Determination of the Percentage Oxygen in Air
|
|
- Gillian Crawford
- 7 years ago
- Views:
Transcription
1 CHEM 121L General Chemistry Laboratory Revision 1.1 Determination of the Percentage Oxygen in Air In this laboratory exercise we will determine the percentage by volume of Oxygen in Air. We will do this by allowing the Oxygen in the Air to react with Iron in the form of Steel Wool. This will convert the gaseous Oxygen into solid Iron Oxide. This will cause the volume of the Air to decrease as it becomes devoid of Oxygen. Once the reaction is complete, the decrease in the Air s volume will be equal to the volume the gaseous Oxygen occupied in the Air. One of the earliest observations concerning combustion was that it stops when the supply of Air is removed from the combustible material. Various theories were put forth to explain this observation. The first of these theories to take hold was the Theory of Phlogiston. This theory, put forth in 1667 by Johann Joachim Becher, postulated; that bodies were composed of three earths - terra lapidea (vitreous), terra mercurialis (mercurial), terra pinguis (fatty). [Becher] considered combustible substances to be rich in terra pinguis, which was lost during burning,. Even metals that were calcinable contained some of the fatty earth. [These ideas were] later developed into an elaborate chemical system in which the term "phlogiston" replaced terra pinguis. The Development of Modern Chemistry Aaron J. Ihde
2 P a g e 2 According to this theory, during combustion, a hypothetical substance called Phlogiston is released. Air was believed to absorb the Phlogiston until a point of saturation. It is at this saturation point that combustion ceases, unless fresh Air is introduced. Material Dephlogisticated Material + Phlogisticated Air This theory was capable of explaining not only combustion and calcination, but was also capable of explaining the smelting of metal ores and respiration. Although inconvenient facts kept pointing to inconsistencies in the Theory of Phlogiston, it was not until the discovery of the gas Oxygen in the late 1700's that it was finally abandoned. Gaseous Oxygen was first produced by Carl Wilhelm Steele in 1774 when, as a result of the strong heating of the Red Calx of Mercury (Mercuric Oxide), the Calx decomposed into elemental Mercury and a gaseous substance now known as Oxygen. Antoine Lavoisier and Joseph Priestley were then able to show that Oxygen is a component of Air and is required for combustion and respiration. With these discoveries it was realized that Air supports combustion because of the presence of Oxygen. When Air is depleted of Oxygen, it no longer supports combustion. Material + Oxygen Oxide of the Material Although it seems as though the Theory of Phlogiston has merely been inverted, Oxygen is an isolatable substance, whereas Phlogiston is not. Additionally, all those inconvenient facts unexplainable by the Theory of Phlogiston suddenly become explainable by the presence and reactivity of Oxygen. Thus, as Ihde points out; "The phlogiston concept gradually disappeared as its elder adherents were removed from the scene by death." Lavoisier was able to show that Air that combined with elemental Mercury lost about 1/6 of its volume. In turn, he was able to regenerate this volume of gas by decomposing the Red Calx that formed. Thus, he reasoned, Air is approximately 1/6 Oxygen. We will do something similar in our determination of the Oxygen content of Air. We will combine Air with elemental Iron. In the presence of Water and an acid catalyst, the Oxygen in Air reacts with Iron to form a complex Hydrate: 2 Fe(s) + 3 O 2 (g) + x H 2 O Fe 2 O 3 xh 2 O(s) (Eq. 1) We must be careful not to use too much acid, however, because if the system is too acidic the Iron will react directly with the acid to form Hydrogen gas: Fe(s) + 2 H + (aq) Fe 2+ (aq) + H 2 (a) (Eq. 2) Thus, we will soak Steel Wool in a dilute aqueous solution of Acetic Acid and allow it to react with the Oxygen in Air. As it does this, the volume of the Air will contract. When complete, the
3 P a g e 3 volume lost by the Air will be equal to the volume Oxygen initially present. We will measure this volume lost by the Air by carrying out this reaction in an inverted test tube placed in a bath of Water. As the Oxygen is depleted from the Air and its volume contracts, Water will rush into the test tube to replace it. By measuring the volume of this Water, we will be measuring the volume of Oxygen in the Air. This method of measuring the volume of Oxygen in Air has one draw-back. The Air above the Water is Moist due to some Water Vapor that will be present in the gas. We can, however, correct for this by subtracting out the volume of the Air occupied by the Water Vapor. Thus, by applying an appropriate correction factor, we can determine the Volume Percentage Oxygen in Dry Air. We can then compare this determination with the accepted literature result.
4 P a g e 4 Pre-Lab Questions 1. Dry Air is reported to be 20.94% Oxygen. What is the Percentage Error in Lavoisier s determination? 2. Write a balanced chemical reaction for Scheele s method for producing Oxygen. 3. The word Oxygen is derived from the Greek word οξυγόνο. What is the meaning of this word and why was it selected as the name for Scheele s new gas?
