3. Calculate the percent yield if you started with 1.56 g of copper wire and recovered 0.88 g of copper. 4. What was the color of CuO?
|
|
- Howard Adams
- 6 years ago
- Views:
Transcription
1 Quiz Study Guide CHEM 109 Copper, Titration, Kinetics, Equilibrium, Enzyme Kinetics, DNA I A. Review all prelab questions, reports and postlab questions. B. Work the sample questions. Remember that all possible types of questions may not be represented. SHOW ALL WORK! Remember to use proper s.f. and units. Chemistry of Copper Lab In general: Be able to identify the type of reaction, predict products, write correct formulas, and balance equations. You should know the colors of all the copper containing products. Review the experiment and your results. Make sure you understand each step that you performed. For example, why was reaction 1 performed in the hood? 1. Classify the reaction type and balance the following equation: Cu + O 2 CuO 2. Classify the reaction type, predict the products, balance the equation and write the net ionic equation for Cu (s) + AgNO 3 (aq) 3. Calculate the percent yield if you started with 1.56 g of copper wire and recovered 0.88 g of copper. 4. What was the color of CuO? Titration of Fake Vinegar In general: Be able to perform the four steps for the calculation of a titration. Review the experiment and your results. Know what was in the buret, what was in the titrating flask and in general how the titration was performed. 1. During a titration of a ml sample of acetic acid (CH 3COOH), the endpoint was reached after adding ml of M NaOH. A) Write a balanced equation for this titration B) How many moles of NaOH were added? C) How many moles of CH 3COOH were present in the sample? D) What was the concentration of the CH 3COOH in the sample? Kinetics: Review your experimental methods. Note that we looked at effects of reactant concentration and temperature on rate. There were some postlab questions that asked you to explain these effects based on collision theory. 1. Based on the following results for the reaction between reactants A and B: A + 2B C a) Kinetics experiment Concentration of Product C Produced at Various Times Trial Reactant 20. s 40. s 60. s 80. s 100. s A conc 1 20 mm 3.21 x x x x x mm 5.50 x x x x x 10 3 Calculate the rate of trial 1 based on the two points for 20 s and 80 s shown in the table above. b) Assuming the numerical value for the rate for trial 2 was 2.82 x 10 5, what can you say about the relationship between the rate of this reaction and the concentration of reactant A? 2. For the reaction we studied: 6H + + IO 3 + 8I 3 I 3 + 3H 2O a) Which was the species used to follow the progress of the reaction? Why? b) Using Beer s Law (A = a b c) calc. the concentration, c, (in M) for a sample reading A 353 = (a = 26,400 cm 1 M 1, b = 1.08 cm)
2 3. Given the following plot of concentration of I 3 versus reaction time, determine the rate of the reaction. 1.80E04 Production of I 3 versus Time 1.60E E04 y = 1.48E06x E06 R 2 = 9.96E E E04 [I 3 ] 8.00E E E E E Time (s) 4. What is the concentration of I, if 7.50 ml of a M solution of KI was diluted to a final volume of ml? Equilibrium: Review all the equilibria studied. Remember that heating and cooling can affect an equilibrium. Do you remember what exothermic and endothermic mean? 1. Given the following equilibrium: 2CrO 4 + 2H + Cr 2O 7 + H 2O a) Adding sulfuric acid (H 2SO 4) to the yellow chromate solution (CrO 4 ) results in a persisting orange color; explain the observed change. b) Write the equilibrium constant expression in terms of concentration of reactants and products. 2. Given the following data for the equilibrium: Fe 3+ + SCN Fe(SCN) 2+ tube A 456 [Fe(SCN) 2+ ] Total [Fe 3+ ] Free [Fe 3+ ] Free [SCN ] K eq E E E E04 NA E06 5.0E05 4.8E E04 a) Write the expression for the equilibrium constant K eq b) Find the values for the equilibrium constant for tube 2. Enzyme Kinetics Given information: A = abc b = 1.08 cm a =10,300 M 1 cm 1 (for benzoq. ) A = abc Student data for enzymatic conversion of catechol to benzoquinone by catechol oxidase. A, Absorbance values for given time Rate Tube Catechol Conc. 30 s 60 s 90 s 120 s (M/s) 1 10 mm mm E mm, no enzyme E mm, boiled enzyme E mm, with inhibitor E08 1. For the 10 mm sample, calculate the concentration of benzoquinone for each of the four time points.
