 2+ (aq) ad Z 2+ (aq) assumig it produces a costat curret of 5.0 A.
Electrochemical Cells II: Stoichiometry and Nernst Equation
CH302 LaBrake and Vanden Bout Electrochemical Cells II: Stoichiometry and Nernst Equation All the electrochemical cells on this worksheet are the same ones on the first Electrochemical Cells worksheet.
More informationWhat is the oxidation number of N in KNO3? Today. Review for our Quiz! K is +1, O is -2 molecule is no charge 1(+1) + 3(-2) = -5 N must be +5
Today What is the oxidatio umber of N i KNO3? Review for our Quiz! Thermo ad Electrochemistry What happes whe the coditios are ot stadard Nerst Equatio! A.!! 0! B.!! +1! C.!! -1! D.!! +3! E.!! +5 K is
More informationElectrochemical 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
More informationStandard Potentials. Redox Reaction - the basics. Ch. 14 & 16 An Introduction to Electrochemistry & Redox Titrations. Standard Electrode Potentials
Red Reactio - the basics Ch. 4 & 6 Itroductio to lectrochemistry & Red Titratios Reduced Oxidizig get Reducig get Oxidized Red reactios: ivolve trasfer of electros from oe species to aother. Oxidizig
More informationNernst Equation. Nernst Equation. Electric Work and Gibb's Free Energy. Skills to develop. Electric Work. Gibb's Free Energy
Nerst Equatio Skills to develop Eplai ad distiguish the cell potetial ad stadard cell potetial. Calculate cell potetials from kow coditios (Nerst Equatio). Calculate the equilibrium costat from cell potetials.
More informationThe Advanced Placement Examination in Chemistry. Part II - Free Response Questions & Answers 1970 to Electrochemistry
The Advaced Placemet Examiatio i Chemistry Part II - Free Respose Questios & Aswers 970 to 005 Electrochemistry Teachers may reproduce this publicatio, i whole or i part, i limited prit quatities for o-commercial,
More informationWhat Is Required? You need to find the molar concentration, c, of the ions in a solution of ammonium phosphate.
Chemistry 11 Solutios Sectio 9.2 Solutio Stoichiometry Solutios for Practice Problems Studet Editio page 417 11. Practice Problem (page 417) If 8.5 g of pure ammoium phosphate, (NH 4 ) 3 PO 4 (s), is dissolved
More informationPractice Questions for Exam 3 CH 1020 Spring 2017
Practice Questios for Exam 3 C 1020 Sprig 2017 1. Which of the followig ca be cosidered a Brøsted-Lowry base? 5. What is the p of a solutio for which [Ba(O) 2 ] = 0.015 M? 6. The figure below shows three
More informationChapter 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
More informationName ID# Section # CH 1020 EXAM 3 Spring Form A
Name ID# Sectio # CH 1020 EXAM 3 Sprig 2016 - Form A Fill i your ame, ID#, ad sectio o this test booklet. Fill i ad bubble i your ame, ID# (bubble 0 for C ), ad sectio o the scatro form. For questio #60
More informationChpt 20: Electrochemistry
Cell Potential and Free Energy When both reactants and products are in their standard states, and under constant pressure and temperature conditions where DG o = nfe o DG o is the standard free energy
More informationNarayana IIT Academy
Narayaa IIT Academy INDIA XII_IC_SPARK JEE-MAIN Date: 3-7-7 Time : 3 Hours CPT -5 Ma Marks : 36 KEY SHEET PHYSICS ) B ) C 3) A 4) C 5) B 6) A 7) A 8) C 9) D ) A ) B ) C 3) D 4) B 5) A 6) A 7) C 8) C 9)
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 informationWhat Is Given? You know the solubility of magnesium fluoride is mol/l. [Mg 2+ ] = [MgF 2 ] = mol/l
122. Magesium fluoride, MgF 2 (aq) has a molar solubility of 2.7 10 3 mol/l. Use this iformatio to determie the K sp value for the solid. You eed to calculate the K sp for magesium fluoride, MgF 2. You
More informationCHEM J-12 June 2013
CHEM1101 2013-J-12 June 2013 In concentration cells no net chemical conversion occurs, however a measurable voltage is present between the two half-cells. Explain how the voltage is produced. 2 In concentration
More informationRedox Reaction - the basics. Ch Electrochemistry. Redox Reaction - the basics. Important Redox Titrants and the Reactions