5 P a g e 5 Procedure 1. Obtain two 20 x 150 test tubes without lips. Mark each tube, from the open end, using a wax pencil, every 0.5 cm for a total length of 6 cm. (You will use these markings to judge the rate of reaction by observing how fast Water fills the tube.) Arrange to clamp these tubes to a ring stand in an inverted position in a 1 L beaker filled with tap Water. 2. On an Analytical Balance, weigh out two ~0.5g pieces of fine Steel Wool (size 00). Do not compress the Wool. 3. In a fume hood, obtain 50mL Acetone, 50 ml of 1.0 M Acetic Acid and 50 ml 0.1 M Acetic Acid in 100 ml beakers. 4. Using forceps, in a fume hood, rinse one of the pieces of Wool in Acetone for about 30 seconds. This will remove any oil from the surface of the Steel Wool. Shake off the excess Acetone and drain it briefly on a paper towel. Do not compress the Steel Wool. 5. Transfer the Wool to the 1 M Acetic Acid. Agitate the Wool in the Acid for about 1 minute. This will help remove any Oxide coating from the Steel Wool and prepare the Wool s surface for reaction with Oxygen. Shake off the excess acid and drain the Wool briefly on a paper towel. Do not compress the Steel Wool. 6. Transfer the Wool to the 0.1 M Acetic Acid. Agitate the Wool in the Acid for about 30 seconds. Remove the Wool and shake it vigorously in the sink to remove as much of the acidic solution as possible. A small amount of this solution will remain adhered to the Wool s surface. This will provide the aqueous acidic solution required to catalyze the reaction between the Iron and the Oxygen. Do not compress the Steel Wool.
6 P a g e 6 7. Insert the Steel Wool into the bottom third of your test tube. Do not compress the Wool as you want as much surface area exposed to the Air as possible. 8. Invert the test tube and lower it into a water tank and clamp it into place. The mouth of the beaker must be below the level of the Water throughout the experiment. 9. At 5 minute intervals, note the level of the Water in the tube. Also, at some point during the reaction measure the temperature of the Water. We will take this temperature to be the temperature of the Air in the test tube. 10. Prepare a second sample of Wool for a second trial. Start the second trial while you are waiting for the first trial to be completed. 11. On a Top-Loading Balance, weigh a 250 ml beaker. 12. When the level of the Water in the test tube is no longer rising, wait 5 minutes longer and then adjust the height of the Water in the test tube such that it equals that of the Water in the beaker. (This will ensure the pressure of the gas in the tube is equal to that of the atmosphere. Think about why this is necessary in terms of Boyle s Law.) 13. Trap the Water in the test tube by firmly holding a large rubber stopper against the mouth of the tube while the mouth of the tube is still under Water. 14. Unclamp the test tube and remove it from the Water. Have your lab partner tap dry your hand, the stopper and the test tube. Quickly transfer the trapped Water to the weighed beaker. Re-weigh the beaker. 15. Using forceps remove the Steel Wool from the test tube and transfer it to the weighed beaker with the Water. Re-weigh the beaker and its contents. 16. Now, fill the test tube to the brim with Water. Add this to the beaker and re-weigh it. 17. Complete your second trial. 18. Measure the barometric pressure of the Atmosphere. When the level of the Water in the test tube is equal to the level of the Water in the beaker, the Atmospheric pressure is equal to the pressure of the gas in the tube.
7 P a g e 7 Data Analysis 1. Calculate the volume of Oxygen in the Moist Air from the mass of the Water trapped in the test tube. (Take the density of Water to be g/ml at Room Temperature.) Mass Water Trapped = Mass Step #14 Mass Step #11 2. Calculate the volume of the Steel Wool in the test tube from its initial mass. (Take the density of Steel Wool to be 7.70 g/ml.) Mass Steel Wool = Mass Step #2 3. Calculate the volume of the solution adhering to the Steel Wool. (Take the density of the adhering solution to be g/ml.) Mass Adhering Solution = Mass Step #15 - Mass Step #13 - Mass Step #2 4. Calculate the volume of the test tube from the mass of the Water that fills the test tube. (Take the density of Water to be g/ml at Room Temperature.) Mass Water in Full Tube = Mass Step #16 - Mass Step #15 5. Calculate the volume of the Air initially in the test tube. This will equal the volume of the test tube minus the volume of the Steel Wool and the volume of the adhering solution. Volume = Data Anal. Step #4 - Data Anal. Step #2 - Data Anal. Step #3 6. Calculate the percentage of Oxygen in the Moist Air. 7. Because the Air above the Water in the test tube contains some Water Vapor, we must correct this result to obtain the percentage Oxygen in Dry Air. Recall, the pressure of the gas in the test tube is equal to the barrometric pressure; P gas = P Barr. So, we need to subtract out the Vapor Pressure of Water P H2O and correct the % Oxygen in Moist Air according to: % Oxygen in Moist Air = % Oxygen in Dry Air x (P Barr - P H2O ) / P Barr Values for the Vapor Pressure of Water can be found in the Appendix. Calculate the percentage Oxygen in Dry Air. 8. Dry Air is reported to be 20.94% Oxygen. Calculate the percentage error for your determination.
