# Wksht 4.2 Aqueous Equilibria II

Size: px
Start display at page:

Transcription

1 Wksht 4.2 Aqueous Equilibria II Date: 10/16/17 1. Label the type of titration each graph represents and whether their equivalence point ph values would be greater than, equal to, or less than 7. WA being titrated by SB: ph > 7 SB being titrated by SA: ph = 7 SA being titrated by SB: ph = 7 WB being titrated by SA: ph < 7 2. What is the solubility (in M; in g/ml) of Cu(OH)2 in water at 25 C? Ksp = and Cu(OH)2 = 99.4 g/mol. (Write the equilibrium equation when it s dissolved in water) 7.32 x 10-5 g/ml a. What is the ph of saturated Cu(OH)2 in water at 25 C? Ksp = ph = Find the molar solubility of Fe(OH)3 in water at 25 C. Ksp = 6.0 x x mol/l (M)

2 a. What is its solubility (in g/l) under the same conditions? (Fe(OH)3 = g/mol) 2.32 x 10-8 g/l 4. What is the Qsp and Ksp in relation to each other for each of the following conditions? i. Solution in which precipitation occurs: Qsp > Ksp ii. Saturated solution: Qsp = Ksp iii. Unsaturated solution: Qsp < Ksp b. Looking at the Ksp value for Fe(OH)3 in question 3, is Fe(OH)3 a soluble salt or a slightly soluble salt? Slightly soluble salt 5. Calculate the ph of a saturated solution of Mn(OH)2. Ksp = 4.60 x ph = 9.66 a. Is Mn(OH)2(s) more soluble, less soluble, or equally soluble in a basic solution at 25 C? Less soluble

3 Wksht 5.1 Electrochemistry I Date: 10/18/17 1. Define oxidation and reduction. Oxidation: loss of electrons; increase in positive charge Reduction: gain of electrons; decrease in positive charge 2. What are the four no-exception oxidation state rules? O for elements 1- for F 1+ for alkali metals 2+ for alkaline earth metals 3. Assign oxidation numbers to the following equation and identify the reducing and oxidizing agents. Fe2O3 (s) + 2 Al (s) 2 Fe (l) + Al2O3 (s) + heat and light Oxidizing agent: Fe2O3 (s) Reducing agent: Al (s) 4. **Correction: it s supposed to be MnO4 - not MnO 4- ** Consider the titration of an acidic solution of Na2C2O4 with KMnO4. MnO4 - is reduced to Mn 2+ and C2O4 2- is oxidized to CO2. Balance this reaction and find the final net equation. 2 MnO4 - (aq) + 16 H + (aq) + 5 C2O4 2- (aq) 2 Mn CO2 (g) + 8 H2O (l) 5. Complete and balance the following equation, and identify the oxidizing and reducing agents. As2O3 (s) + NO3 - (aq) H3AsO4 (aq) + N2O3 (aq) (acidic solution) As2O3 (s) + 2 NO3 - (aq) +2 H + (aq) + 2H2O (l) 2 H3AsO4 (aq) + N2O3 (aq) Oxidizing agent: As2O3(s) Reducing agent: NO3 - (aq)

4 Wksht 5.2 Electrochemistry II Date: 10/22/17 1. The spontaneous movement of electrons is from high potential energy to low potential energy. 2. Draw a generic voltaic cell with a NaNO3 salt bridge, being sure to label the following parts: anode, cathode, electrode where reduction occurs, electrode where oxidation occurs, direction of electron flow, and the migration of salt bridge ions (Problem 20.29) A voltaic cell is constructed. One electrode half-cell consists of a silver strip placed in a solution of AgNO3, and the other has an iron strip placed in a solution of FeCl2. The overall cell reaction is Fe (s) + 2 Ag + (aq) Fe 2+ (aq) + 2 Ag (s) a. What s being oxidized and what s being reduced? Ag + (aq) is being reduced, Fe(s) being oxidized. b. Write the half-reactions that occur in the two half-cells? Oxidation: Fe (s) Fe 2+ (aq) + 2e - Reduction: 2 Ag + (aq) + 2e - 2 Ag (s) c. Which electrode is the anode, and which is the cathode? Anode: where Fe(s) is being oxidized Cathode: where Ag + is being reduced d. Indicate the signs of the electrodes. Anode: - Cathode: + e. Do electrons flow from the silver electrode to the iron electrode or vice versa? From the iron electrode to the silver f. In which directions do the cations and anions migrate through the solution? Cations cathode Anions anode Practice: 4. Balance the following equation. S (s) + HNO3 (aq) H2SO3 (aq) + N2O (g) (acidic solution) 2 S (s) + 2 HNO3 (aq) + H2O 2 H2SO3 (aq) + N2O (g)

