Provide oxidation numbers to complete the following table. Species Cu Zn ion Zinc ion Sulfate ion. Oxidation # S=
|
|
- Pearl Sharp
- 5 years ago
- Views:
Transcription
1 Name (Attach data copies) Section A Describe your observations of any reactions between zinc and cupric sulfate or between copper and zinc sulfate. Write half-reactions describing any chemical changes you observed. Label the half reactions as oxidation or reduction. Indicate which species is the oxidizing agent and which is the reducing agent. Do you think this reaction has a large or small equilibrium constant? Describe the surface of the copper metal in contact with the zinc solution. Does the reaction of copper metal with zinc ion to produce copper (II) ion and zinc have a large or small equilibrium constant? Explain. Provide oxidation numbers to complete the following table. copper(ii) Species Zn ion Zinc ion Sulfate ion Oxidation # S= O= 1
2 Section B Position of red (+) Zn Position of black (- ) Zn Voltage reading (including sign) Calculate the standard oxidation potential (E o ox)for the oxidation of zinc. Calculate the equilibrium constant for the spontaneous redox reaction between cupric ion and zinc. Section C Position of red (+) Ag Position of black (-) Voltage (V) (including sign) E o oxid (V) E o red (V) 2
3 Arrange your calculated standard reduction potentials and corresponding half-reactions in order, starting with the most negative at the top of the table and ending with the most positive at the bottom. Include the standard reduction potential provided for. E (V) Half Reaction Compare the standard reduction potentials for and Ag provided in your lab manual to the ones you experimentally determined. Suggest relatively common materials that could be used to make a battery that will produce an approximate voltage of 1 V. Why are there difficulties in making the voltage measurements with magnesium and aluminum metals? Is the multimeter an effective tool in determining standard reduction potentials? Refer to your specific results as support your answer. 3
4 Section D How did you clean your nickel? What did you observe when the reaction ran for three seconds? What did you observe when dimethylglyoxime was added to the paper? Interpret this result. Which metal is the cathode and which is the anode in this experiment? Write the two half reactions and the chemical equation. Do you think that this electrolysis could be carried out with a standard 1.5 V battery? Whose picture is on the nickel? Section E Part 1. Attach graph of solution voltage vs. number of drops of Ce 4+. Perform a geometric construct on the graph to determine the number of drops to reach the equivalence point. Now utilize the number of drops from the graph and calculate the molarity of the Fe 2+ solution you titrated. Describe the endpoint of the titration (# drops added and color observed). Show calculations to determine the molarity of the Fe 2+ solution you titrated. Write the Nernst equation for the nonstandard conditions in your titration (without numbers). 4
5 Part II. Attach graph of solution voltage vs. number of drops of Cr 2 O Perform a geometric construct on the graph to determine the number of drops to reach the equivalence point. Now utilize the information from the graph and calculate the molarity of the Fe 2+ solution you titrated. Describe the endpoint of the titration (# drops added and color observed). Show calculations to determine the molarity of the Fe 2+ solution you titrated. Write the Nernst equation for the nonstandard conditions in your titration (without numbers). Section F What did you observe when the leads were attached to the battery and the Pb metal? Theoretically, what would happen if the two lead strips touched when the circuit is complete? What type of cell is a lead-acid battery, voltaic or electrolytic? Explain your answer. Write the half cell reactions for all redox reactions occurring in your lead-acid battery. 5
A Study of Electrochemistry Prelab
1. What is the purpose of this experiment? A Study of Electrochemistry Prelab 2. a. Calculate the standard cell potential of a cell constructed from Mg 2+ /Mg and Ni 2+ /Ni (Table I). Which is the anode
More informationElectrochemical 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
More informationElectrochemistry and Concentration Effects on Electrode Potentials Prelab
Electrochemistry and Concentration Effects on Electrode Potentials Prelab 1. What is the purpose of this experiment? 2. a. Calculate the standard cell potential of a cell constructed from Mg 2+ /Mg and
More information12.05 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
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 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 informationPractice Exam Topic 9: Oxidation & Reduction
Name Practice Exam Topic 9: Oxidation & Reduction 1. What are the oxidation numbers of the elements in sulfuric acid, H 2 SO 4? Hydrogen Sulfur Oxygen A. +1 +6 2 B. +1 +4 2 C. +2 +1 +4 D. +2 +6 8 2. Consider
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 information#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
More informationCHAPTER 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
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 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 informationElectrochemistry. 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
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 informationEXPERIMENT 29 VOLTAIC CELLS
Introduction: EXPERIMENT 29 VOLTAIC CELLS When a strip of zinc is placed in a solution containing copper ions, a spontaneous reaction takes place. The zinc atoms lose electrons and become zinc ions. The
More informationOxidation-Reduction Review. Electrochemistry. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions. Sample Problem.
