Experiment 2: The Rate of an Iodine Clock Reaction
|
|
- Benedict Lang
- 6 years ago
- Views:
Transcription
1 Experiment 2: The Rate of an Iodine Clock Reaction Introduction: Some reactions, including most of the ones that you have seen before, occur so rapidly that they are over as soon as the reactants are mixed. There are many more reactions, however, that are slower; they may require minutes, hours, days, or even years to reach completion. A few chemical reactions are so slow that it is difficult to show that they happen at all. Why the wide differences in reaction rates? Some of the factors that affect the rate of a given reaction are the Activation Energy of the reaction, the concentrations of the reactants, the presence of a catalyst (which affects the Activation Energy), and the temperature at which the reaction occurs. Purpose: In the quantitative part of this experiment, you will determine the rate law for an iodine clock reaction and the influence of temperature on that reaction. There are actually many different iodine clock reactions. They all have a common feature: the completion of the reaction is signaled by the appearance of the dark blue-black color that is characteristic of the interaction of molecular iodine (I 2 ) with starch. This color may appear so abruptly that it is as startling as an alarm clock. The rate of an iodine clock reaction depends on the concentrations of the reactants, as you would expect. As a result, the time required for the appearance of the dark color can be adjusted by adjusting the concentrations of the reactants. In this reaction, the rate of the reduction of ammonium persulfate ((NH 4 ) 2 S 2 O 8 ) with potassium iodide (KI) will be studied. The net ionic equation for this reaction is: Rxn 1) S 2 O 8 + 2I - 2SO 4 + I 2 One of the purposes of this experiment is to determine the rate law for this reaction. The rate law's general form will be: Eq 1) Rate = k[s 2 O 8 ] q [I - ] r and you will need to determine values for the rate constant k and the exponents q and r. Remember that the exponents must be determined experimentally; they cannot be obtained simply by looking at the balanced equation. The rate law will be deduced by the initial-rate method, using three experiments. Experiment 1 will be the reference with which the other two will be compared. In Experiment 2, the initial concentration of the S 2 O 8 ions will be twice that in Experiment 1, but the concentration of I - ions will be unchanged. The general form of the rate law for each of these experiments will be: Experiment 1: Rate 1 = k[s 2 O 8 ] q [I - ] r Experiment 2: Rate 2 = k(2[s 2 O 8 ]) q [I - ] r = 2 q rate 1 Chem 401 Lab Manual M Samples Revision 1/30/15 page 3
2 The rate in the second experiment will be 2 q times the original rate. In Experiment 3, the initial concentration of S 2 O 8 ions will be the same as that in Experiment 1, but the concentration of I - ions will be doubled. The rate law will be: Experiment 3: Rate 3 = k[s 2 O 8 ] q (2[I - ]) r = 2 r rate 1 The rate in this experiment will be 2 r times the original rate. You can deduce the true values of q and r from the ratios rate 2 /rate 1 and rate 3 /rate 1 and the initial concentrations of S 2 O 8 and I - ions. After you have evaluated the exponents, you will know the general form of the rate law, but the value of the rate constant will be unknown. You can obtain it from the rate law and any one of the three rates. Each rate should yield the same rate constant within experimental error. However, in order to derive the exponents and the rate law, you need to measure the rate of the reactions. How? In an initial rates method, you need to know the initial concentrations of the reactants (just a dilution calculation), but you also must determine the concentration of at least one of the reactants during the reaction. In this experiment, we will indirectly measure the concentration of the persulfate ions (S 2 O 8 ). Based on the persulfate ion, the rate of the reaction is given by: Eq 2) Rate = S O 2 8 t To find the rate, you will need to know or measure Δ[S 2 O 8 ], the initial change in the concentration of S 2 O 8 ions, and t, the time elapsed during that change. An easy way to obtain Δ[S 2 O 8 ] is by coupling another reaction to the one we are studying. The new reaction is the reduction of I 2 by Na 2 S 2 O 3 (sodium thiosulfate). The net ionic equation for this reaction is: Rxn 2) I 2 + 2S 2 O 3 2I - + S 4 O 6 where S 4 O 6 is the tetrathionate ion. It is important to remember that this reaction is used only as a means of studying the rate of the first reaction. The new reaction is fast. As a result, I 2 is consumed in this reaction as fast as it is formed in the first reaction. Essentially there can be no I 2 present as long as there are S 2 O 3 ions present. However, these ions are being consumed because of the second reaction. As soon as all the S 2 O 3 ions have reacted, I 2 from the first reaction begins to accumulate in the solution. You can detect the sudden presence of I 2 by the sudden appearance of the dark color from the interaction of I 2 with starch, which will be used as an indicator. You will know Δ[S 2 O 8 ] at the instant that this dark color appears. How? The stoichiometry and relative rates of the coupled reactions require the following relationship between Δ[S 2 O 8 ] and Δ[S 2 O 3 ]: Eq 3) [S 2 O 8 ] = 0.5 [S 2 O 3 ] where Eq 4) [S 2 O 3 ] = final [S 2 O 3 ] - initial [S 2 O 3 ] Chem 401 Lab Manual M Samples Revision 1/30/15 page 4