3 Rate (M/s) Reaction Rate (M/s) 2. Using the 30 s and 90 s data from the 10 mm catechol assay, calculate the approximate Rate (or [benzoquinone]/ t). Express your rate in [benzoquinone]/sec. 3. Calculate the relative % activity of your boiled enzyme. 4. Explain the results of question 3 in terms of protein structure. 5(a) Determine the maximum velocity of the enzyme from the graph. (b) At what catechol concentration was halfmaximal activity obtained? Show the lines on graph that help in this determination. Enzyme Activity vs Catechol Concentration 3.50E E E E E E E E Catechol Concentration (mm) 6. Using the data from the accompanying graph, approximately how long of a boiling time was required to reduce enzyme activity to 20% of its original value? Show the lines on graph that help in this determination. 3.5E07 3.0E07 2.5E07 2.0E07 1.5E07 1.0E07 5.0E08 0.0E+00 Effect of Boiling on Enzyme Activity Time (s) DNA I 1. You should be able to draw or interpret a pedigree (family tree), especially as related to hemophilia. For example: what shape is used to represent a female? A male? A individual affected by a disease? 2. What places in a cell contain DNA? In each case, from whom is that DNA inherited? 3. What disease did Alexei of the Romanovs suffer from? What kind of protein does not function properly in individuals with this disease? 4. You should be able to determine some aspects of family relationships by comparing sets of sequences. For example, the table below contains bases from specific regions of mitochondrial DNA from Fred Genetico and four other people. Which people shown do not share the same maternal ancestor with Fred (a grandmother of Fred s)? Explain. Comparing Bases Present in Particular Locations sample location 1 location 2 location 3 location 4 location 5 Fred T C C A T person 1 T C C A T person 2 T A G T C person 3 A G G C T person 4 T C C A T
4 Selected Answers! Chemistry of Copper Lab 1. Classify the type of reaction and balance the equation: Combination or synthesis 2 Cu + O 2 2 CuO 2. Classify the reaction, predict the products, balance the equation and write the net ionic equation for Single replacement Cu (s) + 2 AgNO 3 (aq) 2 Ag + Cu(NO 3) 2 (This reaction proceeds because copper is more active than silver.) NIE Cu (s) + 2 Ag + (aq) 2 Ag + Cu Calculate the percent yield if you started with 1.56 g of copper wire and recovered 0.88 g of copper x 100% = 56.4% rounds to 56% Titration of Fake Vinegar In general: Be able to perform the four steps for the calculation of a titration. Review the experiment and your results. Know what was in the buret, what was in the titrating flask and in general how the titration was performed. 1. During a titration of a ml sample of acetic acid (CH 3COOH), the endpoint was reached after adding ml of M NaOH. a) Write a balanced equation for this titration CH 3COOH + NaOH CH 3COO Na + + H 2O Note: ratio or reactants is 1:1. b) How many moles of NaOH were added? (0.100 moles/l )( ml) ( 1 L 1000 ml c) How many moles of CH 3COOH were present in the sample? mol NaOH) ( 1 mol acid 1 mol NaOH ) = mol, rounds to mol NaOH ) = mol, rounds to mol CH3COOH d) What was the concentration of the CH 3COOH in the sample? ( mol) / L = M, rounds to M CH 3COOH Kinetics: 1. Based on the following results for the reaction between reactants A and B: A + 2B C a) Calculate the rate of trial 1 based on the two points for 20 s and 80 s shown in the table above. Rate = (1.28 x x 10 4 ) / (80 s 20 s) = 1.6 x 10 5 M/s b) Assuming the numerical value for the rate for trial 2 was 2.82 x 10 5, what can you say about the relationship between the rate of this reaction and the concentration of reactant A? The difference between trial 1 and trial 2 is the concentration of reactant A. When the concentration increased (from 20 mm to 40 mm), the rate of the reaction increased as well (from 1.6 x 10 5 M/s to 2.82 x 10 5 M/s. 2. b) Using Beer s Law (A = a b c) calc. the concen., c, (in M) for a sample reading A 353 = 0.042