1 Electrochemistry Oxidation-Reduction Review Topics Covered Oxidation-reduction reactions Balancing oxidationreduction equations Voltaic cells Cell EMF Spontaneity of redox reactions Batteries Electrolysis
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 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 informationCHAPTER 5 REVIEW. C. CO 2 D. Fe 2 O 3. A. Fe B. CO
CHAPTER 5 REVIEW 1. The following represents the process used to produce iron from iron III oxide: Fe 2 O 3 + 3CO 2Fe + 3CO 2 What is the reducing agent in this process? A. Fe B. CO C. CO 2 D. Fe 2 O 3
More informationElectrochemical cells. Section 21.1
Electrochemical cells Section 21.1 Electrochemical processes Chemical process either release energy or absorb energy This does not have to be solely heat or light - sometimes it can be in the form of electricity
More informationName AP CHEM / / Collected Essays Chapter 17
Name AP CHEM / / Collected Essays Chapter 17 1980 - #2 M(s) + Cu 2+ (aq) M 2+ (aq) + Cu(s) For the reaction above, E = 0.740 volt at 25 C. (a) Determine the standard electrode potential for the reaction
More information8. Draw Lewis structures and determine molecular geometry based on VSEPR Theory
Chemistry Grade 12 Outcomes 1 Quantum Chemistry and Atomic Structure Unit I 1. Perform calculations on wavelength, frequency and energy. 2. Have an understanding of the electromagnetic spectrum. 3. Relate
More 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 informationExperiment 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
More informationAP Chemistry: Electrochemistry Multiple Choice Answers
AP Chemistry: Electrochemistry Multiple Choice Answers 14. Questions 14-17 The spontaneous reaction that occurs when the cell in the picture operates is as follows: 2Ag + + Cd (s) à 2 Ag (s) + Cd 2+ (A)
More informationChemistry 213. Electrochemistry
Chemistry 213 Electrochemistry Part A: Electrochemical Cells Objective Oxidation/reduction reactions find their most important use in the construction of voltaic cells (chemical batteries). In this experiment,
More informationChemistry 213. Electrochemistry I
1 Chemistry 213 Electrochemistry I Electrochemical Cells Objective Oxidation/reduction reactions find their most important use in the construction of voltaic cells (chemical batteries). In this experiment,
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 informationChapter 19: Electrochemistry
Chapter 19: Electrochemistry Overview of the Chapter review oxidation-reduction chemistry basics galvanic cells spontaneous chemical reaction generates a voltage set-up of galvanic cell & identification
More informationOxidation-Reduction (Redox) Reactions (4.4) 2) The ox. state of an element in a simple ion is the charge of the ion. Ex:
Redox reactions: Oxidation-Reduction (Redox) Reactions (4.4) Oxidation & reduction always occur simultaneously We use OXIDATION NUMBERS to keep track of electron transfers Rules for Assigning Oxidation
More informationCHEM 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
More information12-8 Taking the oxidation state of H as + 1 and that of O as - 2, the order of increasing oxidation state of the carbon atoms is
12-1 idation occurs when an atom or molecule loses electrons in the course of a reaction. Reduction occurs when an atom or molecule gains electrons in the course of a reaction. 12-4 (a) The Zn 2+ is reduced
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 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 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 information17.1 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
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 informationToday s Objectives: and an electrolytic cell. standard cell potentials. Section 14.3 (pp )
Today s Objectives: 1. Identify the similarities and differences between a voltaic cell and an electrolytic cell 2. Predict the spontaneity of REDOX reactions based on standard cell potentials. 3. Recognize
More informationLecture 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
More informationELECTROCHEMICAL 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
More informationExperiment 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
More informationIf a piece of magnesium is placed in an aqueous solution of copper (II) sulfate, the magnesium displaces the copper in a single displacement reaction.