5 Wksht 5.3 Electrochemistry III Date: 10/25/17 **Use a table of E red values to answer questions 1 & 2** 1. Which of the following are the strongest reducing agents? a. Cl2(g) or Br2(l) Br - (aq) b. Zn 2+ (aq) or Cd 2+ (aq) Zn(s) 2. Which of the following are the strongest oxidizing agents? a. Au + (aq) or ClO3 - (aq) Au + (aq) b. H2O2(aq) or O2(g) H2O2(aq) 3. The following half reactions have standard reduction potentials given in Appendix E. Determine which combination of these half-cell reactions yields the largest positive cell potential AND which combination yields the smallest positive cell potential. What are the values of these potentials? a. Ag + (aq) + e - Ag(s) b. Cu 2+ (aq) + 2e - Cu(s) c. Ni 2+ (aq) + 2e - Ni(s) d. Cr 3+ (aq) + 3e - Cr(s) Ag + (aq) reducing and Cr(s) oxidizing would yield the largest positive cell potential. Ni 2+ (aq) reducing and Cu(s) oxidizing would yield the smallest positive cell potential. 4. Construct a voltaic cell for the following reaction: A + (aq) + B (s) A (s) + B + (aq)

6 Wksht 5.4 Electrochemistry IIII Date: 10/29/17 1. Consider the reaction: 2 Al (s) + 3 Mn 2+ (aq) 2 Al 3+ (aq) + 3 Mn (s) a. Which component is the strongest oxidizing agent? Mn 2+ (aq) b. Evaluate the reaction s E. E = V c. Is this reaction spontaneous under standard conditions? Spontaneous 2. Spontaneous reaction for this voltaic cell? Which half-cell is the anode and which is the cathode? Direction of current? Standard EMF? Spontaneous reaction: Ag + (aq) + Cu (s) Ag (s) + Cu + (aq) Anode (Cu(s) electrode): Cu (s) Cu + (aq) + e - Cathode (Ag(s) electrode): Ag + (aq) + e - Ag (s) Direction of current: from copper electrode to silver electrode E = V 3. Balance the following reaction. 2 NaBr + 1 Cl2 2 NaCl + 1 Br2 (l) a. How many moles of electrons are transferred for 5 moles of Cl2? 5 moles of electrons b. E 0 = for the reaction above. What is the strongest reducing agent? NaBr

7 Wksht 5.4(2) Electrochemistry IIII Date: 10/30/17 1. Formulate the spontaneous redox reaction that would occur between Ca 2+ (aq) and Zn 2+ (aq). Zn 2+ (aq) + Ca (s) Zn (s) + Ca 2+ (aq) a. Calculate this reaction s E. E = V b. What is the total standard EMF if three of these galvanic cells were put in a series? E tot = V c. How would we find the wattage produced by this galvanic cell series? P = current * cell potential 2. Describe the following types of batteries: primary, secondary, and fuel cell. Primary: non-rechargeable Secondary: rechargeable Fuel cells: convert combustion energy to electrical energy 3. What is the difference between a voltaic cell versus an electrolytic cell? Voltaic cells undergo spontaneous reactions; electrolytic cells undergo electrolysis, aka nonspontaneous reactions, and require energy. a. Reaction occurring in this electrolytic cell? Which electrode is the anode and which is the cathode? Direction of current? Standard EMF? 2 Cl - (aq) + 2 Na + (aq) Cl2 (g) + 2 Na (l) Anode: 2 Cl - (aq) Cl2 (g) + 2e - Cathode: 2 Na + (aq) + 2e - 2 Na (l) Direction of current: from Cl electrode to Na electrode E = V

