LABORATORY REPORT SHEET. Name Date Sect Cell 1. Predicted potential for cell reaction (using Nernst equation)
|
|
|
- Madlyn Hudson
- 5 years ago
- Views:
Transcription
1 LABORATORY REPORT SHEET Experiment Cell 1 Cathode half-reaction Anode half-reaction Overall chemical reaction How does your experimental potential compare with the calculated value (i.e. % error)? Cell 2 Cathode half-reaction Anode half-reaction Overall chemical reaction How does your experimental potential compare with the calculated value? 127
2 Cell 3 Cathode half-reaction Anode half-reaction Overall chemical reaction How does your experimental potential compare with the calculated value? 128
3 LABORATORY REPORT SHEET Experiment Cell 4 Cathode half-reaction Anode half-reaction Overall chemical reaction How does your experimental potential compare with the calculated value? 129
4 Cell 5 List the reduction half-reaction involved in this concentration cell, along with the ε values. Write the half-reaction occurring at the cathode (include concentration): Write the half-reaction occurring at the anode(include concentration): Net chemical reaction involved in the cell(include concentrations): How does your experimental potential compare with calculated value? 130
5 LABORATORY REPORT SHEET Cell 6 List the reduction half-reaction involved in this concentration cell, along with the ε values. Write the half-reaction occurring at the cathode(include concentration): Write the half-reaction occurring at the anode(include concentration): Net chemical reaction involved in the cell(include concentrations): How does your experimental potential compare with calculated value? 131
6 Cell 7 List the reduction half-reaction involved in this concentration cell, along with the ε values. Write the half-reaction occurring at the cathode(include concentration): Write the half-reaction occurring at the anode(include concentration): Net chemical reaction involved in the cell(include concentrations): How does your experimental potential compare with calculated value? 132
7 LABORATORY REPORT SHEET Experiment Cell 8 List the reduction half-reaction involved in this cell, along with the ε values. Write the half-reaction occurring at the cathode(include concentration): Write the half-reaction occurring at the anode(include concentration): Net chemical reaction involved in the cell(include concentrations): Reduction Potential for the observed reaction Using the Nernst equation, determine the value for the K sp for AgCl How does calculated K sp value compare with the textbook value? For cell 8, suppose that your observed voltage was 10% higher than the value you actually observed. What change would that make in the calculated value of the K sp? Determine the absolute change as well as the percent (%) change. 133
8 Cell 9 List the reduction half-reaction involved in this cell, along with the ε values. Write the half-reaction occurring at the cathode: Write the half-reaction occurring at the anode: Net chemical reaction involved in the cell: Nernst equation for this electrochemical cell Using the Nernst equation, determine the free [Cu 2+ ] in solution A: Determine K form from [Cu(NH 3 ) 4 2+ ], [Cu 2+ ], and [NH 3 ]. 134
9 LABORATORY REPORT SHEET Experiment Cell 10 Describe the galvanic cell you constructed to determine the standard potential for the reaction: Zn (s) + 2 Ag + (aq) Zn2+ (aq) + 2 Ag (s) Showing your work, use your experimental data to determine the standard potential for this reaction, and compare it to the value obtained by using the table of Standard Reduction Potentials. 135
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:
#13 Electrochemical Cells
#13 Electrochemical Cells If a copper strip is placed in a solution of copper ions, one of the following reactions may occur: Cu 2+ + 2e - Cu Cu Cu 2+ + 2e - The electrical potential that would be developed
REVIEW 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
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
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)
Electrochemical Cells: Virtual Lab
Electrochemical Cells: Virtual Lab Electrochemical cells involve the transfer of electrons from one species to another. In these chemical systems, the species that loses electrons is said to be oxidized
Experiment 18: Galvanic Cells
Chem 1B Dr. White 131 Experiment 18: Galvanic Cells Objectives Introduction To construct galvanic cells To learn how reduction potentials can be used to predict the relative reactivity of metals In a redox
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
CHEM 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
Chpt 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
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
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
When Done Test. Pg. 324 #1-9 Pg. 325 #1-5 Pg. 325 #1-4
When Done Test Pg. 324 #1-9 Pg. 325 #1-5 Pg. 325 #1-4 The Nature of Oxidation- Reduction Reactions I will be able to explain how oxidation and reduction reactions involve the transfer of electrons. I will