Redox Reactio the basics Ch.46 lectrochemistry ox red red ox Oxidizig Aget Reducig Aget Redox reactios: ivolve trasfer of electros from oe species to aother. Oxidizig aget (oxidat): takes electros Reducig
More informationCHEMISTRY 102 EXAM 4 FORM 4D
CHEMISTRY 102 EXAM 4 SECTIONS 529-537 Dr. Joy Heising Directions: FORM 4D April 22, 2002 1. This examination consists of two parts: 12 multiple choice questions (5 points each) in Part 1 and 3 free response
More informationCHAPTER 17: ELECTROCHEMISTRY. Big Idea 3
CHAPTER 17: ELECTROCHEMISTRY Big Idea 3 Electrochemistry Conversion of chemical to electrical energy (discharge). And its reverse (electrolysis). Both subject to entropic caution: Convert reversibly to
More information1.In which of the following is the oxidation number of the underlined element given incorrectly? oxidation number
General Chemistry II Exam 4 Practice Problems 1 1.In which of the following is the oxidation number of the underlined element given incorrectly? oxidation number a. K 2 Cr 2 O 7 +6 b. NaAl(OH) 4 +3 c.
More informationZn+2 (aq) + Cu (s) Oxidation: An atom, ion, or molecule releases electrons and is oxidized. The oxidation number of the atom oxidized increases.
Oxidation-Reduction Page 1 The transfer of an electron from one compound to another results in the oxidation of the electron donor and the reduction of the electron acceptor. Loss of electrons (oxidation)
More informationElectrochemical 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
More informationCheck Your Solution The units for amount and concentration are correct. The answer has two significant digits and seems reasonable.
Act o Your Strategy Amout i moles,, of Ca(CH 3 COO) 2 (aq): CaCH3COO 2 c V 0.40 mol/ L 0.250 L 0.10 mol Molar mass, M, of Ca(CH 3 COO) 2 (s): M 1 M 4 M 6 M 4M Ca CH COO 3 2 Ca C H O 1 40.08 g/mol 4 12.01
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam of General Chemistry :ch.18-19 Name ID MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) When the following half-reaction is balanced, the number
More information25. 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
More informationChapter 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
More informationReview: 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
More informationAnswer Key, Problem Set 9
Chemistry 122 Mines, Spring 2018 Answer Key, Problem Set 9 1. 19.44(c) (Also indicate the sign on each electrode, and show the flow of ions in the salt bridge.); 2. 19.46 (do this for all cells in 19.44);
More informationAim: What are electrochemical cells?
Aim: What are electrochemical cells? Electrochemistry Electrochemistry- involves a redox reaction and a flow of electrons TWO TYPES of ELECTROCHEMICAL CELLS 1.Voltaic (similar to a battery) 2.Electrolytic
More informationAP CHEMISTRY NOTES 12-1 ELECTROCHEMISTRY: ELECTROCHEMICAL CELLS
AP CHEMISTRY NOTES 12-1 ELECTROCHEMISTRY: ELECTROCHEMICAL CELLS Review: OXIDATION-REDUCTION REACTIONS the changes that occur when electrons are transferred between reactants (also known as a redox reaction)
More informationSample Exercise 20.2 Practice Exercise 1 with feedback
Homework Chapter 20 Due: 11:59pm on Wednesday, November 16, 2016 You will receive no credit for items you complete after the assignment is due. Grading Policy Sample Exercise 20.2 Practice Exercise 1 with
More information18.3 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
More informationSolutions to Equilibrium Practice Problems
Solutios to Equilibrium Practice Problems Chem09 Fial Booklet Problem 1. Solutio: PO 4 10 eq The expressio for K 3 5 P O 4 eq eq PO 4 10 iit 1 M I (a) Q 1 3, the reactio proceeds to the right. 5 5 P O
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 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 informationChapter 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
More informationWhat Is Required? You need to find the ph at a certain point in the titration using hypobromous acid and potassium hydroxide solutions.