5 (a = cm 1 M 1, b = 1.08 cm) A = abc so c = A/(a x b) c = 0.042/ (26,400 x 1.08) = 1.5 x 10 6 M 4. What is the concentration of I, if 7.50 ml of a M solution of KI was diluted to a final volume of ml? Use M 1V 1= M 2V 2 Show work. Answer is M Equilibrium: 1. Given the following equilibrium: 2CrO 4 + 2H + Cr 2O 7 + H 2O a) Adding sulfuric acid (H 2SO 4) to the yellow chromate solution (CrO 4 ) results in a persisting orange color; explain the observed change. H 2SO 4 H + + HSO 4 This increases the concentration of H +. The collision rate between H + and CrO 4 increases. The rate of the forward reaction increases and the reaction shifts to the right. 2. Given the following data for the equilibrium: Fe 3+ + SCN Fe(SCN) 2+ a) Write the expression for the equilibrium constant K eq K eq = [Fe(SCN) 2+ ] / ([Fe 3+ ][SCN ]) b) Find the values for the equilibrium constant for tube 2. K eq = [1.97x10 6 ] / ([4.8x10 5 ][1.98x10 4 ]) = (or 2.1x10 2 ) Enzyme Kinetics 1. For the 10 mm sample, calculate the concentration of benzoquinone for each of the four time points. For the 30 s point, c =A/(ab) = 0.172/(10,300*1.08) = 1.55E05 M For the 90 s point, c =A/(ab) = 0.564/(10,300*1.08) = 5.07E05 M 2. Using the 30 s and 90 s data from the 10 mm catechol assay, calculate the approximate Rate (or [benzoquinone]/ t). Express your rate in [benzoquinone]/sec. Rate = (5.07E05 M 1.55E05 M)/(90 s 30 s) = 3.52E05 M/60 s = 5.87E07 M/s 3. Calculate the relative % activity of your boiled enzyme. Part/whole x100% 1.31E07/7.22E07 x 100% = 18.1% 4. Explain the results of question 3 in terms of protein structure. See answers to Enz. Kinetics postlab question Using the data from the accompanying graph, approximately how long of a boiling time was required to reduce enzyme activity to 20% of its original value? Show the lines on graph that help in this determination. Take the unboiled sample activity, 2.94E07 and find 20% of that value or 5.88E08. Locate that value on the yaxis and draw a horizontal line over to the graph line, then drop a vertical line to the xaxis and read the value. Should be ~14 seconds. DNA I 1. For example, what shape is used to represent a female? Circle 2. DNA is located in the nucleus and mitochondria.
6 3. What disease did Alexei of the Romanovs suffer from? hemophilia What kind of protein does not function properly in individuals with this disease? clotting factors 4. The table below contains bases from specific regions of mitochondrial DNA from Fred Genetico and four other people. Which people shown do not share the same maternal ancestor with Fred (a grandmother of Fred s)? Explain. Comparing Bases Present in Particular Locations sample location 1 location 2 location 3 location 4 location 5 Fred T C C A T person 1 T C C A T person 2 T A G T C person 3 A G G C T person 4 T C C A T Persons 2 and 3 are not related to Fred Genetico. Their sequence differs from his at 4 locations. It would be unlikely to have mutations at so many locations in a short stretch of mitochondrial DNA over a few generations time.
+ IO 3 + 8I - 4. What is the concentration of I -, if 7.50 ml of a M solution of KI was diluted to a final volume of ml?
Study Guide SCHM 109 for Vinegar titration, Kinetics, Equilibrium, Enzyme kinetics, & DNA I A. Review all pre-lab questions, reports and post-lab questions. B. Work the sample questions. Remember that
More informationQuiz Study Guide CHEM 109
Quiz Study Guide EM 109 Rep. Organic Structures, opper, Titration, Kinetics, Equilibrium, Enzyme Kinetics, DNA I A. Review all prelab questions, reports and postlab questions. B. Work the sample questions.
More informationEXPERIMENT 23 Lab Report Guidelines
EXPERIMENT 23 Listed below are some guidelines for completing the lab report for Experiment 23: For each part, follow the procedure outlined in the lab manual. Observe all safety rules, including wearing
More informationChemistry 3202 Pre-Public Examination May 2012 Name:
Chemistry 3202 Pre-Public Examination May 2012 Name: Section A: Multiple Choice This section contains 40 multiple choice covering concepts from the entire course. Please answer all multiple choice items
More informationExploring Equilibria
Exploring Equilibria Name: Chem 112 This experiment explores a variety of equilibrium systems. A reference Table of Reactions is attached to aid in your explanations. In this qualitative lab, your observations,
More informationDETERMINATION OF K c FOR AN EQUILIBRIUM SYSTEM
DETERMINATION OF K c FOR AN EQUILIBRIUM SYSTEM 1 Purpose: To determine the equilibrium constant K c for an equilibrium system using spectrophotometry to measure the concentration of a colored complex ion.