3 Essentially all the S 2 O 3 ions will have reacted when the dark color appears, so the final concentration of these ions is essentially zero, and Δ[S 2 O 3 ] becomes: Eq 5) [S 2 O 3 ] = - initial [S 2 O 3 ] = -[S 2 O 3 ] 0 Therefore, Δ[S 2 O 8 ] can be found as: Eq 6) [S 2 O 8 ] = -0.5 [S 2 O 3 ] 0 By combining Equation 2 and Equation 6, we obtain: Eq 7) rate rxn = 0.5 S O 2 3 Δt 0 If we keep the initial concentration of S 2 O 3 ions very small, Δ[S 2 O 3 ] will be small and Δ[S 2 O 8 ] will be even smaller. As a consequence, there will be little change in the concentration of the reactants during the elapsed time Δt. This is a necessary condition for the initial rates method. The time required for the appearance of the dark color is affected by the concentration of the reactants, as you would expect from the general form of the rate law. The time is also affected to a degree by the overall concentration of ions and their charges. This influence, which is well known, cannot be predicted from the rate law. You will maintain a constant volume by the addition of DI water as required. Although this is not quite correct, as we should also be maintaining a constant concentration of charges and ions, this is an advanced topic that we shall ignore now. Lastly, you will demonstrate the influence of the temperature on the rate of this reaction. To do this, you will redo Experiment 1 at three higher temperatures. The rate law will have the same general form at the higher and lower temperatures. As a result, q and r will not change when the temperature is varied. A new rate constant, however, will need to be found at the higher temperatures. The activation energy for the reaction can then be calculated via the Arrhenius equation using all four points and thru the point Adjusted form of the Arrhenius equation using two points. Chemicals: 0.20 M KI 0.20 M (NH 4 ) 2 S 2 O 8 (ammonium persulfate) 3% Starch Sln distilled water M Na 2 S 2 O 3 (sodium thiosulfate) Day 1 Equipment: Thermometer 16x150 test tubes, 3 & test tube rack Waste Beaker 2 ml Pipetman Pipet Tips, 5 Stopwatch 10 ml Beakers, 5 Stir rods, if desired Day 2 Equipment: Thermometer 20x150 mm Test Tubes, 5 & large test tube rack Waste Beaker 2 ml Pipetman Pipet Tips, 5 Stopwatch 10 ml Beakers, 5 Hot Water Baths Stir rods, if desired Chem 401 Lab Manual M Samples Revision 1/30/15 page 5
4 Waste Disposal: All solutions must be disposed of in the proper waste container. Day 1 Procedure: 1. Label 3 clean, dry test tubes as follows: Rxn 1, Rxn 2, Rxn 3. These are the reactions you will conduct on Day 1. Obtain a tray to work on. 2. Label 4 10 ml beakers with the different chemical formulas; DI Water; KI; Starch; Na 2 S 2 O 3. Make sure they are clean & dry. Try to pour around 3-4 ml of each chemical into the appropriately labeled beaker. BE CAREFUL TO POUR THE CORRECT CHEMICAL INTO YOUR BEAKERS! READ AND REREAD THE LABELS! 3. Note and record the temperature of the lab to the nearest 0.1 C. 4. Make sure all your pipet tips are clean & dry. One of these tips is dedicated to ammonium persulfate. If you have 5 pipet tips, label them carefully with the 5 different chemicals, and place each tip in the beaker with the appropriate chemical (the 5 th tip is for ammonium persulfate, Step 8 below). 5. Using a pipetman, add the appropriate amounts of KI to the labeled reaction test tube. BE CAREFUL TO USE THE CORRECT CHEMICAL AND CORRECT AMOUNT! Constantly check your Table of Volumes. 6. Clean & dry the pipet tip if you have to reuse it for a different chemical. Otherwise, place it back in the KI beaker. 7. Repeat Steps 5 and 6 for DI Water, Na 2 S 2 O 3, and 3% Starch. Mix the contents of the reaction test tube by agitating by hand or by using a stir rod. If you use a stir rod, clean and dry it each time after using it. 8. Pour about 3-4 ml of ammonium persulfate, (NH 4 ) 2 S 2 O 8, into a clean, dry, labeled 10 ml beaker. You will start each reaction upon the addition of this chemical. 9. READ STEPS 10 AND 11 COMPLETELY BEFORE PROCEEDING! 10. Start the stopwatch JUST as you pipet the required amount of (NH 4 ) 2 S 2 O 8 to reaction test tube 1. Mix thoroughly, and you may continue to shake it gently or stir it as the reaction progresses. 11. Stop the stopwatch at the EXACT time when the solution turns dark (blue) throughout the solution. BE ALERT! This color may appear suddenly throughout the entire solution. (Note: Experiment 1 should take around 5-12 minutes depending on the exact solution concentrations.) 12. Record the elapsed time. 13. Repeat Steps for Experiments 2 and 3 in test tubes 2 and 3, using the appropriate amounts of (NH 4 ) 2 S 2 O 8. Check your data with your instructor to see if you need to repeat any Experiment. 14. Dispose of all waste in the appropriate container, and clean all glassware and the tray. Return any borrowed items (Except the pipetman, keep reading!). Clean your area. Take your pipetman along with your data to the instructor and obtain a data initial. Put the pipetman back on the pipetman rack. 15. Do Data Analysis Steps 1 and 2 and obtain a data analysis initial. Chem 401 Lab Manual M Samples Revision 1/30/15 page 6