ELECTROCHEMICAL CELLS
ELECTROCHEMICAL CELLS Electrochemistry 1. Redox reactions involve the transfer of electrons from one reactant to another 2. Electric current is a flow of electrons in a circuit Many reduction-oxidation
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
Electrode Potentials and Their Measurement
Electrochemistry Electrode Potentials and Their Measurement Cu(s) + 2Ag + (aq) Cu(s) + Zn 2+ (aq) Cu 2+ (aq) + 2 Ag(s) No reaction Zn(s) + Cu 2+ (aq) Cu(s) + Zn 2+ (aq) In this reaction: Zn (s) g Zn 2+
Chemistry 212 Lab, Spring Design of the Experiment: Standard and Non-Standard Reduction Potentials For Metal/Metal Ion Half-Cells
Chemistry 212 Lab, Spring 2009 Electrochemical Cells: Determination of Reduction Potentials for a Series of Metal/Metal Ion Systems, Verification of Nernst Equation, and Determination of Formation Constant
What is a Voltaic Cell? Voltaic Cells a.k.a. Electrochemical cells. May 25, Voltaic Cells 2018.notebook
What is a? s a.k.a. Electrochemical cells Aim: To analyze the process of a spontaneous chemical reaction that produces electricity. Voltaic cell: an electrochemical cell where chemical energy is spontaneously
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
Lecture 30 Chapter 19, Sections 3-4 Galvanic Cells Electrochemical Potential
Lecture 30 Chapter 19, Sections 3-4 Galvanic Cells Electrochemical Potential Galvanic Cells Defined Standard Hydrogen Electrode Standard Reduction Potentials Redox Balancing One More Example OK, then here
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
Homework 11. Electrochemical Potential, Free Energy, and Applications
HW11 Electrochemical Poten!al, Free Energy, and Applica!ons Homework 11 Electrochemical Potential, Free Energy, and Applications Question 1 What is the E for Zn(s) Zn (aq) Ce (aq) Ce (aq) + cell + 4+ 3+
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
ELECTROCHEMISTRY Chapter 14
ELECTROCHEMISTRY Chapter 14 Basic Concepts: Overview of Electrochemical Process at Constant T, P (14-1) ΔG = ΔG o + RT ln Q = w elec (maximum) = qe = ItE (exp) (E intensive parameter, q extensive) = nfe
CHEMISTRY 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
mccord (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
Lecture 27 Chapter 19, Sections 3-4 Galvanic Cells Electrochemical Potential
Lecture 27 Chapter 19, Sections 3-4 Galvanic Cells Electrochemical Potential Galvanic Cells Defined Standard Hydrogen Electrode Standard Reduction Potentials Redox Balancing One More Example This time
Standard reduction potentials are established by comparison to the potential of which half reaction?
HW10 Electrochemical Poten al, Free Energy, and Applica ons This is a preview of the draft version of the quiz Started: Nov 8 at 5:51pm Quiz Instruc ons Question 1 What is the E for cell + 4+ 3+ Zn(s)
1. What do a chemical indicator and a buffer solution typically both contain?
Acids, Bases & Redox 2 - Practice Problems for Assignment 9 1. What do a chemical indicator and a buffer solution typically both contain? (a) A strong acid and its conjugate acid (b) A strong acid and
CHEM N-12 November In the electrolytic production of Al, what mass of Al can be deposited in 2.00 hours by a current of 1.8 A?
CHEM161 014-N-1 November 014 In the electrolytic production of Al, what mass of Al can be deposited in.00 hours by a current of 1.8 A? What products would you expect at the anode and the cathode on electrolysis
Copyright 2018 Dan Dill 1
when the ions each are 1 M, Zn is consumed. This means 1. 1 2. 1 3. 1 4. 1. More information needed Lecture 24 CH102 A1 (MWF 9:0 am) Monday, March 26, 2018 Cell voltage,, and electrical energy Calculating
CHEMISTRY 1B Fall, 2015 EXAM 3 VERSION A KEY
CHEMISTR 1B Fall, 2015 EAM 3 VERSION A KE Use Scantron Form SC982 E and select the letter corresponding to the correct answer. Make sure to put your full name, lab section number, and exam version (under
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)
Lab #14: Electrochemical Cells
Lab #14: Electrochemical Cells Objectives: 1. To understand the nature of electrochemical cells. 2. To construct a table listing the reduction potentials of a series of metal ions, in order of ease of
Electron Transfer Reactions
ELECTROCHEMISTRY 1 Electron Transfer Reactions 2 Electron transfer reactions are oxidation- reduction or redox reactions. Results in the generation of an electric current (electricity) or be caused by
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
2005 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B)
2005 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B) Answer EITHER Question 2 below OR Question 3 printed on pages 8 and 9. Only one of these two questions will be graded. If you start both questions, be
Chemistry 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
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: 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
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.