8 P a g e 8
9 P a g e 9 Post Lab Questions 1. One of the inconvenient facts the Phlogistonists had to contend with was that metals were observed to increase in mass when they calcinate. Why was this fact inconvenient and how did the Phlogistonists explain it? 2. How would our results be affected if the solution adhering to the Steel Wool is too acidic and this resulted in the production of Hydrogen gas? 3. How many moles of Oxygen are contained in 10 ml of the pure gas at 25 o C and 1 atm pressure? How many grams of Iron is required to react with this much Oxygen?
10 P a g e 10 Appendix - Vapor Pressure and Density of Water Temp [ o C] Vapor Press [mmhg] Density [g/ml]
The Molar Mass of a Gas
The Molar Mass of a Gas Goals The purpose of this experiment is to determine the number of grams per mole of a gas by measuring the pressure, volume, temperature, and mass of a sample. Terms to Know Molar
More informationReaction of Magnesium with Hydrochloric Acid (Gas Laws) Chemicals Needed:
Reaction of Magnesium with Hydrochloric Acid (Gas Laws) Your Name: Date: Partner(s) Names: Objectives: React magnesium metal with hydrochloric acid, collecting the hydrogen over water. Calculate the grams
More informationMolar Mass of Butane
Cautions Butane is toxic and flammable. No OPEN Flames should be used in this experiment. Purpose The purpose of this experiment is to determine the molar mass of butane using Dalton s Law of Partial Pressures
More informationCSUS Department of Chemistry Experiment 8 Chem.1A
EXPERIMENT #8 Name: PRE-LABORATORY ASSIGNMENT: Lab Section 1. The alkali metals are so reactive that they react directly with water in the absence of acid. For example, potassium reacts with water as follows:
More informationDetermining Equivalent Weight by Copper Electrolysis
Purpose The purpose of this experiment is to determine the equivalent mass of copper based on change in the mass of a copper electrode and the volume of hydrogen gas generated during an electrolysis reaction.
More informationThe Empirical Formula of a Compound
The Empirical Formula of a Compound Lab #5 Introduction A look at the mass relationships in chemistry reveals little order or sense. The ratio of the masses of the elements in a compound, while constant,
More informationEXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor
EXPERIMENT 15: Ideal Gas Law: Molecular Weight of a Vapor Purpose: In this experiment you will use the ideal gas law to calculate the molecular weight of a volatile liquid compound by measuring the mass,
More informationEXPERIMENT 9 Evaluation of the Universal Gas Constant, R
Outcomes EXPERIMENT 9 Evaluation of the Universal Gas Constant, R After completing this experiment, the student should be able to: 1. Determine universal gas constant using reaction of an acid with a metal.
More informationMolar Mass and the Ideal Gas Law Prelab
Molar Mass and the Ideal Gas Law Prelab Name Total /10 SHOW ALL WORK NO WORK = NO CREDIT 1. What is the purpose of this experiment? 2. Determine the mass (in grams) of magnesium metal required to produce
More informationDETERMINING THE MOLAR MASS OF CARBON DIOXIDE
DETERMINING THE MOLAR MASS OF CARBON DIOXIDE PURPOSE: The goal of the experiment is to determine the molar mass of carbon dioxide and compare the experimentally determined value to the theoretical value.
More informationAustin Peay State University Department of Chemistry CHEM 1111. Empirical Formula of a Compound
Cautions Magnesium ribbon is flammable. Nitric acid (HNO 3 ) is toxic, corrosive and contact with eyes or skin may cause severe burns. Ammonia gas (NH 3 ) is toxic and harmful. Hot ceramic crucibles and
More informationAP CHEMISTRY 2009 SCORING GUIDELINES (Form B)
AP CHEMISTRY 2009 SCORING GUIDELINES (Form B) Question 3 (10 points) 2 H 2 O 2 (aq) 2 H 2 O(l) + O 2 (g) The mass of an aqueous solution of H 2 O 2 is 6.951 g. The H 2 O 2 in the solution decomposes completely
More informationGeneral Chemistry I (FC, 09-10) Lab #3: The Empirical Formula of a Compound. Introduction
General Chemistry I (FC, 09-10) Introduction A look at the mass relationships in chemistry reveals little order or sense. The ratio of the masses of the elements in a compound, while constant, does not
More informationWhere the exp subscripts refer to the experimental temperature and pressure acquired in the laboratory.