5 Day 2 Procedure: On day 2, you will need approximately 2 ml KI, DI Water, Starch, and Na 2 S 2 O 3 ; and 1 ml of (NH 4 ) 2 S 2 O 8. Label 10 ml beakers and add the appropriate amount of each chemical (less than half full). Make sure these beakers are clean! You may do Experiments 4-7 in any order, although the procedure is written for a specific order. 1. Label 4 20x150 mm clean and dry test tubes as follows: 4, 5, 6, 7. These are the 4 reactions you will conduct on Day 2. The 5 th test tube is dedicated for ammonium persulfate. Label the 5 th test tube (NH 4 ) 2 S 2 O 8. Obtain a spill tray. 2. Make sure the pipet tips are clean and dry or you will need to rinse them and prime them with the chemical. As on Day 1, add the appropriate amount of KI, DI Water, Na 2 S 2 O 3, and 3% Starch to each of your 4 labeled reaction test tubes. Mix well by shaking by hand or by stirring with a stir rod. If you use a stir rod, remove the stir rod and clean and dry it each time you use it. 3. For Experiment 4, have the stopwatch ready. Pipet ml of ammonium persulfate into the ammonium persulfate test tube and then pour it into your waste beaker (this way we coat the bottom of the test tube). Again, pipet ml of ammonium persulfate into the ammonium persulfate test tube and go to step Pour the contents of the ammonium persulfate test tube into test tube #4 (Experiment 4), start the stopwatch, mix quickly by shaking by hand, and place the reaction test tube back in the test tube rack.* Note: Put the ammonium persulfate test back in your test tube rack at your bench. You may reuse the ammonium persulfate test tube for Experiments 5-7 without cleaning and drying it. 5. When the reaction is complete (turns blue as on Day 1), stop the stopwatch, and record the elapsed time. 6. For Experiment 5, you will use a hot water bath at approximately 40 C. 7. Place this labeled test tube in the hot water bath. 8. Pipet ml of the (NH 4 ) 2 S 2 O 8 into the ammonium persulfate test tube. Place this labeled test tube in the hot water bath as well. 9. Let both test tubes sit in the hot water bath for 5 minutes. 10. GET READY TO START TIMING! READ THE STEPS BEFORE PROCEEDING! 11. Remove both test tubes from the hot water bath (to avoid contaminating the hot water bath), quickly add the warm (NH 4 ) 2 S 2 O 8 to the warm reaction test tube. Start the stopwatch. 12. Shake the reaction test tube for a few seconds (without spilling or splashing). Replace the reaction test tube in the hot water bath. The ammonium persulfate test tube may go back in your test tube rack at your bench. 13. BE ALERT! Stop the stopwatch at the EXACT time when the solution turns dark (blue). 14. Remove the test tube, and note and record the actual temperature of the hot water bath. 15. Record the elapsed time. 16. Repeat steps 6-15 for Experiment 6 at approximately 50 C and for Experiment 7 at approximately 60 C. 17. Dispose of all waste in the appropriate container, and clean all glassware and the tray. Return any borrowed items (Except the pipetman, keep reading!). Clean your area. Take your pipetman along with your data to the instructor and obtain a data initial. Put the pipetman back on the rack. 18. Continue working on the Data Analysis and obtain a data analysis initial at the end of the lab. * This seems awkward, but you are mimicking what you will be doing with the other reactions this day. Chem 401 Lab Manual M Samples Revision 1/30/15 page 7
6 Data: Fill in the data section at the end of the lab. Data Analysis: 1. Calculate [S 2 O 3 ] 0 for the reaction solution for experiments 1-3. Remember that these are diluted solutions, so you are solving for M 2 in the dilution equation M 1 V 1 =M 2 V 2. M 2 is the initial concentration just before the reaction started but after all of the solutions were mixed together. Look at the volume table on page 9 so that you use the correct start concentrations, the correct volume of S 2 O 3, and the correct total volume for all of the experiments. Show all units and work and equations. 2. Calculate the initial rates for Exp. 1, 2, and 3 from Equation 7 and the [S 2 O 3 ] 0 you just calculated in Data Analysis Calculate [S 2 O 8 ] 0 and [I - ] 0 for each experiment (including Exp 4-7) using M 1 V 1 =M 2 V 2. Show all units and work. Again, look at the volume table on page 9 so that you know exactly what volumes, etc. were actually used for each experiment. 4. Make a Table like the following (fill in the blanks with your results for Exp 1-3): Exp # [I - ] 0 [S 2 O 8 ] 0 rate (M/s) Determine the reaction orders with respect to I - and S 2 O 8. These should be whole numbers, so you will need to round to the nearest whole number. Show all units and work, however, you may be able to determine the reaction orders by eyeballing the start concentrations and the rates. 5. Write the correct rate equation. You are now done with Day 1 data! In Steps 6 and 7 you will use Day 2 data and this rate law to calculate the rate constant k for 4 different temperatures. 6. Calculate the rate for Experiments 4-7 exactly as you did for Experiments 1-3 in Steps 1 and 2 above. 7. Calculate the rate constant k for Experiments 4-7 using the rates you just calculated in Step 6, the concentrations of [S 2 O 8 ] 0 and [I - ] 0 from Step 3, and the rate equation you found in Step 5. Show all units and work. 8. Using your room temperature k (from Exp 4 on Day 2), and one of your k values from an elevated temperature, use the adjusted point form of the Arrhenius Equation to calculate E a. Show all units, work, and equations. 9. Now you have 4 rate constants for 4 different temperatures. Determine the Activation Energy from the slope of a linear plot of lnk vs. 1/T. Y-axis is ln(k). Show all units, work, and equations. Discussion/Errors: 1) Compare your rate law to the known room temperature rate law of rate = [I - ][ S 2 O 8 ]; 2) discuss how your k values change with temperature; 3) calculate the %- error between your room temperature k and the accepted room temperature k of ; 4) compare your two E a values (which should be more accurate and why); and 5) discuss possible or known sources or errors. Use your graphs to highlight errors that may be seen; graphs often show errors in accuracy and precision. Chem 401 Lab Manual M Samples Revision 1/30/15 page 8