8 Wksht 6.1(2) Chem Thermodynamics I Date: 11/6/17 1. At 25 C, ΔH is 572 kj/mol for the reaction 2 H2 + O2 2 H2O. Is this reaction likely to be spontaneous or non-spontaneous? Spontaneous 2. The enthalpy of vaporization for one mole of Ar gas at C is 6.52 kj/mol. What is the entropy change? ΔSvap = 74.7 J/K 3. The normal boiling point of methanol is 64.7 o C. Its molar enthalpy of vaporization is Hvap = 71.8 kj/mol. The molecular weight of methanol is g/mol. a. When gaseous methanol condenses at its normal boiling point, does entropy increase or decrease? Decrease b. Calculate the value of S when 33.7 g of methanol gas condenses at normal condensation point. Scondensation = J/K 4. The hypothetical substance Z has a melting point of 23 C and a boiling point of 90 C. a. For the process Z (g) Z (l) at 90 C and 1.00 atm, Ssys = J/K. What is the value of Ssurr? Ssurr = J/K b. For the process Z (s) Z (l) at 30 C and 1.00 atm, Ssurr = J/K. What is the value of Ssys? Ssys > J/K 5. (Sample Exercise 19.3) Predict whether S is positive or negative for each process, assuming each occurs at constant temperature. a. H2O (l) H2O (g) positive b. Ag + (aq) + Cl - (aq) AgCl (s) negative c. 4 Fe (s) + 3 O2 (g) 2 Fe2O3 (s) negative d. N2(g) + O2 (g) 2 NO (g) cannot determine; will be close to zero

9 Wksht 6.2 Chem Thermodynamics II Date: 11/8/17 1. a. Rank the following species from smallest to largest standard entropy at 298 K? i. Li(g) ii. Mg(g) iii. Fe(g) iv. Mn(g) Li(g) < Mg(g) < Mn(g) < Fe(g) b. Which of the following species has the largest standard entropy at 298 K? i. NH3(aq) ii. POCl3(g) iii. NH3(g) iv. POCl3(l) 2. Answer the following in terms of phase changes and moles present in reaction. a. Sreaction < 0 (generally) when (g) (l) or solution (l) or solution (s) Decrease in mols of gas b. Sreaction > 0 (generally) when (l) or soln (g) (s) (l) or soln mols of gas increases 3. Entropy increases with mass. 4. What does the S reaction look like for the balanced reaction aa + bb cc + dd? S reaction = c S (C) + d S (D) - a S (A) - b S (B) a. Calculate the standard-state entropy of the reaction and explain the sign of each value. i. 2 NO2(g) N2O4(g) S NO2 = S N2O4 =

10 S rxn = J/K (decrease in mols of gas) ii. N2(g) + O2(g) 2 NO(g) S N2 = S O2 = S NO = S rxn = J/K (decrease in mols of gas) 5. The reaction between lime and water is spontaneous at 25 C. CaO (s) + H2O (l) Ca(OH)2 (s) a. Which statement below is true? Select all that apply. i. Sreaction < 0 ii. Sreaction > 0 iii. Suniverse < 0 iv. Sreaction = - Ssurroundings v. Suniverse > 0 b. Calculate S reaction. S rxn = J/K c. What can you say about Ssurroundings for this process? Ssurroundings > J/K 6. What is the equation for G? How can you determine whether a reaction is spontaneous, nonspontaneous, or at equilibrium at a specific temperature based on its G value?