104. A chemist titrated 35.00 ml of a 0.150 mol/l solutio of hypobromous acid, HBrO(aq), K a = 2.8 10 9. Calculate the resultig ph after the additio of 15.00 ml of 0.1000 mol/l sodium hydroxide solutio,
More informationGuide 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
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 informationmccord (pmccord) HW12 Electrochemistry II mccord (51520) 1
mccord (pmccord) HW12 Electrochemistry II mccord (51520) 1 This print-out should have 25 questions. Multiple-choice questions may continue on the next column or page find all choices before answering.
More informationBatteries. How does a battery (voltaic cell) work? Time Passes
Why? Batteries How does a battery (voltaic cell) work? When we use portable devices like MP3 players and cell phones we need a ready source of electricity to provide a flow of electrons. Batteries are
More informationChapter 20. Electrochemistry
Chapter 20. Electrochemistry 20.1 OxidationReduction Reactions Oxidationreduction reactions = chemical reactions in which the oxidation state of one or more substance changes (redox reactions). Recall:
More informationCHM152 Exam Pts Spring 2017 Name: Due Friday May 5 th at the beginning of class.
CHM152 Exam 4 100 Pts Spring 2017 Name: Due Friday May 5 th at the beginning of class. Show all work. You are to work alone on this exam, but may see me for questions. 1. Arrange these compounds in order
More informationDetermination of Amount of Acid by Back Titration. Experiment 4. Experiment 4
Determiatio of Amout of Acid by Back Titratio Experimet 4 Goal: Experimet 4 Determie amout of acid that ca be eutralized by a commercial atacid Method: React atacid tablet with excess stomach acid (HCl)
More informationChapter 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:
More informationElectrochemistry 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
More informationElectrolysis and Faraday's laws of Electrolysis
Electrolysis and Faraday's laws of Electrolysis Electrolysis is defined as the passage of an electric current through an electrolyte with subsequent migration of positively and negatively charged ions
More informationPractice Test Redox. Page 1
1. What is the oxidation state of nitrogen in the compound NH4Br? (1) 1 (2) +2 (3) 3 (4) +4 2. What is the oxidation number of sulfur in Na2S2O3? (1) 1 (2) +2 (3) +6 (4) +4 3. During which process does
More informationElectrochemistry Pulling the Plug on the Power Grid
Electrochemistry 18.1 Pulling the Plug on the Power Grid 18.3 Voltaic (or Galvanic) Cells: Generating Electricity from Spontaneous Chemical Reactions 18.4 Standard Electrode Potentials 18.7 Batteries:
More informationChem. 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.
More informationCHEM 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
More informationChapter 19 - Electrochemistry. the branch of chemistry that examines the transformations between chemical and electrical energy
Chapter 19 - Electrochemistry the branch of chemistry that examines the transformations between chemical and electrical energy 19.1 Redox Chemistry Revisited A Spontaneous Redox Reaction Znº(s) + Cu 2+
More informationRedox reactions & electrochemistry
Redox reactions & electrochemistry Electrochemistry Electrical energy ; Chemical energy oxidation/reduction = redox reactions Electrochemistry Zn + Cu 2+ º Zn 2+ + Cu Oxidation-reduction reactions always
More information2. Balance the following reaction. How many electrons would be transferred?