7 Data/Observations: Pipetman Day 1: Pipetman Day 2: Laboratory Temperature: Day 1 3% Volumes (ml) of Solutions for Experiments (May Change): Experiment 0.20 M DI Water M 0.20 M KI Na 2 S 2 O 3 Starch (NH 4 ) 2 S 2 O , 5, 6, Note that the total volume for each experiment is ml (May change). Elapsed Times for Iodine Clock Reactions Experiment Elapsed Time (s) Observations (what color blue, etc.) (Day 2) 5 (Day 2) 6 (Day 2) 7 (Day 2) Temperature of Reaction Solution for Experiment 4: 5: 6: 7: Formulas: Arrhenius Equation (in form of equation of line: y = mx + b) ln(k) = E a RT + ln(a) Pt Adjusted Form of Arrhenius Equation: ln k 2 k 1 = E a 1 1 R T 1 T 2 Chem 401 Lab Manual M Samples Revision 1/30/15 page 9
Kinetics of an Iodine Clock Reaction
Kinetics of an Iodine Clock Reaction Introduction: In this experiment, you will determine the rate law for a reaction and the effect of concentration on the rate of the reaction by studying the initial
More informationKinetics of an Iodine Clock Reaction
Kinetics of an Iodine Clock Reaction Introduction: In this experiment, you will determine the rate law for a reaction and the effect of concentration on the rate of the reaction by studying the initial
More informationCHM112 Lab Iodine Clock Reaction Part 2 Grading Rubric
Name Team Name CHM112 Lab Iodine Clock Reaction Part 2 Grading Rubric Criteria Points possible Points earned Lab Performance Printed lab handout and rubric was brought to lab 3 Initial concentrations completed
More informationDetermining the Rate Law for a Chemical Reaction
Determining the Rate Law for a Chemical Reaction Purpose: To determine the reaction orders, rate law, and rate constant for the reaction between persulfate ions, SO8 -, and iodide ions, I - Introduction
More informationEXPERIMENT 1 REACTION RATE, RATE LAW, AND ACTIVATION ENERGY THE IODINE CLOCK REACTION
PURPOSE: To determine the Rate Law and the Activation Energy for a reaction from experimental data. PRINCIPLES: The Rate Law is a mathematical expression that predicts the rate of a reaction from the concentration
More informationExperimental Procedure Lab 402
Experimental Procedure Lab 402 Overview Measured volume of several solutions having known concentrations of reactants are mixed in a series of trials. The time required for a visible color change to appear
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 informationIODINE CLOCK REACTION KINETICS
Name: Section Chemistry 104 Laboratory University of Massachusetts Boston IODINE CLOCK REACTION KINETICS PRELAB ASSIGNMENT Calculate the initial concentration of H 2 O 2 that exists immediately after mixing
More informationExperiment #5. Iodine Clock Reaction Part 1
Experiment #5. Iodine Clock Reaction Part 1 Introduction In this experiment you will determine the Rate Law for the following oxidation- reduction reaction: 2 H + (aq) + 2 I (aq) + H 2 O 2 (aq) I 2 (aq)
More informationRate Properties of an Iodide Oxidation Reaction
Rate Properties of an Iodide Oxidation Reaction GOAL AND OVERVIEW The rate law for the reduction reaction of peroxodisulfate (PODS) by iodide: S 2 O8 2 (aq) + 2 I (aq) I 2 (aq) + 2 SO4 2 (aq) will be determined.
More informationCHM112 Lab Iodine Clock Reaction Part 1 Grading Rubric
Name Team Name CHM112 Lab Iodine Clock Reaction Part 1 Grading Rubric Criteria Points possible Points earned Lab Performance Printed lab handout and rubric was brought to lab 3 Initial concentrations completed
More informationA Chemical Clock. 5. Consider each of the following questions regarding data and measurements:
A Chemical Clock Things to Consider 1. What are the three major objectives of this experiment? What methods will you try using to achieve each of these three objectives? 2. What is difference between reaction
More informationExamining the Effect of Temperature on Reaction Rate
1 Purpose: To measure reaction rate at different temperatures for the reaction between persulfate ions, S2O8-2, and iodide ions, I -, and thereby determine the activation energy and frequency factor for
More informationA STUDY OF REACTION RATES
CH095 A Study of Reaction Rates Page 1 A STUDY OF REACTION RATES Chemical reaction rates are affected by changes in concentration of the reactants and temperature. How concentration and temperature affect
More informationKinetics; A Clock Reaction
Kinetics; A Clock Reaction Background This experiment involves the study of the rate properties, or chemical kinetics, of the following reaction between iodide ion (I - ) and bromate ion (BrO 3 - ) under
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 3 THE IODINE CLOCK
EXPERIMENT 3 THE IODINE CLOCK Introduction The Rates of Chemical Reactions Broadly defined, chemical kinetics is the study of the rates at which chemical reactions proceed. Oftentimes, reaction rate data
More informationExperiment 26 - Kinetics
Chem 1B Dr. White 175 Experiment 26 - Kinetics Objectives To determine the rate law for the reaction between iodide and bromate under acidic conditions To investigate the effect of temperature on rate
More informationIodine Clock Part I Chemical Kinetics
Collect: Iodine Clock Part I Chemical Kinetics (2015/11/17 revised) 50 ml Erlenmeyer flask (10): wash clean, dry, and cool 5 ml graduated pipet (2), pipet filler (1) Cork stopper (6) Stopwatch (1) (given
More information#5 Chemical Kinetics: Iodine Clock Reaction
#5 Chemical Kinetics: Iodine Clock Reaction In the previous experiment, we discussed the factors that influence the rate of a chemical reaction and presented the terminology used in quantitative relations
More informationCHEM Experiment 1 Factors Governing the Speed of Chemical Reactions
CHEM 3310 Experiment 1 Factors Governing the Speed of Chemical Reactions Experiment 1: Factors Affecting Reaction Rates Part A Effect of Concentration on Reaction Rate CHEM 3310 2 Iodine clock Reaction
More informationHow Do Certain Factors Affect the Rate of a Chemical Reaction?