More informationLab #12: Determination of a Chemical Equilibrium Constant
Lab #12: Determination of a Chemical Equilibrium Constant Objectives: 1. Determine the equilibrium constant of the formation of the thiocyanatoiron (III) ions. 2. Understand the application of using a
More informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemistry 11 Notes on Chemical Reactions Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred:
More informationJohn Abbott College Department of Chemistry Chemistry 202-NYB-05 Sample Final Exam
John Abbott College Department of Chemistry Chemistry 202-NYB-05 Sample Final Exam Please Note: 1. Available space for answers has been removed from some questions to conserve space. 2. The questions begin
More informationEXPERIMENT 4. Le Chatelier s Principle INTRODUCTION
EXPERIMENT 4 Le Chatelier s Principle INTRODUCTION Le Chatelier s Principle states: When a stress is applied to a chemical system at equilibrium, the equilibrium concentrations will shift in a direction
More informationCHEMICAL EQUILIBRIUM. I. Multiple Choice 15 marks. 1. Reactions that can proceed in both the forward and reverse directions are said to be:
Name: Unit Test CHEMICAL EQUILIBRIUM Date: _ 50 marks total I. Multiple Choice 15 marks 1. Reactions that can proceed in both the forward and reverse directions are said to be: A. complete B. reversible
More informationExperiment 8: DETERMINATION OF AN EQUILIBRIUM CONSTANT
Experiment 8: DETERMINATION OF AN EQUILIBRIUM CONSTANT Purpose: The equilibrium constant for the formation of iron(iii) thiocyanate complex ion is to be determined. Introduction: In the previous week,
More informationName: Chemistry 400: General Chemistry Miller Exam I September 20, 2017 Approximately 150 points
Name: Chemistry 400: General Chemistry Miller Exam I September 20, 2017 Approximately 150 points Please answer each of the following questions to the best of your ability. If you wish to receive partial
More informationFinal NYB Fall 2009 Condensed Version (Working Spaces Removed)
Please Note: 1. There was a set of 15 multiple choice questions that were present on this exam, but have not been reproduced for the practice version. It would have taken approximately 10-30 minutes to
More informationProblem Set on Tracking Reaction Progress
CHM 103 Problem Set on Tracking Reaction Progress Sinex 1. Consider the titration of a weak acid, HX, as given below. A weak acid sample of 216.1 mg was dissolved to make 15.00 ml solution. This was titrated
More informationPROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS
INSERT STUDENT I.D. NUMBER (PEN) STICKER IN THIS SPACE APRIL 1996 PROVINCIAL EXAMINATION MINISTRY OF EDUCATION CHEMISTRY 12 GENERAL INSTRUCTIONS 1. Insert the stickers with your Student I.D. Number (PEN)
More informationDate: Names: Section: To investigate various chemical equilibria and explain them using Le Chatelier s Principle. Equilibrium I
Chem 1105 EQUILIBRIUM Date: Names: Section: OBJECTIVE: PROCEDURE: To investigate various chemical equilibria and explain them using Le Chatelier s Principle. As in Chem. 1105 lab manual, pp. Equilibrium
More informationEquilibrium Multiple Choice
Equilibrium Multiple Choice January 1999 7. Consider the following graph: When equilibrium is reached, the rate of the forward reaction is A. 0.00 mol/min B. 0.25mol/min C. 1.0 mol/min D. 3.0 mol/min 8.
More informationChemistry 12 August 2002 Provincial Examination
Chemistry 12 August 2002 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationEXPERIMENT 4 THE EFFECT OF CONCENTRATION CHANGES ON EQUILIBRIUM SYSTEMS
PURPOSE In this experiment, you will look at different equilibria, observe how addition or removal of components affects those equilibria and see if the results are consistent with Le Chatelier's principle.
More informationChemistry Stoichiometry and Heat Exam (ver.1) Mr. Thaler. Please do not write on this exam. Mark your answers on the scantron only.
1. Identify from the unbalanced equations below the one that does not represent a redox reaction. a. H 2O 2(aq) + MnO 4 - (aq) O 2(g) + Mn 2+ (aq) b. H 2(g) + N 2(g) NH 3(g) c. NaCl (aq) + AgNO 3(aq) NaNO
More informationExperiment 5 Equilibrium Systems
PURPOSE In this experiment, you will look at different equilibria, observe how addition or removal of components affects those equilibria and see if the results are consistent with Le Chatelier's principle.
More informationNotes: Balancing Chemical Equations
Notes: Balancing Chemical Equations Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products are completely
More informationChemistry 12 January 2000 Provincial Examination
Chemistry 2 January 2000 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationHonors text: Ch 10 & 12 Unit 06 Notes: Balancing Chemical Equations
Notes: Balancing Chemical Equations Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products are completely
More informationCHEM 12 Unit 3 Review package (solubility)
CHEM 12 Unit 3 Review package (solubility) 1. Which of the following combinations would form an ionic solid? A. Metalloid - metal B. Metal non-metal C. Metalloid metalloid D. Non-metal non-metal 2. Which
More information2 nd Semester Study Guide 2016
Chemistry 2 nd Semester Study Guide 2016 Name: Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More information8. The table below describes two different reactions in which Reaction 1 is faster. What accounts for this observation? Reaction 1 Reaction 2.