Molar Volume of Carbon Dioxide Reading assignment: Julia Burdge, Chemistry 3rd edition, Chapter 10. Goals To determine the molar volume of carbon dioxide gas and the amount of sodium carbonate in a sample.
More informationEXPERIMENT 7 Reaction Stoichiometry and Percent Yield
EXPERIMENT 7 Reaction Stoichiometry and Percent Yield INTRODUCTION Stoichiometry calculations are about calculating the amounts of substances that react and form in a chemical reaction. The word stoichiometry
More informationPREPARATION FOR CHEMISTRY LAB: COMBUSTION
1 Name: Lab Instructor: PREPARATION FOR CHEMISTRY LAB: COMBUSTION 1. What is a hydrocarbon? 2. What products form in the complete combustion of a hydrocarbon? 3. Combustion is an exothermic reaction. What
More informationChemistry 212 VAPOR PRESSURE OF WATER LEARNING OBJECTIVES
Chemistry 212 VAPOR PRESSURE OF WATER LEARNING OBJECTIVES The learning objectives of this experiment are to explore the relationship between the temperature and vapor pressure of water. determine the molar
More informationLaboratory Exercise: Smelting of Lead
CHEM 109 Introduction to Chemistry Revision 1.0 Laboratory Exercise: Smelting of Lead In this laboratory exercise we will carry out a pyrometallurgical conversion of Lead Oxide into elemental Lead. This
More informationChemistry 101 Generating Hydrogen Gas
Chemistry 101 Generating Hydrogen Gas Objectives To experimentally verify the molar volume of hydrogen gas at STP To gain experience in collecting gas over water Discussion The molar volume of a gas is
More informationOxygen Give and Take. Correlation to National Science Education Standards
Chemistry and Environmental Sciences Oxygen Give and Take Summary This is a series of three activities followed by a worksheet. The concepts taught include gas production (O 2 and CO 2 ), chemical reactions,
More informationEXPERIMENT 13: GAS STOICHIOMETRY
EXPERIMENT 13: GAS STOICHIOMETRY PURPOSE To collect a gas produced in a reaction and compare the volume actually collected to a "target volume". To discover and compensate for assumptions made in the stoichiometric
More informationExperiment 6 Coffee-cup Calorimetry
6-1 Experiment 6 Coffee-cup Calorimetry Introduction: Chemical reactions involve the release or consumption of energy, usually in the form of heat. Heat is measured in the energy units, Joules (J), defined
More informationExperiment 3 Limiting Reactants
3-1 Experiment 3 Limiting Reactants Introduction: Most chemical reactions require two or more reactants. Typically, one of the reactants is used up before the other, at which time the reaction stops. The
More informationChemistry 112 Laboratory Experiment 6: The Reaction of Aluminum and Zinc with Hydrochloric Acid
Chemistry 112 Laboratory Experiment 6: The Reaction of Aluminum and Zinc with Hydrochloric Acid Introduction Many metals react with acids to form hydrogen gas. In this experiment, you will use the reactions
More informationDETERMINING THE ENTHALPY OF FORMATION OF CaCO 3
DETERMINING THE ENTHALPY OF FORMATION OF CaCO 3 Standard Enthalpy Change Standard Enthalpy Change for a reaction, symbolized as H 0 298, is defined as The enthalpy change when the molar quantities of reactants
More informationEXPERIMENT 12: Empirical Formula of a Compound
EXPERIMENT 12: Empirical Formula of a Compound INTRODUCTION Chemical formulas indicate the composition of compounds. A formula that gives only the simplest ratio of the relative number of atoms in a compound
More informationPre-Lab Notebook Content: Your notebook should include the title, date, purpose, procedure; data tables.
Determination of Molar Mass by Freezing Point Depression M. Burkart & M. Kim Experimental Notes: Students work in pairs. Safety: Goggles and closed shoes must be worn. Dispose of all chemical in the plastic
More information1. The Determination of Boiling Point
1. The Determination of Boiling Point Objective In this experiment, you will first check your thermometer for errors by determining the temperature of two stable equilibrium systems. You will then use
More informationPhysical Properties of a Pure Substance, Water
Physical Properties of a Pure Substance, Water The chemical and physical properties of a substance characterize it as a unique substance, and the determination of these properties can often allow one to
More informationExperiment 8 Synthesis of Aspirin
Experiment 8 Synthesis of Aspirin Aspirin is an effective analgesic (pain reliever), antipyretic (fever reducer) and anti-inflammatory agent and is one of the most widely used non-prescription drugs. The
More informationHonors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C-4.4)
Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1 1. 2. 3. 4. 5. 6. Question What is a symbolic representation of a chemical reaction? What 3 things (values) is a mole of a chemical
More informationPhysical and Chemical Properties and Changes
Physical and Chemical Properties and Changes An understanding of material things requires an understanding of the physical and chemical characteristics of matter. A few planned experiments can help you
More informationOxidation States of Copper Two forms of copper oxide are found in nature, copper(i) oxide and copper(ii) oxide.