EXPERIMENT 7 How Do Certain Factors Affect the Rate of a Chemical Reaction? INTRODUCTION Two important questions may be asked about a chemical reaction. () How completely do the reactants combine to give
More informationExperiment 2: Factors Affecting Reaction Rates
Objective: Part A To determine the effect of concentration on the rate of formation of Iodine, I 2, and therefore, determine the reaction s rate law. Part B To study the effect of temperature on the rate
More informationExperiment 7 Can You Slow It Down?
Experiment 7 Can You Slow It Down? OUTCOMES After completing this experiment, the student should be able to: tell which factors influence the reaction rate and how they influence the rate. change the temperature
More informationThe Kinetics of the Iodine Clock Reaction
Experiment 2 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 on a separate (new)
More informationCHEM Experiment 1. of Chemical Reactions
Experiment 1 Factors Governing the Speed of Chemical Reactions Experiment 1: Factors Affecting Reaction Rates Part A Effect of Concentration on Reaction Rate 2 Iodine clock Reaction S 2 O 8 (aq) + 2 I
More informationDetermination of the Rate Constant for an Iodine Clock Reaction
CHEM 122L General Chemistry Laboratory Revision 1.3 Determination of the Rate Constant for an Iodine Clock Reaction To learn about Integrated Rate Laws. To learn how to measure a Rate Constant. To learn
More informationTHE EFFECT OF TEMPERATURE AND CONCENTRATION ON REACTION RATE
THE EFFECT OF TEMPERATURE AND CONCENTRATION ON REACTION RATE INTRODUCTION FACTORS INFLUENCING REACTION RATE: The study of chemical reactions is not complete without a consideration of the rates at which
More informationKinetics of an Iodine Clock Reaction Lab_ Teacher s Key
Kinetics of an Iodine Clock Reaction Lab_ Teacher s Key Purpose: In this lab, you will find the reaction rate, rate law,, and observe the effects of a catalyst for the oxidation of iodide ions by bromate
More informationKinetics of an Iodine Clock Reaction Lab_Student Copy
Kinetics of an Iodine Clock Reaction Lab_Student Copy Purpose: Purpose: In this lab, you will find the reaction rate, rate law,, and observe the effects of a catalyst for the oxidation of iodide ions by
More informationExperiment #12. Enthalpy of Neutralization
Experiment #12. Enthalpy of Neutralization Introduction In the course of most physical processes and chemical reactions there is a change in energy. In chemistry what is normally measured is ΔH (enthalpy
More informationChemistry 1B Experiment 17 89
Chemistry 1B Experiment 17 89 17 Thermodynamics of Borax Solubility Introduction In this experiment, you will determine the values of H and S for the reaction which occurs when borax (sodium tetraborate
More informationCIE Chemistry A-Level Practicals for Papers 3 and 5
CIE Chemistry A-Level Practicals for Papers 3 and 5 Rate of Reaction Disappearing cross: Change in rate of the reaction of sodium thiosulphate with hydrochloric acid as temperature is changed: Na 2 S 2
More informationPURPOSE: To determine the Rate Law for the following chemical reaction:
PURPOSE: To determine the Rate Law for the following chemical reaction: H 2 O 2 (aq) + 2 I - (aq) + 2 H 3 O + (aq) 4 H 2 O(l) + I 2 (aq) Hydrogen Iodide Hydronium Water Iodine Peroxide Ion Ion PRINCIPLES:
More informationSolubility Product Constants
Solubility Product Constants PURPOSE To measure the solubility product constant (K sp ) of copper (II) iodate, Cu(IO 3 ) 2. GOALS To measure the molar solubility of a sparingly soluble salt in water. To
More informationExperiment #10: Analysis of Antacids
Experiment #10: Analysis of Antacids Purpose: In this experiment you will prepare one solution that is approximately 0.1 M NaOH. Then you will standardize this solution, which means that you will experimentally
More informationThe thermodynamics of the solubility of borax
Chemistry 1 6 3 The thermodynamics of the solubility of borax Purpose: To determine the thermodynamic quantities ΔH and ΔS for the solvation reaction of borax in water by measuring the solubility product
More informationCHEMICAL KINETICS E + 2B 2C + D (1)
CHEMICAL KINETICS Chemical kinetics is the branch of chemistry that is concerned with the study of the rates and mechanisms of chemical reactions. The rate of a reaction is a measure of its speed. Consider
More informationSupernatant: The liquid layer lying above the solid layer after a precipitation reaction occurs.