Public Review - Rates and Equilibrium June 2005 1. What does X represent in the diagram below? (A) activation energy for the forward reaction (B) activation energy for the reverse reaction (C) heat of
More informationChemistry 12 June 2003 Provincial Examination
Chemistry 12 June 2003 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation
More informationEquilibrium Written Response
Equilibrium Written Response January 1998 2. Consider the following equilibrium: CS2 (g) + 3Cl2 (g) CCl4 (g) + S2Cl2 (g) ΔH = -238 kj a) Sketch a potential energy diagram for the reaction above and label
More information1 A. That the reaction is endothermic when proceeding in the left to right direction as written.
1 Q. If Δ r H is positive, what can you say about the reaction? 1 A. That the reaction is endothermic when proceeding in the left to right direction as written. 2 Q If Δ r H is negative, what can you say
More informationAP Chapter 15 & 16: Acid-Base Equilibria Name
AP Chapter 15 & 16: Acid-Base Equilibria Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 15 & 16: Acid-Base Equilibria 2 Warm-Ups (Show
More informationEquilibrium Written Response
Equilibrium Written Response January 1998 2. Consider the following equilibrium: CS2 (g) + 3Cl2 (g) CCl4 (g) + S2Cl2 (g) H = -238 kj a) Sketch a potential energy diagram for the reaction above and label
More informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred: Temperature change Different coloured materials
More information2 nd Semester Study Guide 2017
Chemistry 2 nd Semester Study Guide 2017 Name: KEY Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More informationShifts in Equilibrium: Le Châtelier s Principle
6 Shifts in Equilibrium: Le Châtelier s Principle Introduction Whenever a chemical reaction occurs, the reverse reaction can also occur. As the original reactants, on the left side of the equation, react
More informationFunsheet 9.1 [VSEPR] Gu 2015
Funsheet 9.1 [VSEPR] Gu 2015 Molecule Lewis Structure # Atoms Bonded to Central Atom # Lone Pairs on Central Atom Name of Shape 3D Lewis Structure NI 3 CF 4 OCl 2 C 2 F 2 HOF Funsheet 9.1 [VSEPR] Gu 2015
More informationChemistry 12 August 2008 Form A Provincial Examination Answer Key
Cognitive Processes K = Knowledge U = Understanding H = Higher Mental Processes Topics 1. Reaction Kinetics 2. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation Reduction
More informationChemistry 12. Resource Exam B. Exam Booklet
Chemistry 12 Resource Exam B Exam Booklet Contents: 21 pages Examination: 2 hours 50 multiple-choice questions in the Exam Booklet Additional Time Permitted: 60 minutes Province of British Columbia PART
More informationLab #16: Determination of the Equilibrium Name: Constant of FeSCN 2+ Lab Exercise. 10 points USE BLUE/BLACK INK!!!! Date: Hour:
Lab #16: Determination of the Equilibrium Name: Constant of FeSCN 2+ Lab Exercise Chemistry II Partner: 10 points USE BLUE/BLACK INK!!!! Date: Hour: Goal: The goal of this lab is to determine the equilibrium
More informationLe Chatelier s Principle
Le Chatelier s Principle Introduction: In this experiment you will observe shifts in equilibrium systems when conditions such as concentration and temperature are changed. You will explain the observed
More informationChemistry 12 August 2000 Provincial Examination
Chemistry August 000 Provincial Examination ANSWER KEY / SCORING GUIDE CURRICULUM: Organizers. Reaction Kinetics. Dynamic Equilibrium 3. Solubility Equilibria 4. Acids, Bases, and Salts 5. Oxidation Ð
More informationLa Châtelier s Principle Science Olympiad Edgewood Regional
La Châtelier s Principle School: I will demonstrate several reactions for you and ask questions regarding the reagents and results. REACTION 1 Tetrachlorocobaltate(II) [left] and hexaaquacobalt(ii) equilibrium
More information11 Equilibrium. S T A T I O N 1 K e q E X P R E S S I O N S S T A T I O N 2 G R A P H S. South Pasadena Honors Chemistry 11 Equilibrium Period Date
South Pasadena Honors Chemistry Name 11 Equilibrium Period Date S T A T I O N 1 K e q E X P R E S S I O N S Write the expression for the equilibrium constant for the reaction: Fe 3+ (aq) + SCN (aq) FeSCN