The Empirical Formula of a Copper Oxide Reading assignment: Chang, Chemistry 10 th edition, pp. 55-58. Goals The reaction of hydrogen gas with a copper oxide compound will be studied quantitatively. By
More informationThe Synthesis of trans-dichlorobis(ethylenediamine)cobalt(iii) Chloride
CHEM 122L General Chemistry Laboratory Revision 2.0 The Synthesis of trans-dichlorobis(ethylenediamine)cobalt(iii) Chloride To learn about Coordination Compounds and Complex Ions. To learn about Isomerism.
More informationexperiment5 Understanding and applying the concept of limiting reagents. Learning how to perform a vacuum filtration.
81 experiment5 LECTURE AND LAB SKILLS EMPHASIZED Synthesizing an organic substance. Understanding and applying the concept of limiting reagents. Determining percent yield. Learning how to perform a vacuum
More informationCatalase. ***You will be working with hot water, acids and bases in this laboratory*** ****Use Extreme Caution!!!****
AP BIOLOGY BIOCHEMISTRY ACTIVITY #9 NAME DATE HOUR CATALASE LAB INTRODUCTION Hydrogen peroxide (H 2 O 2 ) is a poisonous byproduct of metabolism that can damage cells if it is not removed. Catalase is
More informationMeasurement and Calibration
Adapted from: H. A. Neidig and J. N. Spencer Modular Laboratory Program in Chemistry Thompson Learning;, University of Pittsburgh Chemistry 0110 Laboratory Manual, 1998. Purpose To gain an understanding
More informationMicro Mole Rockets Hydrogen and Oxygen Mole Ratio As adapted from Flinn ChemTopic- Labs - Molar Relationships & Stoichiometry
Micro Mole Rockets Hydrogen and Oxygen Mole Ratio As adapted from Flinn ChemTopic- Labs - Molar Relationships & Stoichiometry Introduction The combustion reaction of hydrogen and oxygen is used to produce
More informationSUPPLEMENTARY MATERIAL
SUPPLEMENTARY MATERIAL (Student Instructions) Determination of the Formula of a Hydrate A Greener Approach Objectives To experimentally determine the formula of a hydrate salt. To learn to think in terms
More informationIn this experiment, we will use three properties to identify a liquid substance: solubility, density and boiling point..
Identification of a Substance by Physical Properties 2009 by David A. Katz. All rights reserved. Permission for academic use provided the original copyright is included Every substance has a unique set
More informationTemperature. Number of moles. Constant Terms. Pressure. Answers Additional Questions 12.1
Answers Additional Questions 12.1 1. A gas collected over water has a total pressure equal to the pressure of the dry gas plus the pressure of the water vapor. If the partial pressure of water at 25.0
More informationExperiment 7: Titration of an Antacid
1 Experiment 7: Titration of an Antacid Objective: In this experiment, you will standardize a solution of base using the analytical technique known as titration. Using this standardized solution, you will
More informationUnit 6 The Mole Concept
Chemistry Form 3 Page 62 Ms. R. Buttigieg Unit 6 The Mole Concept See Chemistry for You Chapter 28 pg. 352-363 See GCSE Chemistry Chapter 5 pg. 70-79 6.1 Relative atomic mass. The relative atomic mass
More informationAN EXPERIMENT IN ALCHEMY: COPPER TO SILVER TO GOLD 2005, 2000, 1996 by David A. Katz. All rights reserved
AN EXPERIMENT IN ALCHEMY: COPPER TO SILVER TO GOLD 2005, 2000, 1996 by David A. Katz. All rights reserved INTRODUCTION One of the goals of the ancient alchemists was to convert base metals into gold. Although
More informationExperiment 8 Preparation of Cyclohexanone by Hypochlorite Oxidation
Experiment 8 Preparation of Cyclohexanone by ypochlorite xidation In this experiment we will prepare cyclohexanone from cyclohexanol using hypochlorite oxidation. We will use common household bleach that
More informationTransfer of heat energy often occurs during chemical reactions. A reaction
Chemistry 111 Lab: Thermochemistry Page I-3 THERMOCHEMISTRY Heats of Reaction The Enthalpy of Formation of Magnesium Oxide Transfer of heat energy often occurs during chemical reactions. A reaction may
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Chapter 10 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A gas at a pressure of 10.0 Pa exerts a force of N on an area of 5.5 m2. A) 1.8 B) 0.55
More information7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.
CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,
More informationExperiment 9: Acids and Bases Adapted from: Chemistry, Experimental Foundations, 4th Ed. Laboratory Manual, by Merrill, Parry & Bassow.
Chem 121 Lab Clark College Experiment 9: Acids and Bases Adapted from: Chemistry, Experimental Foundations, 4th Ed. Laboratory Manual, by Merrill, Parry & Bassow. Content Goals: Increase understanding
More informationEnzyme Action: Testing Catalase Activity 50 Points
Names: LabQuest Enzyme Action: Testing Catalase Activity 50 Points 6A Many organisms can decompose hydrogen peroxide (H 2 O 2 ) enzymatically. Enzymes are globular proteins, responsible for most of the
More informationCalibration of Volumetric Glassware
CHEM 311L Quantitative Analysis Laboratory Revision 2.3 Calibration of Volumetric Glassware In this laboratory exercise, we will calibrate the three types of glassware typically used by an analytical chemist;
More informationExtraction: Separation of Acidic Substances
Extraction: Separation of Acidic Substances Chemists frequently find it necessary to separate a mixture of compounds by moving a component from one solution or mixture to another. The process most often
More informationCHEM 105 HOUR EXAM III 28-OCT-99. = -163 kj/mole determine H f 0 for Ni(CO) 4 (g) = -260 kj/mole determine H f 0 for Cr(CO) 6 (g)
CHEM 15 HOUR EXAM III 28-OCT-99 NAME (please print) 1. a. given: Ni (s) + 4 CO (g) = Ni(CO) 4 (g) H Rxn = -163 k/mole determine H f for Ni(CO) 4 (g) b. given: Cr (s) + 6 CO (g) = Cr(CO) 6 (g) H Rxn = -26
More informationMaterials 10-mL graduated cylinder l or 2-L beaker, preferably tall-form Thermometer
VAPOR PRESSURE OF WATER Introduction At very low temperatures (temperatures near the freezing point), the rate of evaporation of water (or any liquid) is negligible. But as its temperature increases, more
More informationMixtures and Pure Substances
Unit 2 Mixtures and Pure Substances Matter can be classified into two groups: mixtures and pure substances. Mixtures are the most common form of matter and consist of mixtures of pure substances. They
More informationProblem Solving. Stoichiometry of Gases
Skills Worksheet Problem Solving Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations.
More informationDetermination of the Empirical Formula of Magnesium Oxide
Determination of the Empirical Formula of Magnesium Oxide GOAL AND OVERVIEW The quantitative stoichiometric relationships governing mass and amount will be studied using the combustion reaction of magnesium
More informationPaper Chromatography: Separation and Identification of Five Metal Cations
Paper Chromatography: Separation and Identification of Five Metal Cations Objectives Known and unknown solutions of the metal ions Ag +, Fe 3+, Co 2+, Cu 2+ and Hg 2+ will be analyzed using paper chromatography.
More informationEnzyme Action: Testing Catalase Activity
Enzyme Action: Testing Catalase Activity Experiment 6A Many organisms can decompose hydrogen peroxide (H 2 O 2 ) enzymatically. Enzymes are globular proteins, responsible for most of the chemical activities
More informationExperiment 1: Measurement and Density
Experiment 1: Measurement and Density Chemistry 140 Learning Objectives Become familiar with laboratory equipment and glassware Begin to see the link between measurement and chemical knowledge Begin to
More informationEnzyme Action: Testing Catalase Activity
Enzyme Action: Testing Catalase Activity Experiment 6A Many organisms can decompose hydrogen peroxide (H 2 O 2 ) enzymatically. Enzymes are globular proteins, responsible for most of the chemical activities
More informationBLOWING UP BALLOONS, chemically
BLOWING UP BALLOONS, chemically PRE LAB DISCUSSION: Today we will be using a closed system. A closed system does not permit matter to enter or exit the apparatus. Lavoisier's classic 12-day experiment,
More informationDYES AND DYEING 2003 by David A. Katz. All rights reserved. Permission for classroom use provided original copyright is included.