Limiting Reagent Introduction The quantities of substances involved in a chemical reaction represented by a balanced equation are often referred to as stoichiometric amounts. Solution stoichiometry is
More informationEXPERIMENT 6: Photometric Determination of an Equilibrium Constant
EXPERIMENT 6: Photometric Determination of an Equilibrium Constant The following preparatory questions should be answered before coming to class. They are intended to introduce you to several ideas important
More informationChemistry 213. A KINETIC STUDY: REACTION OF CRYSTAL VIOLET WITH NaOH LEARNING OBJECTIVES
Chemistry 213 A KINETIC STUDY: REACTION OF CRYSTAL VIOLET WITH NaOH The objectives of this experiment are to... LEARNING OBJECTIVES study the reaction rate of crystal violet with NaOH using a Spectronic
More informationExperiment #7. Determination of an Equilibrium Constant
Experiment #7. Determination of an Equilibrium Constant Introduction It is frequently assumed that reactions go to completion, that all of the reactants are converted into products. Most chemical reactions
More informationA Clock Reaction: Determination of the Rate Law for a Reaction
1 A Clock Reaction: Determination of the Rate Law for a Reaction This experiment involves the study of the rate properties, or chemical kinetics, of the following reaction between iodide ion and bromate
More informationThe Thermodynamics of the Solubility of Borax
Experiment 10 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 on a separate
More informationTHE EFFECT OF TEMPERATURE AND CONCENTRATION ON REACTION RATE
THE EFFECT OF TEMPERATURE AND CONCENTRATION ON REACTION RATE INTRODUCTION FACTORS INFLUENCING REACTION RATE: The study of chemical reactions is not complete without a consideration of the rates at which
More informationThe Decomposition of Hydrogen Peroxide. Evaluation copy
The Decomposition of Hydrogen Peroxide Computer 12 The decomposition of hydrogen peroxide in aqueous solution proceeds very slowly. A bottle of 3% hydrogen peroxide sitting on a grocery store shelf is
More informationSafety Note: Safety glasses and laboratory coats are required when performing this experiment
The Determination of Hypochlorite in Bleach Reading assignment: Burdge, Chemistry 4 th edition, section 4.6. We will study an example of a redox titration in order to determine the concentration of sodium
More informationH + [ ] [ ] H + NH 3 NH 4. = poh + log HB +
Titration Lab: Determination of a pk a for an Acid and for a Base Theory A Brønsted-Lowry acid is a substance that ionizes in solution (usually aqueous, but it doesn t have to be, ammonia is often used
More informationExperiment 2: Analysis of Commercial Bleach Solutions
Experiment 2: Analysis of Commercial Bleach Solutions I. Introduction The ability of household bleach to remove stains is related to the amount of oxidizing agent in it. The oxidizing agent in bleach is
More informationTHE TEMPERATURE DEPENDENCE OF THE EQUILIBRIUM CONSTANT
Experiment 7B THE TEMPERATURE DEPENDENCE OF THE EQUILIBRIUM CONSTANT Prepared by Ross S. Nord, Chemistry Department, Eastern Michigan University PURPOSE To investigate the relationship between the equilibrium
More informationC q T q C T. Heat is absorbed by the system H > 0 endothermic Heat is released by the system H < 0 exothermic
PLEASE REORD ALL DATA DIRETLY INTO YOUR LAB NOTEBOOKS Introduction Heating a substance is one of the simplest processes carried out in the chemical laboratory, and is usually accompanied by a rise in the
More informationExperiment 4: Rates of Chemical Reactions II: Kinetic Study of the Reaction between Ferric and Iodine Ions
Experiment 4: Rates of Chemical Reactions II: Kinetic Study of the Reaction between Ferric and Iodine Ions PURPOSE: To study kinetics of the reaction between ferric (Fe 3+ ) and iodide (I - ) ions, i.e.
More informationKINETICS: INITIAL RATES
Experiment 6B KINETICS: INITIAL RATES Prepared by Ross S. Nord, Stephen E. Schullery, and Masanobu M. Yamauchi, Eastern Michigan University PURPOSE Learn how to measure initial rates. Determine the order
More informationLab #5 - Limiting Reagent
Objective Chesapeake Campus Chemistry 111 Laboratory Lab #5 - Limiting Reagent Use stoichiometry to determine the limiting reactant. Calculate the theoretical yield. Calculate the percent yield of a reaction.
More informationEXPERIMENT 8 Determining K sp
EXPERIMENT 8 Determining K sp Introduction The solubility product constant, or K sp of a compound is an equilibrium constant that describes the degree to which a solid dissolves in water. The K sp is calculated
More informationChemical Equilibrium: Finding a Constant, Kc
Chemical Equilibrium: Finding a Constant, Kc Computer 20 The purpose of this lab is to experimentally determine the equilibrium constant, K c, for the following chemical reaction: Fe 3+ (aq) + SCN (aq)
More information8 Enthalpy of Reaction
E x p e r i m e n t Enthalpy of Reaction Lecture and Lab Skills Emphasized Calculating the heat and enthalpy of reactions. Writing net ionic equations. Using Hess s law to determine the enthalpy of a reaction.
More informationUNIT 2: KINETICS RATES of Chemical Reactions (TEXT: Chap 13-pg 573)
UNIT 2: KINETICS RATES of Chemical Reactions (TEXT: Chap 13-pg 573) UNIT 2: LAB 1. A Brief Introductory Kinetics Investigation A) Set up 4 test tubes containing about 5 ml of 0.1 M sodium oxalate sol n.
More informationUse this dramatic iodine clock reaction to demonstrate the effect of concentration, temperature, and a catalyst on the rate of a chemical reaction.