More informationLe Chatelier s Principle
Le Chatelier s Principle Introduction: In this experiment you will observe shifts in equilibrium systems when conditions such as concentration and temperature are changed. You will explain the observed
More informationAP Chemistry Laboratory #16: Determination of the Equilibrium Constant of FeSCN 2+
AP Chemistry Laboratory #16: Determination of the Equilibrium Constant of FeSCN 2 Lab days: Thursday and Friday, February 22-23, 2018 Lab due: Tuesday, February 27, 2018 Goal (list in your lab book): The
More informationa) This reaction is (circle one): ENDOTHERMIC/EXOTHERMIC b) provide the correct chemical names for the given chemical formulas:
1. For the following questions (a c), refer to the reaction below: Fe2O3 (s) + 2 Al (s) Al2O3 (s) + 2 Fe (s) Hrxn = 852 kj/mol a) This reaction is (circle one): ENDOTHERMIC/EXOTHERMIC b) provide the correct
More informationClass Results Simulator:
Class Results http://chemconnections.org/general/chem120/equil-graph.html Simulator: http://chemconnections.org/java/equilibrium/ http://chemconnections.org/general/chem120/equil-graph.html The changes
More informationDetermination of the Equilibrium Constant for the Iron (III) thiocynate Reaction
Lab 4. Determination of the Equilibrium Constant for the Iron (III) thiocynate Reaction Prelab Assignment Before coming to lab: After reading "Lab Notebook Policy and Format for Lab Reports" handout, complete
More informationChemistry 12 APRIL Course Code = CH. Student Instructions
MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry 12 2002 Ministry of Education APRIL 2002 Course Code
More informationTITRATIONS: USING PRECIPITATION TO DETERMINE THE CONCENTRATION OF AN ION IN SOLUTION
TITRATIONS: USING PRECIPITATION TO DETERMINE THE CONCENTRATION OF AN ION IN SOLUTION In this section, you will be shown: 1. How titrations involving precipitation reactions can be used to determine the
More informationChemical Equilibria 2
Chemical Equilibria 2 Reading: Ch 14 sections 6-9 Homework: Chapter 14: 27*, 29*, 31, 33, 41, 43, 45, 51*, 55, 61*, 63, 67*, 69* * = important homework question Review A chemical equilibrium and its respective
More informationTitration a solution of known concentration, called a standard solution
Acid-Base Titrations Titration is a form of analysis in which we measure the volume of material of known concentration sufficient to react with the substance being analyzed. Titration a solution of known
More informationChemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances
Chemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances 1. Identify each of the following as ionic or molecular substances: a) NaCl (aq)... b) CH 3 COOH (aq)... c) CCl 4(l)... d) HNO 3(aq)...
More informationCHEM Lab 7: Determination of an Equilibrium Constant using Spectroscopy
CHEM 0012 Lab 7: Determination of an Equilibrium Constant using Spectroscopy 1 Determination of the equilibrium constant of the following equilibrium system at room temperature. Fe 3+ (aq) + SCN- (aq)
More informationChemistry 12. Tutorial 12
Chemistry 12 Tutorial 12 Determining the Concentration of a Specific Ion Using Precipitation Titrations In Tutorial 12, you will be shown: 1. How titrations involving precipitation reactions can be used
More informationIf you have a Mac do whatever you have to do to play it as a slide show I don t know Macs well. Dr. Buckley
For best results please view this as a slide show. You can hit the F5 key or go to the Slide Show tab on the menu bar and click on From Beginning. Page Down and Page Up will move you through the presentation.
More informationChemical Equilibrium Practice Problems #2
Chemical Equilibrium Practice Problems #2 2-20-2015 1. A CPHS student does an equilibrium experiment with the general chemical equation and derives the 2 graphs below: A = B: a. When at equilibrium is
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationChemical Equilibrium. A state of no net change in reactant & product concentrations. There is a lot of activity at the molecular level.