Electrochemistry Virtual Activities AP Chemistry Date: Activity 1 Results for each combination Mg(NO 3 ) 2 Zn(NO 3 ) 2 Cu(NO 3 ) 2 AgNO 3
Electrochemistry Virtual Activities AP Chemistry Name: Date: Part I :Go to http://www.missgurganus.com and click on the Activity Series virtual activity link. (Full web address is http://intro.chem.okstate.edu/1515f01/laboratory/activityofmetals/home.html)
Unit 4: Electrochemistry UNIFYING ELECTROCHEMISTRY, FREE ENERGY, & EQUILIBRIUM
Unit 4: Electrochemistry UNIFYING ELECTROCHEMISTRY, FREE ENERGY, & EQUILIBRIUM Goals for Today 1. Describe fully the rela2onship between electrical poten2al (ε) and free energy ( G) ΔG = nfε 2. Describe
Chem 321 Lecture 16 - Potentiometry 10/22/13
Student Learning Objectives Chem 321 Lecture 16 - Potentiometry 10/22/13 In lab you will use an ion-selective electrode to determine the amount of fluoride in an unknown solution. In this approach, as
Introduction to Electrochemical reactions. Schweitzer
Introduction to Electrochemical reactions Schweitzer Electrochemistry Create and or store electricity chemically. Use electricity to drive a reaction that normally would not run. Plating metal onto a metal
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.
Suppose, we want to measure the standard electrode potential for zinc electrode, then we construct the cell according to the following cell diagram
Standard Electrode Potential The galvanic cell has two electrode potentials; anode potential and cathode potential When the cell potential is measured with voltmeter, it gives the difference of both potentials
CHEM 10123/10125, Exam 3
CHEM 10123/10125, Exam 3 April 4, 2012 (50 minutes) Name (please print) Please box your answers, and remember that significant figures, phases (for chemical equations), and units do count! 1. (18 points)
EXPERIMENT C4: ELECTROCHEMISTRY. Learning Outcomes. Introduction. Upon completion of this lab, the student will be able to:
1 Learning Outcomes EXPERIMENT C4: ELECTROCHEMISTRY Upon completion of this lab, the student will be able to: 1) Construct an electrochemical cell. 2) Measure the cell potential for an electrochemical
12.05 Galvanic Cells. Zn(s) + 2 Ag + (aq) Zn 2+ (aq) + 2 Ag(s) Ni(s) + Pb 2+ (aq) «Ni 2+ (aq) + Pb(s)
12.05 Galvanic Cells 1. In an operating voltaic cell, reduction occurs A) at the anode B) at the cathode C) in the salt bridge D) in the wire 2. Which process occurs in an operating voltaic cell? A) Electrical
Electrochemical Cells Worksheet
General Chemistry II Labs Worksheet 10-1 Electrochemical Cells Worksheet As you work through the steps in the lab procedures, record your experimental values and the results on this worksheet. Use the
Electrochemistry. Electrochemical Process. The Galvanic Cell or Voltaic Cell
Electrochemistry Electrochemical Process The conversion of chemical energy into electrical energy and the conversion of electrical energy into chemical energy are electrochemical process. Recall that an
Electrochemistry. Review oxidation reactions and how to assign oxidation numbers (Ch 4 Chemical Reactions).
Electrochemistry Oxidation-Reduction: Review oxidation reactions and how to assign oxidation numbers (Ch 4 Chemical Reactions). Half Reactions Method for Balancing Redox Equations: Acidic solutions: 1.