Clock Reaction Race Reaction Pathways SCIENTIFIC Introduction Use this dramatic iodine clock reaction to demonstrate the effect of concentration temperature and a catalyst on the rate of a chemical reaction.
More informationExperiment 2: Reaction Stoichiometry by Thermometric Titration
Experiment 2: Reaction Stoichiometry by Thermometric Titration Introduction The net result of a reaction (a chemical change) is summarized by a chemical equation. In order to write a chemical equation,
More informationChemical Equilibrium: Finding a Constant, Kc
Lab12 Chemical Equilibrium: Finding a Constant, Kc The purpose of this lab is to experimentally determine the equilibrium constant, K c, for the following chemical reaction: Fe 3+ (aq) + SCN (aq) FeSCN
More informationClocking the Effect of Molarity on Speed of Reaction. reaction. While most people do assume that the temperature of the solution is often the most
Ding 1 Chunyang Ding Mr. Rierson AP/IB Chemistry SL 28 January 2013 Clocking the Effect of Molarity on Speed of Reaction In basic levels of chemistry, most of the experimenter s attention is on the reaction
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 informationIodine Clock Challenge Rate Laws
Iodine Clock Challenge Rate Laws SCIENTIFIC Introduction The demonstration of an iodine clock involves a chemical reaction that suddenly turns blue due to the formation of the familiar iodine starch complex.
More informationChemistry CP Lab: Additivity of Heats of Reaction (Hess Law)
Chemistry CP Lab: Additivity of Heats of Reaction (Hess Law) Name: Date: The formation or destruction of chemical bonds is always accompanied by an energy exchange between the reactant molecules and the
More informationDetermination of an Equilibrium Constant Minneapolis Community and Technical College Principles of Chemistry II, C1152 v.1.16
Determination of an Equilibrium Constant Minneapolis Community and Technical College Principles of Chemistry II, C1152 v.1.16 I. Introduction Equilibrium Consider the following situation: It is rush hour
More informationWhat Is the Rate Law for the Reaction Between Hydrochloric Acid and Sodium Thiosulfate?
What Is the Rate Law for the Reaction Between Hydrochloric Acid and Sodium Thiosulfate? Introduction The collision theory of reactions suggests that the rate of a reaction depends on three important factors.
More informationDate Completed: Lab Partner(s):
Name: Lab Partner(s): Date Completed: Lab # 23: Factors Affecting Reaction Rate Accelerated Chemistry 1 Purpose Did you ever wonder why certain chemicals when mixed do not react; yet others upon immediate
More informationSynthesis and Analysis of a Coordination Compound
Synthesis and Analysis of a Coordination Compound In addition to forming salts with anions, transition metal cations can also associate with neutral molecules (and ions) through a process called ligation.
More informationAqueous Chemical Reactions
Aqueous Chemical Reactions Introduction Many chemical reactions occur in water and therefore they are considered aqueous chemical reactions. The reagents are typically dissolved or diluted in water and
More informationExperiment#1 Beer s Law: Absorption Spectroscopy of Cobalt(II)
: Absorption Spectroscopy of Cobalt(II) OBJECTIVES In successfully completing this lab you will: prepare a stock solution using a volumetric flask; use a UV/Visible spectrometer to measure an absorption
More informationLab Section. Observations and evidence for a chemical reaction:
Experiment #3: Shifting Reactions (Adapted from Exp. I-4 from Inquiries in Chemistry, 3 rd edition) Problem Statement: How can we shift reactions forward and backward? I. Data Collections and Analysis
More informationDetermination of Orthophosphate Ion
Determination of Orthophosphate Ion Introduction Phosphorous, in the form of phosphate, is one of several important elements in the growth of plants. Excessive algae growth in water is stimulated by the
More informationTHE IRON(III) THIOCYANATE REACTION SYSTEM
Experiment 7 THE IRON(III) THIOCYANATE REACTION SYSTEM Prepared by Ross S. Nord, Chemistry Department, Eastern Michigan University PURPOSE To investigate a novel reaction system by utilizing a spectrophotometer.
More informationEnzyme Catalysis Lab
AP Biology Name: Enzyme Catalysis Lab Objectives In this laboratory, you will observe the role of an enzyme (catalase) in conversion of hydrogen peroxide (H 2 O 2 ) to water and oxygen determine the rate
More informationRate law Determination of the Crystal Violet Reaction Using the Isolation Method
Rate law Determination of the Crystal Violet Reaction Using the Isolation Method Introduction A common challenge in chemical kinetics is to determine the rate law for a reaction with multiple reactants.
More informationSupernatant: The liquid layer lying above the solid layer after a precipitation reaction occurs.
Limiting Reagent Introduction The quantities of substances involved in a chemical reaction represented by a balanced equation are often referred to as stoichiometric amounts. Solution stoichiometry is
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 informationExperimental Procedure Lab 402
Experimental Procedure Lab 402 Overview One set of solutions having known molar concentrations of FeNCS 2+ is prepared for a calibration curve, a plot of absorbance versus concentration. A second set of
More information1-50 ml beaker stirring rod 1-10 ml beaker 0.10 M NaOH (1 ml) calibrated plastic dropper (1 ml) 50 ml dispensing burette (for Crystal Violet)
Exercise 2 Page 1 Illinois Central College CHEMISTRY 132 Name: Kinetics, Part II. Equipment Objectives. 1-50 ml beaker stirring rod 1-10 ml beaker 0.10 M NaOH (1 ml) calibrated plastic dropper (1 ml) 1.5x10-5
More informationChemical Equilibrium: Finding a Constant, Kc
Chemical Equilibrium: Finding a Constant, Kc Experiment 20 The purpose of this lab is to experimentally determine the equilibrium constant, K c, for the following chemical reaction: Fe 3+ (aq) + SCN -
More informationAqueous Chemical Reactions
Aqueous Chemical Reactions Introduction Many chemical reactions occur in water and therefore they are considered aqueous chemical reactions. The reagents are typically dissolved or diluted in water and
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 informationExperiment #13. Enthalpy of Hydration of Sodium Acetate.