11 G = H - T S G < 0 spontaneous G = equilibrium G > 0 nonspontaneous

### Chapter 18 problems (with solutions)

Chapter 18 problems (with solutions) 1) Assign oxidation numbers for the following species (for review see section 9.4) a) H2SO3 H = +1 S = +4 O = -2 b) Ca(ClO3)2 Ca = +2 Cl = +5 O = -2 c) C2H4 C = -2

### 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.

### CHM 2046 Test #4 Review: Chapter 17 & Chapter 18

1. Which of the following is true concerning a nonspontaneous reaction? a. It s impossible for the reaction to occur b. The reaction occurs, but very slowly c. It can be made spontaneous by adding a catalyst

### a. Write the balanced equation for the reaction that occurs in this cell.

EXAM 3 PRACTICE Leaders: Deborah Course: CHEM 178 Instructor: Miller Date: 1. A voltaic cell is formed at room temperature (25 C) by a silver strip immersed into an aqueous 1.0 M Ag + solution (E o red

### Guide to Chapter 18. Electrochemistry

Guide to Chapter 18. Electrochemistry We will spend three lecture days on this chapter. During the first class meeting we will review oxidation and reduction. We will introduce balancing redox equations

### Chemistry 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

### 1022_3rd Exam_

1022_3rd Exam_1030521 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) For the following example, identify the following. H2O(l) H2O(g) A) a negative

### 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

### Name 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

### Oxidation-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

### Electrochemistry 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:

### 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 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

### Oxidation & 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

### CHEMISTRY 102 FALL 2010 FINAL EXAM FORM C Section 502 DR. KEENEY-KENNICUTT PART 1

NAME (Block Print) CHEMISTRY 102 FALL 2010 FINAL EXAM FORM C Section 502 DR. KEENEY-KENNICUTT Directions: (1) Put your name on PART 1 and your name and signature on PART 2 of the exam where indicated.

### (c) dilute solution of glucose (d) chloroform 12 Which one of the following represents the same net reaction as the electrolysis of aqueous H2SO4

1 Electrolysis is the process in which a chemical reaction takes place at the expense of (a) chemical energy (b) electrical energy (c) heat energy (d) none of these 2 Standard hydrogen electrode has an

### CHEMISTRY 13 Electrochemistry Supplementary Problems

1. When the redox equation CHEMISTRY 13 Electrochemistry Supplementary Problems MnO 4 (aq) + H + (aq) + H 3 AsO 3 (aq) Mn 2+ (aq) + H 3 AsO 4 (aq) + H 2 O(l) is properly balanced, the coefficients will

### 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

### Redox 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+

### Chemistry 112 Name Exam III Form A Section November 13,

Chemistry 112 Name Exam III Form A Section November 13, 2012 email IMPORTANT: On the scantron (answer sheet), you MUST clearly fill your name, your student number, section number, and test form (white

### Exam3Fall2009thermoelectro

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

### (for tutoring, homework help, or help with online classes)

www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. chem10b 20.4-3 In a voltaic cell electrons flow from the anode to the cathode. Value 2. chem10b 20.1-35 How many grams

### GENERAL CHEMISTRY II CHM202 Unit 4 Practice Test

GENERAL CHEMISTRY II CHM202 Unit 4 Practice Test This test is intended to help you get acquainted with the types of questions you will be asked on the Unit Test administered at the end of the unit. The

### 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

### (aq) 5VO2 + (aq) + Mn 2+ (aq) + 10H + + 4H 2 O. (aq) 5VO2 + (aq) + Mn 2+ (aq) + 2H + (aq) basic solution. MnO2 + 2H 2 O) 3H 2 O + I IO 3

Chem 1515 Section 2 Problem Set #15 Spring 1998 Name ALL work must be shown to receive full credit. Due Due in lecture at 1:30 p.m. Friday, May 1st. PS15.1. Balance the following oxidation-reduction reactions

### 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)

### 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

### CHAPTER 12. Practice exercises

CHAPTER 12 Practice exercises 12.1 2Al(s) + 3Cl 2 (g) 2AlCl 3 (aq) Aluminium is oxidised and is therefore the reducing agent. Chlorine is reduced and is therefore the oxidising agent. 12.3 First the oxidation

### CHAPTER 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

### 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

### DO NOT USE A CALCULATOR.

Practice Test 20.1 (va pg 1 of 5) This is practice - Do NOT cheat yourself of finding out what you are capable of doing. Be sure you follow the testing conditions outlined below. DO NOT USE A CALCULATOR.