Oxidation 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,
Experiment 21. Voltaic Cells
Experiment 21 Voltaic Cells INTRODUCTION: A voltaic cell is a specially prepared system in which an oxidation-reduction reaction occurs spontaneously. The oxidation and reduction half-reactions are separated
Section 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
Electrochemistry: Voltaic Cells
Name: Band: Date: An Overview and Review Electrochemistry: Voltaic Cells Electrochemistry is the field of chemistry that focuses on reactions involving electrical energy. All electrochemical reactions
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
Chapter 22. Bulk Electrolysis: Electrogravimetry and Coulometry. Definition. Features of Bulk Electrolysis Cells
Chapter 22 Bulk Electrolysis: Electrogravimetry and Coulometry Definition Bulk Electrolysis deals with methods that involve electrolysis producing a quantitative change in oxidation state Example: In a
Practice Exam 2 for VandenBout and Laude Spring 2008
Practice Exam 2 for VandenBout and Laude Spring 2008 1. What is the concentration of hydroxide ions in a solution that contains of 0.100 M HCN(aq) and 0.200 M NaCN(aq)? A. 2.4 10 5 M B. 1.1 10 9 M C. 2.5
Oxidation Numbers, ox #
Oxidation Numbers, ox # are or numbers assigned to each or assuming that the are transferred from the electronegative element to the electronegative element. now mimic systems. ox # are written followed
8. ELECTROCHEMICAL CELLS. n Electrode Reactions and Electrode Potentials a. H 2 2H + + 2e. Cl 2 + 2e 2Cl. H 2 + Cl 2 2H + + 2Cl ; z = 2
8. ELECTROCHEMICAL CELLS n Electrode Reactions and Electrode Potentials 8.1. a. H H + + e Cl + e Cl H + Cl H + + Cl ; z = E = E RT F ln ( a H +a Cl ) b. Hg(l)+ Cl Hg Cl + e H + + e H Hg + H + + Cl Hg Cl
3. Potentials and thermodynamics
Electrochemical Energy Engineering, 2012 3. Potentials and thermodynamics Learning subject 1. Electrochemical reaction 2. Thermodynamics and potential 3. Nernst equation Learning objective 1. To set up
Ch. 13 Fundamentals of Electrochemistry
Ch. 13 Fundamentals of Electrochemistry 13.1 13-1. Basic Concepts of electrochemistry redox reaction : reactions with electron transfer oxidized : loses electrons reduced : gains electrons Fe 3+ + V 2+
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
CHEM 116-Dr. Babb s Sections Answer Key to Lecture Problem Sheet Questions for Chapters 20, 21, and 23.
CHEM 116-Dr. Babb s Sections Answer Key to Lecture Problem Sheet Questions for Chapters 20, 21, and 23. 199. First complex: Co(NH 3 ) 6 Cl 3 + 3 AgNO 3 > Co(NH 3 ) 6 +3 + 3 AgCl(s); the three Cl - are
Topic 4 Electrochem. The study of interchange energy chemical electrical
Topic 4 lectrochem The study of interchange energy chemical electrical Review of Terms Oxidation reduction (redox) reaction involves a transfer of electrons from the reducing agent to the oxidizing agent
Announcements. Comprehensive Final Exam: March 24 7:30AM - 9:30 C114 2,9,10,11,13,17,22,29,31,38,40,44,46,50,53,58,62,64,65,70, 72,73,82,85,87
Announcements Exam 3 March 17 Comprehensive Final Exam: March 24 7:30AM - 9:30 C114 Problems Chapter 21: 2,9,10,11,13,17,22,29,31,38,40,44,46,50,53,58,62,64,65,70, 72,73,82,85,87 Up to but not including
ELECTROCHEMISTRY. Oxidation/Reduction
ELECTROCHEMISTRY Electrochemistry involves the relationship between electrical energy and chemical energy. OXIDATION-REDUCTION REACTIONS SPONTANEOUS REACTIONS Examples: voltaic cells, batteries. NON-SPONTANEOUS
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
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
CHAPTER 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
CHEM 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
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
Electrochem 1 Electrochemistry Some Key Topics Conduction metallic electrolytic Electrolysis effect and stoichiometry Galvanic cell Electrolytic cell Electromotive Force (potential in volts) Electrode
AP* 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 =
Chem 4501 Introduction to Thermodynamics, 3 Credits Kinetics, and Statistical Mechanics. Fall Semester Homework Problem Set Number 12 Solutions
Chem 4501 Introduction to Thermodynamics, 3 Credits Kinetics, and Statistical Mechanics Fall Semester 017 Homework Problem Set Number 1 Solutions 1. (Based on McQuarrie and Simon, 13-1.) Write balanced
Redox 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
Chapter 20. Electrochemistry
Chapter 20. Electrochemistry Sample Exercise 20.1 (p. 845) The nickelcadmium (nicad) battery, a rechargeable dry cell used in batteryoperated devices, uses the following redox reaction to generate electricity:
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.