DYES AND DYEING 2003 by David A. Katz. All rights reserved. Permission for classroom use provided original copyright is included. Dyeing of textiles has been practiced for thousands of years with the first
More informationBuilding Electrochemical Cells
Cautions Heavy metals, such as lead, and solutions of heavy metals may be toxic and an irritant. Purpose To determine the cell potential (E cell ) for various voltaic cells and compare the data with the
More informationSEPARATION OF A MIXTURE OF SUBSTANCES LAB
SEPARATION OF A MIXTURE OF SUBSTANCES LAB Purpose: Every chemical has a set of defined physical properties, and when combined they present a unique fingerprint for that chemical. When chemicals are present
More informationCHM220 Addition lab. Experiment: Reactions of alkanes, alkenes, and cycloalkenes*
CM220 Addition lab Experiment: Reactions of alkanes, alkenes, and cycloalkenes* Purpose: To investigate the physical properties, solubility, and density of some hydrocarbon. To compare the chemical reactivity
More informationMeasuring volume of gas produced Measuring precipitation (because sulphur is produced) e.g. look for X to disappear Measure mass lost
Introduction My investigation is about the rate of reaction. A rate of reaction is defined as how fast or slow a reaction takes place. For example, the oxidation of iron under the atmosphere is a slow
More informationDetermination of Molar Mass by Boiling Point Elevation of Urea Solution
Determination of Molar Mass by Boiling Point Elevation of Urea Solution CHRISTIAN E. MADU, PhD AND BASSAM ATTILI, PhD COLLIN COLLEGE CHEMISTRY DEPARTMENT Purpose of the Experiment Determine the boiling
More informationSynthesis of Aspirin and Oil of Wintergreen
Austin Peay State University Department of hemistry hem 1121 autions Purpose Introduction Acetic Anhydride corrosive and a lachrymator all transfers should be done in the vented fume hood Methanol, Ethanol
More informationCHEMICAL REACTIONS OF COPPER AND PERCENT YIELD KEY
CHEMICAL REACTIONS OF COPPER AND PERCENT YIELD Objective To gain familiarity with basic laboratory procedures, some chemistry of a typical transition element, and the concept of percent yield. Apparatus
More informationChapter 3 Student Reading
Chapter 3 Student Reading If you hold a solid piece of lead or iron in your hand, it feels heavy for its size. If you hold the same size piece of balsa wood or plastic, it feels light for its size. The
More informationCatalytic Activity of Enzymes
Catalytic Activity of Enzymes Introduction Enzymes are biological molecules that catalyze (speed up) chemical reactions. You could call enzymes the Builders and Do-ers in the cell; without them, life could
More informationDesalination of Sea Water E7-1
Experiment 7 Desalination of Sea Water E7-1 E7-2 The Task The goal of this experiment is to investigate the nature and some properties of sea water. Skills At the end of the laboratory session you should
More informationPartner: Jack 17 November 2011. Determination of the Molar Mass of Volatile Liquids
Partner: Jack 17 November 2011 Determination of the Molar Mass of Volatile Liquids Purpose: The purpose of this experiment is to determine the molar mass of three volatile liquids. The liquid is vaporized
More informationPhysical Changes and Chemical Reactions
Physical Changes and Chemical Reactions Gezahegn Chaka, Ph.D., and Sudha Madhugiri, Ph.D., Collin College Department of Chemistry Objectives Introduction To observe physical and chemical changes. To identify
More informationVitamin C Content of Fruit Juice
1 Vitamin C Content of Fruit Juice Introduction Vitamin C Vitamins are organic compounds that have important biological functions. For instance, in humans they enable a variety of enzymes in the body to
More informationPreparation of an Alum
Preparation of an Alum Pages 75 84 Pre-lab = pages 81 to 82, all questions No lab questions, a lab report is required by the start of the next lab What is an alum? They are white crystalline double sulfates
More informationRecovery of Elemental Copper from Copper (II) Nitrate
Recovery of Elemental Copper from Copper (II) Nitrate Objectives: Challenge: Students should be able to - recognize evidence(s) of a chemical change - convert word equations into formula equations - perform
More informationExperiment 13H THE REACTION OF RED FOOD COLOR WITH BLEACH 1
Experiment 13H FV 1/25/2011(2-run) THE REACTION OF RED FOOD COLOR WITH BLEACH 1 PROBLEM: Determine the rate law for the chemical reaction between FD&C Red Dye #3 and sodium hypochlorite. LEARNING OBJECTIVES:
More informationHEAT OF FORMATION OF AMMONIUM NITRATE
303 HEAT OF FORMATION OF AMMONIUM NITRATE OBJECTIVES FOR THE EXPERIMENT The student will be able to do the following: 1. Calculate the change in enthalpy (heat of reaction) using the Law of Hess. 2. Find
More informationKinetic Theory of Gases. 6.1 Properties of Gases 6.2 Gas Pressure. Properties That Describe a Gas. Gas Pressure. Learning Check.
Chapter 6 Gases Kinetic Theory of Gases 6.1 Properties of Gases 6.2 Gas Pressure A gas consists of small particles that move rapidly in straight lines. have essentially no attractive (or repulsive) forces.