### 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

### Name (Print) Section # or TA. 1. You may use a crib sheet which you prepared in your own handwriting. This may be

Name (Print) Section # or TA 1. You may use a crib sheet which you prepared in your own handwriting. This may be one 8-1/2 by 11 inch sheet of paper with handwriting only on one side. 2. You may use a

### Chapter 20. Electrochemistry

Chapter 20. Electrochemistry 20.1 Oxidation-Reduction Reactions Oxidation-reduction reactions = chemical reactions in which the oxidation state of one or more substance changes (redox reactions). Recall:

### Redox 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+

### Chapter 19 Chemical Thermodynamics

Chapter 19. Chemical Thermodynamics Sample Exercise 19.2 (p. 819) Elemental mercury is a silver liquid at room temperature. Its normal freezing point is -38.9 o C, and its molar enthalpy of fusion is H

### CHEMISTRY - CLUTCH CH.18 - ELECTROCHEMISTRY.

!! www.clutchprep.com CONCEPT: OXIDATION-REDUCTION REACTIONS Chemists use some important terminology to describe the movement of electrons. In reactions we have the movement of electrons from one reactant

### 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

### Regents review Electrochemistry(redox)

2011-2012 1. Chlorine has an oxidation state of +3 in the compound A) HClO B) HClO2 C) HClO3 D) HClO4 2. What is the oxidation number of iodine in KIO4? A) +1 B) 1 C) +7 D) 7 3. What is the oxidation number

### Practice 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

### Ch 11 Practice Problems

Ch 11 Practice Problems 1. How many electrons are transferred in the following reaction? 2Cr 2O 7 2- + 14H + + 6Cl 2Cr 3+ + 3Cl 2 + 7H 2O A) 2 B) 4 C) 6 D) 8 2. Which metal, Al or Ni, could reduce Zn 2+

### Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions.

Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions. In electrochemical reactions, electrons are transferred from one species to another. Learning goals and

### 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

### Electrochemistry. 1. For example, the reduction of cerium(iv) by iron(ii): Ce 4+ + Fe 2+ Ce 3+ + Fe 3+ a. The reduction half-reaction is given by...

Review: Electrochemistry Reduction: the gaining of electrons Oxidation: the loss of electrons Reducing agent (reductant): species that donates electrons to reduce another reagent. Oxidizing agent (oxidant):

### 22. What is the maximum concentration of carbonate ions that will precipitate BaCO 3 but not MgCO 3 from a solution that is 2.

PX312-1718 1. What is the solubility product expression for Th(IO 3 ) 4? A) K sp = [Th 4+ ][4IO 3 ] 4 B) K sp = [Th 4+ ][IO 3 ] C) K sp = [Th][IO 3 ] 4 D) K sp = [Th 4+ ][IO 3 ] 4 E) K sp = [Th 4+ ][IO

### Electrochem: It s Got Potential!

Electrochem: It s Got Potential! Presented by: Denise DeMartino Westlake High School, Eanes ISD Pre-AP, AP, and Advanced Placement are registered trademarks of the College Board, which was not involved

### Electrochemistry. 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.

### E) Buffer capacity is the amount of acid that can be added until all of the base is used up.

Chem 124 Spring 2016 Exam 3 VERSION 1 Name make sure you fill in your version number in the TN box on the side of your scantron sheet 1) Which of the following solutions is a good buffer system? A) a solution

### CH 223 Sample Exam Exam II Name: Lab Section:

Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. Which of the following equations is the solubility