JASPERSE CHEM 210 Ch. 19 Electrochemistry PRACTICE TEST 4 VERSION 3 Ch. 20 Nuclear Chemistry 1 Formulas: E cell =E reduction + E oxidation G = nfe cell (for kj, use F = 96.5) E cell = E [0.0592/n]log Q
More informationElectrochemistry Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry
2012 Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry Electricity from Chemistry Many chemical reactions involve the transfer of electrons between atoms or ions electron transfer
More informationUnit 5. Gases (Answers)
Uit 5. Gases (Aswers) Upo successful completio of this uit, the studets should be able to: 5. Describe what is meat by gas pressure.. The ca had a small amout of water o the bottom to begi with. Upo heatig
More informationDr. Anand Gupta
By Dr Anand Gupta Mr. Mahesh Kapil Dr. Anand Gupta 09356511518 09888711209 anandu71@yahoo.com mkapil_foru@yahoo.com Electrochemistry Electrolysis Electric energy Chemical energy Galvanic cell 2 Electrochemistry
More informationChapter 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
More informationmccord (pmccord) HW11 Electrochemistry I mccord (51520) 1
mccord (pmccord) HW11 Electrochemistry I mccord (51520) 1 This print-out should have 27 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. 001
More informationElectrochem: 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
More informationChemistry 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
More informationCh 18 Electrochemistry OIL-RIG Reactions
Ch 18 Electrochemistry OIL-RIG Reactions Alessandro Volta s Invention Modified by Dr. Cheng-Yu Lai Daily Electrochemistry Appliactions Electrochemistry: The area of chemistry that examines the transformations
More informationCHEMISTRY - 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
More informationChapter 14: Chemical Equilibrium
hapter 14: hemical Equilibrium 46 hapter 14: hemical Equilibrium Sectio 14.1: Itroductio to hemical Equilibrium hemical equilibrium is the state where the cocetratios of all reactats ad products remai
More informationGeneral Chemistry Review
General Chemistry Review Helping you remember what you learned, oh, so long ago. Topics (Until we run out of time) The mole Stoichiometry Limiting Reactants Solution Chemistry Molarity Dilution Stoichiometry
More informationSCH 4U: UNIT 7 LESSONS ELECTROCHEMISTRY (Chap 5-pg & Chap 19-pg )
SCH 4U: UNIT 7 LESSONS ELECTROCHEMISTRY (Chap 5-pg 193-229 & Chap 19-pg 845-899) 1. Rationale: Oxidation & Reduction reactions occur in many chemical systems. Examples include the rusting of iron, the
More informationElectrochem 1 Electrochemistry Some Key Topics Conduction metallic electrolytic Electrolysis effect and stoichiometry Galvanic cell Electrolytic cell Electromotive Force (potential in volts) Electrode
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 informationUnit - 3 ELECTROCHEMISTRY VSA QUESTIONS (1 - MARK QUESTIONS) 3. Mention the purpose of salt-bridge placed between two half-cells of a galvanic cell?
Unit - 3 ELECTROCHEMISTRY 1. What is a galvanic cell? VSA QUESTIONS (1 - MARK QUESTIONS) 2. Give the cell representation for Daniell Cell. 3. Mention the purpose of salt-bridge placed between two half-cells
More informationPage 1 Name: 2Al 3+ (aq) + 3Mg(s) 3Mg 2+ (aq) + 2Al(s) Fe 2 O 3 + 2Al Al 2 O 3 + 2Fe
9666-1 - Page 1 Name: 1) What is the oxidation number of chromium in the chromate ion, CrO 2-4? A) +8 B) +3 C) +2 D) +6 2) What is the oxidation number of sulfur in Na 2 S 2 O 3? A) +6 B) +4 C) +2 D) -1
More informationWhat is the importance of redox reactions? Their importance lies in the fact that we can use the transfer of electrons between species to do useful
What is the importance of redox reactions? Their importance lies in the fact that we can use the transfer of electrons between species to do useful work. This is accomplished by constructing a voltaic
More informationRedox Reactions and Electrochemistry
Redox Reactions and Electrochemistry Redox Reactions and Electrochemistry Redox Reactions (19.1) Galvanic Cells (19.2) Standard Reduction Potentials (19.3) Thermodynamics of Redox Reactions (19.4) The
More informationFernando O. Raineri. Office Hours: MWF 9:30-10:30 AM Room 519 Tue. 3:00-5:00 CLC (lobby).