A + B C +D ΔG = ΔG + RTlnKp. Me n+ + ne - Me. Me n n
A + B C +D ΔG = ΔG + RTlnKp Me n+ + ne - Me K p a a Me Me n a n e 1 mol madde 6.2 x 1 23 atom elektron yükü 1.62 x 1-19 C FARADAY SABİTİ: 6.2 x 1 23 x 1.62 x 1-19 = 96485 A.sn (= coulomb) 1 Faraday 965
Q1. Why does the conductivity of a solution decrease with dilution?
Q1. Why does the conductivity of a solution decrease with dilution? A1. Conductivity of a solution is the conductance of ions present in a unit volume of the solution. On dilution the number of ions per
Chemistry Discussion #9, Chapter 16 Student name TA name Section. Things you should know when you leave Discussion today:
Chemistry 102 2016 Discussion #9, Chapter 16 Student name TA name Section Things you should know when you leave Discussion today: 1. Potential E cell at standard conditions.(all concentrations are at 1M)
Instructors Guide: Introduction to Voltaic Cells
Instructors Guide: Introduction to Voltaic Cells Standards Connections: Connections to NSTA Standards for Science Teacher Preparation C.3.a.8 Oxidation reduction chemistry. Connections to the National
Oxidation and Reduction. Oxidation and Reduction
Oxidation and Reduction ϒ When an element loses an electron, the process is called oxidation: Na(s) Na + (aq) + e - ϒ The net charge on an atom is called its oxidation state in this case, Na(s) has an
Chemistry 222 Exam 4: Chapters 11, 13, 14 Spring Points
Chemistry 222 Name Exam 4: Chapters 11, 13, 14 Spring 2014 80 Points Complete five (5) of the following problems. Each problem is worth 16 points. CLEARLY mark the problems you do not want graded. You
Introduction. can be rewritten as follows: Oxidation reaction. H2 2H + +2e. Reduction reaction: F2+2e 2F. Overall Reaction H2+F2 2H + +2F
Electrochemistry is the study of chemical processes that cause electrons to move. This movement of electrons is called electricity, which can be generated by movements of electrons from one element to
A 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,
Chem Midterm 4 May 14, 2009
Chem. 101 - Midterm 4 May 14, 009 Name 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. Only
5) do sample calculations 1) In electrogravimetry, analyte deposited as a solid ("plated") onto one of the electrodes.
Page 1 of 1 Chem 201 Lecture 8b Summer 09 Return tests Last time: 0) Intro to Electrochemistry 1) E, Galvanic cells Today: Potentiometry Lecture: GALVANIC CELLS: -spontaneous reaction is utilized. ; voltaic
Date 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
Chemistry 2000 Lecture 15: Electrochemistry
Chemistry 2000 Lecture 15: Electrochemistry Marc R. Roussel February 21, 2018 Marc R. Roussel Chemistry 2000 Lecture 15: Electrochemistry February 21, 2018 1 / 33 Electrochemical cells Electrochemical
CHEM Pharmacy Week 9: Nernst Equation. Dr. Siegbert Schmid School of Chemistry, Rm 223 Phone:
CHEM1612 - Pharmacy Week 9: Nernst Equation Dr. Siegbert Schmid School of Chemistry, Rm 223 Phone: 9351 4196 E-mail: siegbert.schmid@sydney.edu.au Unless otherwise stated, all images in this file have
Module-1: Electrode Potential And Cells 2015
Lecture-2 Standard Electrode potential Standard electrode potential is the electrode potential when the metal is in contact with a solution of its own ions of unit concentration (1M) at 298K. If the electrode
AP 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)
18.2 Voltaic Cell. Generating Voltage (Potential) Dr. Fred Omega Garces. Chemistry 201. Miramar College. 1 Voltaic Cell.
18.2 Voltaic Cell Generating Voltage (Potential) Dr. Fred Omega Garces Chemistry 201 Miramar College 1 Voltaic Cell Redox Between If Zn (s) and Cu 2+ (aq) is in the same solution, then the electrons transfer
Aim: 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
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)
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
Unit 12 Redox and Electrochemistry
Unit 12 Redox and Electrochemistry Review of Terminology for Redox Reactions OXIDATION loss of electron(s) by a species; increase in oxidation number. REDUCTION gain of electron(s); decrease in oxidation