Chemical Equilibrium A state of no net change in reactant & product concentrations. BUT There is a lot of activity at the molecular level. 1 Kinetics Equilibrium For an elementary step in the mechanism:
More informationExperiment 7A ANALYSIS OF BRASS
Experiment 7A ANALYSIS OF BRASS FV 10/21/10 MATERIALS: Spectronic 20 spectrophotometers, 2 cuvettes, brass sample, 7 M HNO 3, 0.100 M CuSO 4, 2 M NH 3, two 50 ml beakers, 100 ml beaker, two 25 ml volumetric
More informationChapter 4: Chemical Quantities and Aqueous Reactions
Chapter 4: Chemical Quantities and Aqueous Reactions C (s) + O 2 (g) CO 2 (g) CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 0 (g) 2 C 8 H 18 (g) + 25 O 2 (g) 16 CO 2 (g) + 18 H 2 0 (g) Stoichiometry Calculations
More informationChapter Four. Chapter Four. Chemical Reactions in Aqueous Solutions. Electrostatic Forces. Conduction Illustrated
1 Electrostatic Forces 2 Chemical Reactions in Aqueous Solutions Unlike charges (+ and ) attract one another. Like charges (+ and +, or and ) repel one another. Conduction Illustrated 3 Arrhenius s Theory
More informationLe Chatelier s Principle
Le Chatelier s Principle Introduction: In this experiment you will observe shifts in equilibrium systems when conditions such as concentration and temperature are changed. You will explain the observed
More informationChemical Equilibrium and Le Chatlier s Principle
MiraCosta College Introductory Chemistry Laboratory Chemical Equilibrium and Le Chatlier s Principle EXPERIMENTAL TASK Examine a number of chemical reaction systems at equilibrium, predict the shifts they
More informationName. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
More informationph Measurement and its Applications
ph Measurement and its Applications Objectives: To measure the ph of various solutions using indicators and ph meters. To perform a ph titration. To create and study buffer solutions. To determine the
More informationCH 101 Fall 2018 Discussion #8 Chapter 6 Your name: TF s name: Discussion Day/Time: Things you should know when you leave Discussion today:
CH 101 Fall 2018 Discussion #8 Chapter 6 Your name: TF s name: Discussion Day/Time: Things you should know when you leave Discussion today: Precipitation Reaction & Solubility Solubility of Ionic compounds
More informationChem 400 Basics What You Need to Know Before Coming to Class
Chem 400 Basics What You Need to Know Before Coming to Class A C grade or better in Chem 305, Chem 310, or high school chemistry is a prerequisite for this class. You are therefore expected to know, or
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationc. K 2 CO 3 d. (NH 4 ) 2 SO 4 Answer c
Chem 130 Name Exam 2, Ch 4-6 July 7, 2016 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units and
More information2] What is the difference between the end point and equivalence point for a monobasicmonoacid
4 Titrations modified October 9, 2013 1] A solution of 0.100 M AgNO 3 is used to titrate a 100.00 ml solution of 0.100 M KCl. The K sp of AgCl is 1.8e-11 a) What is pag if 50.00 ml of the titrant is added
More informationChapter 6 and 7 Study Guide Reactions and Bonds
Name_ Per. Block _ Multiple Choice: Chapter 6 and 7 Study Guide Reactions and Bonds 1. Copper is a good conductor of electricity because its electrons A. are positively charged B. are free to move and
More informationChemistry. Approximate Timeline. Students are expected to keep up with class work when absent.
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 15 SOLUTIONS Day Plans for the day Assignment(s) for the day 1 Begin Chapter 15
More informationDETERMINATION OF AN EQUILIBRIUM CONSTANT
DETERMINATION OF AN EQUILIBRIUM CONSTANT In this experiment the equilibrium properties of the reaction between the iron(iii) ion and the thiocyanate ion will be studied. The relevant chemical equation
More informationUNIT II - REVIEW EQUILIBRIA. Part I - Multiple Choice. 1. In which of the following does the entropy decrease?
CHEMISTRY 12 UNIT II - REVIEW EQUILIBRIA Part I - Multiple Choice 1. In which of the following does the entropy decrease? A. NaCl (s) Na + (aq) + Cl (aq) B. 4 NO (g) + 6 H 2 O (g) 4 NH 3 (g) + 5 O 2 (g)
More informationExperiment 4, Calculation of Molarity of H 3 PO 4 by Titration with NaOH Chemistry 201, Wright College, Department of Physical Science and Engineering
Name Date Experiment 4, Calculation of Molarity of H 3 PO 4 by Titration with NaOH Chemistry 201, Wright College, Department of Physical Science and Engineering Molarity is a common unit within the chemical
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationClassify each compound as Ionic (I), Covalent (C), or Acid (A). Write the names or formulas for each compound. Name Type Formula Name Type Formula
South Pasadena Chemistry Name Period Date U N I T 6 C O M P O U N D S Consider the compound Ba(NO 3) 2. Classify: [ Ionic Covalent Acid Organic ] Name the compound: Calculate the Molar Mass. Consider the
More informationRate of Reaction. Introduction
5 Rate of Reaction Introduction This experiment will allow you to study the effects of concentration, temperature, and catalysts on a reaction rate. The reaction whose rate you will study is the oxidation
More informationExperiment 7: SIMULTANEOUS EQUILIBRIA