Fernando O. Raineri Office Hours: MWF 9:30-10:30 AM Room 519 Tue. 3:00-5:00 CLC (lobby). P1) What is the reduction potential of the hydrogen electrode g bar H O aq Pt(s) H,1 2 3 when the aqueous solution
More informationREVIEW QUESTIONS Chapter 19
Chemistry 10 ANSWER KEY REVIEW QUESTIONS Chapter 19 1. For each of the following unbalanced equations, (i) write the half-reactions for oxidation and reduction, and (ii) balance the overall equation in
More informationTypes of Cells Chemical transformations to produce electricity- Galvanic cell or Voltaic cell (battery)
Electrochemistry Some Key Topics Conduction metallic electrolytic Electrolysis effect and stoichiometry Galvanic cell Electrolytic cell Electromotive Force Electrode Potentials Gibbs Free Energy Gibbs
More informationElectrochemistry Worksheets
Electrochemistry Worksheets Donald Calbreath, Ph.D. Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) To access a customizable version of this book, as well as other interactive
More informationSOLUTIONS Homogeeous mixture: Substaces which dissolve with each other thoroughly to form a uiform mixture is called homogeeous mixture. Eg: Water + Salt. Solutios: homogeeous mixture formed with two or
More informationOxidation number. The charge the atom would have in a molecule (or an ionic compound) if electrons were completely transferred.
Oxidation number The charge the atom would have in a molecule (or an ionic compound) if electrons were completely transferred. 1. Free elements (uncombined state) have an oxidation number of zero. Na,
More informationELECTROCHEMICAL CELLS NAME ROW PD
4-26-12 NAME ROW PD (1) Which statement describes the redox reaction that occurs when an object is electroplated? The diagram below shows the electrolysis of fused KCl. A) It is spontaneous and requires
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 informationCHEM 1423 Chapter 21 Homework Questions TEXTBOOK HOMEWORK
CHEM 1423 Chapter 21 Homework Questions TEXTBOOK HOMEWORK 21.5 Consider the following balanced redox reaction: 16 H + (aq) + 2 MnO 4- (aq) + 10 Cl - (aq) 2 Mn 2+ (aq) + 5 Cl 2 (g) + 8 H 2 O(l) (a) Which
More informationCHAPTER 11. Practice Questions (a) OH (b) I. (h) NH 3 CH 3 CO 2 (j) C 6 H 5 O - (k) (CH 3 ) 3 N conjugate pair
CAPTER 11 Practice Questios 11.1 (a) O (b) I (c) NO 2 (d) 2 PO 4 (e) 2 PO 4 (f) 3 PO 4 (g) SO 4 (h) N 3 (i) C 3 CO 2 (j) C 6 5 O - (k) (C 3 ) 3 N 11.3 cojugate pair PO 3 4 (aq) C 3 COO(aq) PO 2 4 (aq)
More informationHg2 2+ (aq) + H2(g) 2 Hg(l) + 2H + (aq)
The potential difference between two electrodes in a cell is called the electromotive force, or The EMF of a voltaic cell is called the The cell voltage of a voltaic cell will be a Note: We are used to
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 informationIntroduction Oxidation/reduction reactions involve the exchange of an electron between chemical species.
Introduction Oxidation/reduction reactions involve the exchange of an electron between chemical species. The species that loses the electron is oxidized. The species that gains the electron is reduced.