### CHM 2046 Final Exam Review: Chapters 11 18

Chapter 11 1. Which of the following has the lowest boiling point? a. NH 3 b. CH 3 Cl c. NaCl d. CO 2 e. CH 3 CH 2 CH 2 CH 2 CH 3 2. Which of the following has the lowest vapor pressure? a. CH 3 F b. CH

### REDOX 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

### 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

### 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 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,

### (c) Na is deposited at the cathode (d) Na appears at the anode

year chemiry n0tes new CHAPTER 10 ELECTROCHEMISTRY MCQS Q.1 Electrolysis is the process in which a chemical reaction takes place at the expense of (a) chemical energy (b) electrical energy (c) heat energy

### 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

### Lecture Presentation. Chapter 20. Electrochemistry. James F. Kirby Quinnipiac University Hamden, CT Pearson Education

Lecture Presentation Chapter 20 James F. Kirby Quinnipiac University Hamden, CT is the study of the relationships between electricity and chemical reactions. It includes the study of both spontaneous and

### CHEMpossible. Final Exam Review

CHEMpossible Final Exam Review 1. Given the following pair of reactions and their equilibrium constants: 2NO 2 (g) 2NO (g) + O 2 (g) K c = 15.5 2NO (g) + Cl 2 (g) 2 NOCl (g) K c = 3.20 10-3 Calculate a

### 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

### 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

http://redoxanswers.weebly.com REDOX LESSON LEARNING GOALS http://redoxanswers.weebly.com Lesson 1: Introduction to Redox Relate to examples of oxidation-reduction reactions in the real-world. Understand

CHAPTER 10 ELECTROCHEMISTRY TEXT BOOK EXERCISE Q1. Multiple choice questions. (i) The cathode reaction in the electrolysis of dill. H2SO4 with Pt electrode is (a) Reduction (b) Oxidation (c) Both oxidation

### CHM152 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

### Chapter 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

### Bonus Final Exam 3. 1 Calculate the heat of reaction,δh 0 rxn, for the following reaction as written at 298 K: g 2H 2 CH 4. g CF 4.

Bonus Final Exam 3 1 Calculate the heat of reaction,δh rxn, for the following reaction as written at 298 K: CH 4 2F 2 CF 4 2H 2 substance CH 4 CF 4 ΔH f kj/mol 75 68 (A) ΔH rxn 23 kj (B) ΔH rxn 914 kj

### 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

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

### Chapter 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:

### MULTIPLE 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

### 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

### CHE 107 FINAL EXAMINATION December 10, 2012

CHE 107 FINAL EXAMINATION December 10, 2012 University of Kentucky Department of Chemistry READ THESE DIRECTIONS CAREFULLY BEFORE STARTING THE EXAMINATION! It is extremely important that you fill in the

### Oxidation-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

### AP 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)

### Unit 8 Redox 8-1. At the end of this unit, you ll be able to

8-1 Unit 8 Redox At the end of this unit, you ll be able to Define and identify oxidation reactions Define and identify reduction reactions Assign oxidation numbers to elements in a compound Write and

### Chapter 19: Oxidation - Reduction Reactions

Chapter 19: Oxidation - Reduction Reactions 19-1 Oxidation and Reduction I. Oxidation States A. The oxidation rules (as summarized by Mr. Allan) 1. In compounds, hydrogen has an oxidation # of +1. In compounds,

### CH Practice Exam #2

CH1810 - Practice Exam #2 Part I - Multiple Choice - Choose the best answer and place the letter corresponding to the answer in the space provided. 1. Consider the following reaction and its equilibrium

### Electrochemistry (Galvanic and Electrolytic Cells) Exchange of energy in chemical cells

Electrochemistry (Galvanic and Electrolytic Cells) Exchange of energy in chemical cells Oxidation loss of electrons (oxidation number increases) OIL RIG Reduction gain of electrons (oxidation number decreases)

### Answer 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);

### I 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

### Practice Packet: Oxidation Reduction. Regents Chemistry: Mrs. Mintz. Practice Packet. Chapter 14: Oxidation Reduction & Electrochemistry