5.3 REDOX Reactions Half-reactions from Full Redox Equations If a piece of magnesium is placed in an aqueous solution of copper (II) sulfate, the magnesium displaces the copper in a single displacement
More informationLab #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
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 informationFind the oxidation numbers of each element in a reaction and see which ones have changed.
Find the oxidation numbers of each element in a reaction and see which ones have changed. Rules for oxidation numbers: An element that is not in a compound has an oxidation number of zero (0) Group 1 Metals
More informationBubble 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.
More informationGalvanic Cells Spontaneous Electrochemistry. Electrolytic Cells Backwards Electrochemistry
Today Galvanic Cells Spontaneous Electrochemistry Electrolytic Cells Backwards Electrochemistry Balancing Redox Reactions There is a method (actually several) Learn one (4.10-4.12) Practice (worksheet)
More information1. The following reaction was studied at a certain temperature and the data below were collected. H 2 SeO 3 (aq) + 6I (aq) + 4H + (aq) Se(s) + 2I 3
1. The following reaction was studied at a certain temperature and the data below were collected. H 2 SeO 3 (aq) + 6I (aq) + 4H + (aq) Se(s) + 2I 3 (aq) + 3H2 O(l) [H 2 SeO 3 ] 0, [H + ] 0, [I ] 0, M Initial
More informationAP Chemistry Laboratory #21: Voltaic Cells. Lab day: Monday, April 21, 2014 Lab due: Wednesday, April 23, 2014
AP Chemistry Laboratory #21: Voltaic Cells Lab day: Monday, April 21, 2014 Lab due: Wednesday, April 23, 2014 Goal (list in your lab book): The goal of this lab is to determine what factors affect the
More informationIntroduction. 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
More informationElectrochemistry. Part I: Electrochemical Activity from Chemical Reactions. Part II. Electrochemical activity from cell potentials.
Electrochemistry Introduction: Redox (oxidation-reduction) reactions will be used to determine the relative electrochemical reactivity of 5 metals. In Part I of the experiment, you will determine the activity
More informationRedox and Electrochemistry
Redox and Electrochemistry 1 Electrochemistry in Action! 2 Rules for Assigning Oxidation Numbers The oxidation number of any uncombined element is 0. The oxidation number of a monatomic ion equals the
More informationInstructors 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
More informationChemistry 112 Name Exam III Form A Section November 13,
Chemistry 112 Name Exam III Form A Section November 13, 2012 email IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white
More informationElectrochemistry. Pre-Lab Assignment. Purpose. Background. Experiment 12
Experiment 12 Electrochemistry Pre-Lab Assignment Before coming to lab: Read the lab thoroughly. Answer the pre-lab questions that appear at the end of this lab exercise. The questions should be answered
More informationElectrochemistry C020. Electrochemistry is the study of the interconversion of electrical and chemical energy
Electrochemistry C020 Electrochemistry is the study of the interconversion of electrical and chemical energy Using chemistry to generate electricity involves using a Voltaic Cell or Galvanic Cell (battery)
More informationELECTROCHEMISTRY. these are systems involving oxidation or reduction there are several types METALS IN CONTACT WITH SOLUTIONS OF THEIR IONS
Electrochemistry 1 ELECTROCHEMISTRY REDOX Reduction gain of electrons Cu 2+ (aq) + 2e > Cu(s) Oxidation removal of electrons Zn(s) > Zn 2+ (aq) + 2e HALF CELLS these are systems involving oxidation or
More informationExercise 4 Oxidation-reduction (redox) reaction oxidimetry. Theoretical part
Exercise 4 Oxidation-reduction (redox) reaction oxidimetry. Theoretical part In oxidation-reduction (or redox) reactions, the key chemical event is the net movement of electrons from one reactant to the
More informationI pledge, on my honor, that I have neither given nor received inappropriate aid on this examination
Chemistry 102b General Chemistry Exam #2 Name (Printed) I pledge, on my honor, that I have neither given nor received inappropriate aid on this examination Signature Circle the section in which you are
More informationAP Questions: Electrochemistry
AP Questions: Electrochemistry I 2 + 2 S 2O 2-3 2 I - + S 4O 2-6 How many moles of I 2 was produced during the electrolysis? The hydrogen gas produced at the cathode during the electrolysis was collected
More informationA voltaic cell using the following reaction is in operation: 2 Ag + (lm) + Cd(s) 2 Ag(s) + Cd 2+ (l M)
0. Cu (s) + 2Ag + Cu 2+ + 2Ag (s) If the equilibrium constant for the reaction above is 3.7x10 15, which of the following correctly describes the standard voltage, E o and the standard free energy change,
More informationOxidation & Reduction (Redox) Notes
Oxidation & Reduction (Redox) Notes Chemical Activity (or Chemical Reactivity) is the measure of the reactivity of elements. If an element has high activity, then it means that the element is willing to
More informationReducing Agent = a substance which "gives" electrons to another substance causing that substance to be reduced; a reducing agent is itself oxidized.