More informationPercentage of Water in Popcorn
Skills Practice DATASHEET FOR IN-TEXT LAB Percentage of Water in Popcorn Popcorn pops because of the natural moisture inside each kernel. When the internal water is heated above 100 C, the liquid water
More informationMaking Biodiesel from Virgin Vegetable Oil: Teacher Manual
Making Biodiesel from Virgin Vegetable Oil: Teacher Manual Learning Goals: Students will understand how to produce biodiesel from virgin vegetable oil. Students will understand the effect of an exothermic
More informationTo measure the solubility of a salt in water over a range of temperatures and to construct a graph representing the salt solubility.
THE SOLUBILITY OF A SALT IN WATER AT VARIOUS TEMPERATURES 2007, 1995, 1991 by David A. Katz. All rights reserved. Permission for academic use provided the original copyright is included. OBJECTIVE To measure
More informationPRE-LAB FOR YEAST RESPIRATION AND FERMENTATION
PRE-LAB FOR YEAST RESPIRATION AND FERMENTATION PURPOSE: To identify the products of yeast cultures grown under aerobic and anaerobic conditions STUDENTS' ENTERING COMPETENCIES: Before doing this lab, students
More informationThe volume of a penny will be calculated from its mass and density.
Measurement and Density In science a key concern is the quantities involved in chemical processes. These amounts can be directly measured or calculated from other measurements. A measurement consists of
More informationDistillation of Alcohol
CHEM 121L General Chemistry Laboratory Revision 1.6 Distillation of Alcohol To learn about the separation of substances. To learn about the separation technique of distillation. To learn how to characterize
More informationDetermination of a Chemical Formula
1 Determination of a Chemical Formula Introduction Molar Ratios Elements combine in fixed ratios to form compounds. For example, consider the compound TiCl 4 (titanium chloride). Each molecule of TiCl
More informationChemical Equations & Stoichiometry
Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term
More informationCHEM 36 General Chemistry EXAM #1 February 13, 2002
CHEM 36 General Chemistry EXAM #1 February 13, 2002 Name: Serkey, Anne INSTRUCTIONS: Read through the entire exam before you begin. Answer all of the questions. For questions involving calculations, show
More informationWhoosh Bottle Safe Laboratory Practices
E-Learning Introduction Whoosh Bottle Safe Laboratory Practices Teach essential safety precautions relative to combustion, flammability, and the fire triangle. Publication No. 95010 Concepts Flammable
More informationChapter 8 - Chemical Equations and Reactions
Chapter 8 - Chemical Equations and Reactions 8-1 Describing Chemical Reactions I. Introduction A. Reactants 1. Original substances entering into a chemical rxn B. Products 1. The resulting substances from
More informationH H H O. Pre-Lab Exercises Lab 6: Organic Chemistry. Lab 6: Organic Chemistry Chemistry 100. 1. Define the following: a.
Lab 6: Organic hemistry hemistry 100 1. Define the following: a. ydrocarbon Pre-Lab Exercises Lab 6: Organic hemistry Name Date Section b. Saturated hydrocarbon c. Unsaturated hydrocarbon 2. The formula
More informationRajesh Swaminathan. March 13, 2005
Chemistry 12 IB Corrosion of Iron Rajesh Swaminathan March 13, 2005 1 Planning A 1.1 Aim The aim of the experiment is to investigate factors that affect the rate of corrosion of iron. More specifically,
More informationIB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
More informationSugar or Salt? Ionic and Covalent Bonds
Lab 11 Sugar or Salt? Ionic and Covalent Bonds TN Standard 2.1: The student will investigate chemical bonding. Have you ever accidentally used salt instead of sugar? D rinking tea that has been sweetened
More informationModule 5: Combustion Technology. Lecture 34: Calculation of calorific value of fuels
1 P age Module 5: Combustion Technology Lecture 34: Calculation of calorific value of fuels 2 P age Keywords : Gross calorific value, Net calorific value, enthalpy change, bomb calorimeter 5.3 Calculation
More informationPHYSICAL SEPARATION TECHNIQUES. Introduction
PHYSICAL SEPARATION TECHNIQUES Lab #2 Introduction When two or more substances, that do not react chemically, are blended together, the result is a mixture in which each component retains its individual
More informationMetalloids will also react with oxygen. Upon reaction with oxygen silicon forms silicon dioxide, the main component of sand.
The Preparation and Properties of xygen Reading assignment: Chang, Chemistry 10 th edition, pp. 135-141. Goals We will observe the thermal decomposition of several oxygen-containing compounds called oxides.
More informationSOLUBILITY OF A SALT IN WATER AT VARIOUS TEMPERATURES LAB
SOLUBILITY OF A SALT IN WATER AT VARIOUS TEMPERATURES LAB Purpose: Most ionic compounds are considered by chemists to be salts and many of these are water soluble. In this lab, you will determine the solubility,
More information