Practice Packet: Oxidation Reduction Regents Chemistry: Mrs. Mintz Practice Packet Chapter 14: Oxidation Reduction & Electrochemistry 1 Assigning Oxidation Numbers Objective: How do we assign atoms the

### CHEMISTRY 1B Fall, 2015 FINAL EXAM 1 VERSION A

CHEMISTRY 1B Fall, 2015 FINAL EXAM 1 VERSION A 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

### Study Guide for Module 17 Oxidation-Reduction Reactions and Electrochemistry

Chemistry 1020, Module 17 Name Study Guide for Module 17 Oxidation-Reduction Reactions and Electrochemistry Reading Assignment: Chapter 17 in Chemistry, 6th Edition by Zumdahl. Guide for Your Lecturer:

### Chapter 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

### Introduction to electrochemistry

Introduction to electrochemistry Oxidation reduction reactions involve energy changes. Because these reactions involve electronic transfer, the net release or net absorption of energy can occur in the

### Part One: Introduction. a. Chemical reactions produced by electric current. (electrolysis)

CHAPTER 19: ELECTROCHEMISTRY Part One: Introduction A. Terminology. 1. Electrochemistry deals with: a. Chemical reactions produced by electric current. (electrolysis) b. Production of electric current

### Chem 1B, Test Review #2

1. The following kinetics data were obtained for the reaction: Expt.# 2NO(g) + Cl 2 (g) 2NOCl(g) [NO] 0 (mol/l) [Cl 2 ] 0 (mol/l) Initial Rate, (mol/l.s) 1 0.20 0.10 6.3 x 10 3 2 0.20 0.30 1.9 x 10 2 3

### Exercise 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

### 4. [7 points] Which of the following reagents would decrease the solubility of AgCl(s)? NaOH HCl NH 3 NaCN

1. [7 points] It takes 0.098 g of silver iodate, AgIO 3, to make 1.00-L of a saturated solution saturated at 25 C. What is the value of the solubility product, K sp? a. 3.5 10 4 b. 1.2 10 7 c. 9.8 10 2

### 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

### 7. Which equation represents an oxidation-reduction reaction?

1. Which polyatomic ion has a charge of 3? 1) chromate ion 2) oxalate ion 3) phosphate ion 4) thiocyanate ion 2. An oxidation-reduction reaction involves the 1) sharing of electrons 2) sharing of protons

### 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

### Homework #3 Chapter 11 Electrochemistry

Homework #3 Chapter 11 Electrochemistry Chapter 4 83. a) Oxidation ½ Reaction Fe + HCl HFeCl 4 Fe + 4HCl HFeCl 4 Fe + 4HCl HFeCl 4 + 3H + Fe + 4HCl HFeCl 4 + 3H + + 3e Reduction ½ Reaction H 2 2H + H 2

### 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

### Lecture 14. Thermodynamics of Galvanic (Voltaic) Cells.

Lecture 14 Thermodynamics of Galvanic (Voltaic) Cells. 51 52 Ballard PEM Fuel Cell. 53 Electrochemistry Alessandro Volta, 1745-1827, Italian scientist and inventor. Luigi Galvani, 1737-1798, Italian scientist

### 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+

### SCHOOL YEAR CH- 19 OXIDATION-REDUCTION REACTIONS SUBJECT: CHEMISTRY GRADE: 12

SCHOOL YEAR 2017-18 NAME: CH- 19 OXIDATION-REDUCTION REACTIONS SUBJECT: CHEMISTRY GRADE: 12 TEST A Choose the best answer from the options that follow each question. 1. During oxidation, one or more electrons

### Chem 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

### 2. Using Half Cell Potentials and Latimer Diagrams. 100 measured half cell potentials generate 10,000 full reactions

Electrochemistry 1. Balancing Redox Reactions 2. Using Half Cell Potentials and Latimer Diagrams 100 measured half cell potentials generate 10,000 full reactions 3. E as a Thermodynamic state function

### 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