Oxidation = a loss of electrons; an element which loses electrons is said to be oxidized. Reduction = a gain of electrons; an element which gains electrons is said to be reduced. Oxidizing Agent = a substance
More informationLecture 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
More informationChapter Objectives. Chapter 13 Electrochemistry. Corrosion. Chapter Objectives. Corrosion. Corrosion
Chapter Objectives Larry Brown Tom Holme Describe at least three types of corrosion and identify chemical reactions responsible for corrosion. www.cengage.com/chemistry/brown Chapter 13 Electrochemistry
More informationElectrochemistry. Chapter 19. Concept Check Concept Check Solution. Solution
Chapter 19 Electrochemistry Concept Check 19.1 If you were to construct a wet cell and decided to replace the salt bridge with a piece of copper wire, would the cell produce sustainable current? Explain
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 information5.7 Galvanic Cells. Electrochemical Gizmos
5.7 Galvanic Cells Have you ever accidentally bitten into a piece of aluminum foil? If you have silver amalgam fillings, you may have experienced a bit of a jolt (Figure 1). The aluminium, in contact with
More informationChemistry 30 Review Test 3 Redox and Electrochemistry /55
Chemistry 30 Review Test 3 Redox and Electrochemistry /55 Part I Multiple choice / Numerical Response Answer the following multiple choice questions on the scantron sheet. Answer the numerical response
More 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 informationTo determine relative oxidizing and reducing strengths of a series of metals and ions.
Redox Reactions PURPOSE To determine relative oxidizing and reducing strengths of a series of metals and ions. GOALS 1 To explore the relative oxidizing and reducing strengths of different metals. 2 To
More informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking
INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Oxidation and Reduction by Christopher Hamaker 1 Oxidation Reduction Reactions Oxidation reduction reactions are
More informationElectrochemistry 1 1
Electrochemistry 1 1 Half-Reactions 1. Balancing Oxidation Reduction Reactions in Acidic and Basic Solutions Voltaic Cells 2. Construction of Voltaic Cells 3. Notation for Voltaic Cells 4. Cell Potential
More informationElectrochemistry. 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.