More informationTopic 19 Redox 19.1 Standard Electrode Potentials. IB Chemistry T09D04
Topic 19 Redox 19.1 Standard Electrode Potentials IB Chemistry T09D04 19.1 Standard Electrode Potentials 19.1.1 Describe the standard hydrogen electrode. (2) 19.1.2 Define the term standard electrode potential,
More informationCHEMISTRY 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
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 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 informationChemistry 1011 TOPIC TEXT REFERENCE. Electrochemistry. Masterton and Hurley Chapter 18. Chemistry 1011 Slot 5 1
Chemistry 1011 TOPIC Electrochemistry TEXT REFERENCE Masterton and Hurley Chapter 18 Chemistry 1011 Slot 5 1 18.5 Electrolytic Cells YOU ARE EXPECTED TO BE ABLE TO: Construct a labelled diagram to show
More informationSection 7.4: Calculations Involving Limiting Reagents
Sectio 7.4: Calculatios Ivolvig Limitig Reagets Tutorial 1 Practice, page 33 1. Give:.3 mol ;.0 mol HNO = 3 Required: amout of water, NaCO = 3 O H Solutio: Step 1. List the give values ad the required
More informationBATTERIES AND ELECTROLYTIC CELLS. Practical Electrochemistry
BATTERIES AND ELECTROLYTIC CELLS Practical Electrochemistry How Batteries Work One of the most practical applications of spontaneous redox reactions is making batteries. In a battery, a spontaneous electron
More informationCh 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+
More informationCh : Electrochemistry and Radiochemistry AP Review Questions
Ch. 17-21: Electrochemistry and Radiochemistry AP Review Questions Radioactivity: Zone of Stability All nuclides with 84 or more protons are unstable (radioactive). Light elements like the neutron to proton
More informationElectrolysis. Electrolysis is the process of using electrical energy to break a compound apart or to reduced an metal ion to an element.
Electrolysis Electrolysis is the process of using electrical energy to break a compound apart or to reduced an metal ion to an element. Electrolysis is done in an electrolytic cell. Electrolytic cells
More informationAQA A2 CHEMISTRY TOPIC 5.3 REDOX EQUILIBRIA BOOKLET OF PAST EXAMINATION QUESTIONS
AQA A2 CHEMISTRY TOPIC 5.3 REDOX EQUILIBRIA BOOKLET OF PAST EXAMINATION QUESTIONS 1. (a) Define the term oxidising agent in terms of electrons.... 2. Use the data in the table below, where appropriate,
More informationHow many grams of AgCl will precipitate out if 0.27 mole CaCl 2 is reacted? CaCl 2 (aq) + 2 AgNO 3 (aq) 2 AgCl (s) + Ca(NO 3 ) 2 (aq)
SAT Chemistry Problem Solving Drill 12: Stoichiometry Question No. 1 of 5 How many grams of will precipitate out if 0.27 mole is reacted? (aq) + 2 AgNO 3 (aq) 2 (s) + Ca(NO 3 ) 2 (aq) Question #01 A. 77
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 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 informationChem 401 Unit 3 Exam F18 (Buffers, Titrations, Ksp, Transition Metals & Electrochemistry)
Seat #: Date: Chem 401 Unit 3 Exam F18 (Buffers, Titrations, Ksp, Transition Metals & Electrochemistry) Multiple Choice Identify the choice that best completes the statement or answers the question. (4.2pts
More informationREDOX test practice. 2 Cr(s) + 3 Sn 2+ (aq) 2 Cr 3+ (aq) + 3 Sn(s)
1. Which polyatomic ion has a charge of 3? A) chromate ion B) oxalate ion C) phosphate ion D) thiocyanate ion 2. What is the oxidation state of nitrogen in NaNO2? A) +1 B) +2 C) +3 D) +4 3. What are the
More information