Experiment 7: SIMULTANEOUS EQUILIBRIA Purpose: A qualitative view of chemical equilibrium is explored based on the reaction of iron(iii) ion and thiocyanate ion to form the iron(iii) thiocyanate complex
More informationDYNAMIC EQUILIBRIUM STUDY GUIDE multiple choice
DYNAMIC EQUILIBRIUM STUDY GUIDE multiple choice Multiple Choice Section: This study guide is a compilation of questions from provincial exams since April 1994. I urge you to become intimately familiar
More informationCHEMISTRY 130 General Chemistry I OXIDATION-REDUCTION CHEMISTRY
CHEMISTRY 130 General Chemistry I OXIDATION-REDUCTION CHEMISTRY A solution of potassium permanganate is pink. [1] Color changes can often be used to monitor chemical reactions. DEPARTMENT OF CHEMISTRY
More informationExperiment 6 Shifts in Equilibrium: Le Châtelier s Principle
Experiment 6 Shifts in Equilibrium: Le Châtelier s Principle Introduction Whenever a chemical reaction occurs, the reverse reaction can also occur. As the original reactants, on the left side of the equation,
More informationCalorimetric Determination of Reaction Enthalpies
H + (aq) + OH - q H 2 O Calorimetric Determination of Reaction Enthalpies Purpose: Determine the enthalpy of dissociation of CH 3 COOH CH 3 COOH (aq) CH 3 COO - (aq) + H + (aq) Techniques: Calorimetry
More information+ H 2 O Equation 1. + NaOH CO 2 Na
Experiment # 5 VINEGAR: AN FDA INVESTIGATION Objective In this experiment, you will play the role of an FDA analytical chemist, You will verify whether a vinegar manufacturer's quality control lab remains
More informationCHEMpossible. 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
More informationScience Olympiad Regional UW-Milwaukee Chemistry test 2013
Science Olympiad Regional UW-Milwaukee Chemistry test 2013 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. What is another name for the representative
More informationChemical Reactions. Section 7.1: Nature of Reactions
Chemical Reactions Section 7.1: Nature of Reactions When do chemical reactions take place? What is the role of energy in chemical reactions? 1 Chemical Reactions It is a change in matter that produces
More informationThe Titration of Acetic Acid in Vinegar
Experiment 22 Revision 1.0 The Titration of Acetic Acid in Vinegar To learn about Volumetric Analysis and Titration. To learn about Aceticc Acid and Vinegar. To learn about Weak Acids. To learn about Equilibria
More informationSolubility & Equilibrium Unit Review
Solubility & Equilibrium Unit Review This review is worth 3 marks of your total test marks. It must be completed on test day. 3 marks will be given to students who have fully completed this review with
More informationLowell High School AP Chemistry Spring 2009 REACTION KINETICS EXPERIMENT
Lowell High School AP Chemistry Spring 2009 REACTION KINETICS EXPERIMENT Complete the following for Pre-Lab on a clean sheet of paper: (1) In your own words, explain the following: a. why the I 2 concentration
More informationChemical Equilibrium: Le Chatelier s Principle Examples of Chemical Equilibria
E6 Chemical Equilibrium: Le Chatelier s Principle Examples of Chemical Equilibria Objective! Observe several interesting and colorful chemical reactions that are examples of chemical systems at equilibrium.!
More information*You should work in groups of no more than 3 students. Each individual is responsible for all data and information in their own booklet.
Name Period 1 *You should work in groups of no more than 3 students. Each individual is responsible for all data and information in their own booklet. Pre-Lab Questions: What is the molarity equation?
More informationAcid-Base Titration Acetic Acid Content of Vinegar
Acid-Base Titration Acetic Acid Content of Vinegar Prelab Assignment Read the entire lab. Write an objective and any hazards associated with this lab in your laboratory notebook. On a separate sheet of
More information2002 D Required 2001 D Required
2002 D Required A student is asked to determine the molar enthalpy of neutralization, H neut, for the reaction represented above. The student combines equal volumes of 1.0 M HCl and 1.0 M NaOH in an open
More informationIII.2 Calculating Solubility and Ion Concentrations. ***This is a re-visitation to Chemistry 11: translating grams/l to moles/l (M) and back again.
III.2 Calculating Solubility and Ion Concentrations Solubility ***This is a re-visitation to Chemistry 11: translating grams/l to moles/l (M) and back again. Grams moles (M) L L Since Solubility is a measure
More informationSect 7.1 Chemical Systems in Balance HMWK: Read pages
SCH 4UI Unit 4 Chemical Systems and Equilibrium Chapter 7 Chemical Equilibrium Sect 7.1 Chemical Systems in Balance HMWK: Read pages 420-424 *Some reactions are reversible, ie not all reactions are as
More informationChem 1A Dr. White Fall Handout 4
Chem 1A Dr. White Fall 2014 1 Handout 4 4.4 Types of Chemical Reactions (Overview) A. Non-Redox Rxns B. Oxidation-Reduction (Redox) reactions 4.6. Describing Chemical Reactions in Solution A. Molecular
More informationChemistry 30 Mr. de Bruin Unit 3 Assignment.
NAME: Chemistry 30 Mr. de Bruin Unit 3 Assignment. All work must be fully shown in all questions to get process marks. As this is a summative assessment item, questions of clarification may be asked, but
More information