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 informationChapter 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,
More information9.1 Introduction to Oxidation and Reduction
9.1 Introduction to Oxidation and Reduction 9.1.1 - Define oxidation and reduction in terms of electron loss and gain Oxidation The loss of electrons from a substance. This may happen through the gain
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 information4. cannot occur. occurring within the same system. (A) I, III (B) II, V (C) III, IV (D) IV, V (E) V, II
Practice Exercises Oxidation-Reduction Reactions and Electrochemistry 483 Multiple-Choice For the first four problems below, one or more of the following responses will apply; each response may be used
More informationIf you're told the reaction is in basic solution: Exam 3 moved to Wednesday. More of Ch 18 today. Add OH to both sides to cancel H +
Announcements Monday, May 03, 2010 Exam 3 moved to Wednesday. Balancing in basic solution 5. If you're told the reaction is in basic solution: More of Ch 18 today. Answer keys for Quiz 3 and the titration
More informationIB Topics 9 & 19 Multiple Choice Practice
IB Topics 9 & 19 Multiple Choice Practice 1. What are the oxidation states of chromium in (NH 4) 2Cr 2O 7 (s) and Cr 2O 3 (s)? 2. Which of the following is a redox reaction? 3Mg (s) + 2AlCl 3 (aq) 2Al
More informationElectrochemical 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
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 informationGeneral Chemistry I. Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University
General Chemistry I Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University Module 7: Oxidation-reduction reactions and transformation of chemical energy Oxidation-reduction reactions
More informationAP Chemistry Readiness Thermodynamics and Electrochemistry Review Page 1 of 15. AP Chemistry Review Session UCLA April 23, 2016
AP Chemistry Readiness Thermodynamics and Electrochemistry Review Page 1 of 15 AP Chemistry Review Session UCLA April 23, 2016 Michael A. Morgan Richard Erdman Larry Walker mmorgan@lausd.net xchemteach@yahoo.com
More informationChem II. Zn(s) + CuSO4(aq)
Redox Review Chem II 1. What is the sum of the oxidation numbers of the atoms in the compound CO2? A) 0 B) 2 C) 4 D) +4 2. In which substance does phosphorus have a +3 oxidation state? A) P4O10 B) PCl5
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 informationRedox and Voltaic Cells
Name: Redox and Voltaic Cells Period: 1. Which half-reaction equation represents the reduction of an iron(ii) ion? 1) Fe 2+ Fe 3+ + e 2) Fe 2+ + 2e Fe 1) 1 to +2 2) 1 to 2 3) Fe 3+ + e Fe 2+ 4) Fe Fe 2+
More informationReview. Chapter 17 Electrochemistry. Outline. Voltaic Cells. Electrochemistry. Mnemonic
Review William L Masterton Cecile N. Hurley Edward J. Neth cengage.com/chemistry/masterton Chapter 17 Electrochemistry Oxidation Loss of electrons Occurs at electrode called the anode Reduction Gain of
More informationEXPERIMENT 16 Electrochemical Cells: A Discovery Exercise 1. Introduction. Discussion
EXPERIMENT 16 Electrochemical Cells: A Discovery Exercise 1 Introduction This lab is designed for you to discover the properties of electrochemical cells. It requires little previous knowledge of electrochemical
More informationRedox and Voltaic Cells
Name: Redox and Voltaic Cells Period: 1. Which half-reaction equation represents the reduction of an iron(ii) ion? 1) Fe 2+ Fe 3+ + e 2) Fe 2+ + 2e Fe 1) 1 to +2 2) 1 to 2 3) Fe 3+ + e Fe 2+ 4) Fe Fe 2+
More informationElectrochemical Cells Homework Unit 11 - Topic 4
Electrochemical Cell Vocabulary Electrochemical Cells Homework Unit 11 - Topic 4 Electrode Anode Voltaic Cell Oxidation Electrolytic Cell Cathode Salt Bridge Reduction Half Reaction Refer to Table J: For
More informationChapter 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:
More informationHonors Chemistry Mrs. Agostine. Chapter 19: Oxidation- Reduction Reactions
Honors Chemistry Mrs. Agostine Chapter 19: Oxidation- Reduction Reactions Let s Review In chapter 4, you learned how atoms rearrange to form new substances Now, you will look at how electrons rearrange
More informationChemistry 1B Experiment 14 65
Chemistry 1B Experiment 14 65 14 Electrochemistry Introduction In this experiment you will observe some spontaneous and non-spontaneous oxidation-reduction reactions, and see how the spontaneous reactions
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
A.P. Chemistry Practice Test - Ch. 17: Electochemistry MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The gain of electrons by an element is called.
More informationELEMENTS OF ELEC TROCHEMIS TRY. A. A number of analytical techniques are based upon oxidation-reduction reactions.
Page 1 of 8 Chem 201 Winter 2006 I. Introduction ELEMENTS OF ELEC TROCHEMIS TRY A. A number of analytical techniques are based upon oxidationreduction reactions. B. Examples of these techniques would include:
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 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 information