Experiment #13 Enthalpy of Hydration of Sodium Acetate Goal To determine the enthalpy (ΔH) for the following process: NaC 2 H 3 O 2 (s) + 3 H 2 O(l) à NaC 2 H 3 O 2 3H 2 O(s) Introduction Most chemical
More informationPRACTICAL NUMBER 1 AN EXPERIMENT TO DETERMINE THE RATE CONSTANT AND THE REACTION ORDER FOR THE OXIDATION OF IODIDE BY PEROXODISULFATE
PRACTICAL NUMBER 1 AN EXPERIMENT TO DETERMINE THE RATE CONSTANT AND THE REACTION ORDER FOR THE OXIDATION OF IODIDE BY PEROXODISULFATE INTRODUCTION In this experiment you will determine the initial rate
More informationExperiment #8. LeChatelier s Principle
Experiment #8. LeChatelier s Principle Aim: To study the effect of concentration and temperature on chemical equilibrium When the rate of the forward reaction becomes equal to the rate of the reverse reaction,
More informationChem 1B Saddleback College Dr. White 1. Experiment 5: Separation and Identification of Group I Cations (The Chloride Group: Ag +, Pb 2+, and Hg 2
Chem 1B Saddleback College Dr. White 1 Experiment 5: Separation and Identification of Group I Cations (The Chloride Group: Ag +, Pb 2+, and Hg 2 2+) Objective To understand the chemical reactions involved
More informationCopper (II) Glycinate Titration
Copper (II) Glycinate Titration In this experiment you will standardize (determine the concentration of) a solution of sodium thiosulfate. You will then use that sodium thiosulfate solution to titrate
More informationTHE THERMODYNAMICS OF POTASSIUM NITRATE DISSOLVING IN WATER V010516
THE THERMODYNAMICS OF POTASSIUM NITRATE DISSOLVING IN WATER V010516 OBJECTIVE The ΔG, ΔH and ΔS of the potassium nitrate (KNO3) dissolving reaction will be determined by measuring the equilibrium constant
More informationActivity 2: Determine the Effect of Temperature on the Reaction Rate
STUDENT MANUAL Activity 2: Determine the Effect of Temperature on the Reaction Rate Temperature can affect the speed of the reaction. Heat can speed up the movement of the substrate and enzyme molecules,
More informationChem 2115 Experiment # 6 PERIODIC RELATIONSHIPS
Chem 2115 Experiment # 6 PERIODIC RELATIONSHIPS OBJECTIVES: Gaining insight into property and reactivity trends within families and across periods for the chemical elements through experimental observation.
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 informationKinetics of Crystal Violet Fading AP* Chemistry Big Idea 4, Investigation 11 An Advanced Inquiry Lab
Introduction Kinetics of Crystal Violet Fading AP* Chemistry Big Idea 4, Investigation 11 An Advanced Inquiry Lab Catalog o. AP7644S Publication o. 7644S Crystal violet is a common, beautiful purple dye.
More informationTo use calorimetry results to calculate the specific heat of an unknown metal. To determine heat of reaction ( H) from calorimetry measurements.
Calorimetry PURPOSE To determine if a Styrofoam cup calorimeter provides adequate insulation for heat transfer measurements, to identify an unknown metal by means of its heat capacity and to determine
More informationChemical Equilibrium: Finding a Constant, Kc
Chemical Equilibrium: Finding a Constant, Kc Experiment 20 The purpose of this lab is to experimentally determine the equilibrium constant, K c, for the following chemical reaction: Fe 3+ (aq) + SCN (aq)
More informationChemical Kinetics: Integrated Rate Laws. ** updated Procedure for Spec 200 use **
Chemical Kinetics: Integrated Rate Laws ** updated Procedure for Spec 200 use ** *DISCLAIMER: It is highly recommended that students bring in their own computers to lab this week to use excel. There may
More informationRead the lab thoroughly. Answer the pre-lab questions that appear at the end of this lab exercise.
Experiment 10 Stoichiometry- Gravimetric Analysis Pre-lab Assignment Read the lab thoroughly. Answer the pre-lab questions that appear at the end of this lab exercise. Purpose The purpose this experiment
More informationFactors in Reaction Rates
Section 6 Factors in Reaction Rates What Do You See? Learning Outcomes In this section you will Discover conditions that make a reaction proceed faster or slower. Discuss explanations for why this happens
More informationEXPERIMENT 17. Oxidation-Reduction Reactions INTRODUCTION
EXPERIMENT 17 Oxidation-Reduction Reactions INTRODUCTION Oxidizing agents are compounds or ions that contain an element capable of achieving a lower oxidation state by gaining electrons The stronger the
More informationPERIODIC RELATIONSHIPS
PERIODIC RELATIONSHIPS OBJECTIVES: Gaining insight into property and reactivity trends within families and across periods for the chemical elements through experimental observation. SKILLS: Observations,
More information