How To Use A Bomb Calorimeter
|
|
- Milton Goodwin
- 3 years ago
- Views:
Transcription
1 University of Lethbridge Chemistry 2740 Laboratory Department of Chemistry & Biochemistry COMBUSTION CALORIMETRY Required materials In this experiment, you will obtain the combustion energy of a food product. Each group must bring to the laboratory one food. Given the equipment currently available in the Department, some foods cannot be studied. The sample must fit into a small sample cup (about 2 cm across) and you need a single piece with a mass of about 1 g. Chocolate is an example of a food that can easily be cut into appropriate pieces. Nuts and coated candies (M&M s, etc.) are often of a roughly appropriate size and can be studied directly. Other foods may be suitable if they can be formed into a pellet with equipment available in the lab. Most breakfast cereals can be pelletized since they have components that make them slightly sticky. Many dry goods (flour, starch, sugar) would almost certainly also work out. On the other hand, pasta and rice are too dry. Foods with an extremely high fluid content (soft drinks, jams, many fruits) must be desiccated before use and so require prior arrangement with the instructor. Although you only need one food item, it is recommended that each group member bring a different food, just in case technical difficulties get in the way of your first choice. Nonfood items which have appropriate chemical and mechanical properties and whose combustion is of interest (wood, coal, etc.) may be studied instead of a foodstuff if desired. However, it may be necessary to study smaller samples than recommended below for some materials so consult the instructor before proceeding. Theory The bomb calorimeter to be used in this experiment is a constant volume device. Accordingly, it measures changes in internal energy. It is an almost adiabatic device. Hence, if a reaction is carried out within it, we have ΔEtotal = 0 = ΔEreaction + q (1) or q = -ΔEreaction where ΔEreaction is the change in internal energy in the reaction and q is the heat released. Page 3-1
2 The heat released is related to the heat capacity of the system by q = CVΔT (2) The calorimeter is operated while containing both the bomb and a quantity of water whose total heat capacity is much larger than that of the products of the reaction. CV can therefore be taken to be a constant for a given calorimeter filled with a given amount of water. Enthalpy and internal energy are related by H = E + PV (3) so that ΔH = ΔE + Δ(PV) (4) Solids and liquids have small volumes and low compressibilities so that their appearance or disappearance during a chemical reaction has little effect on the product PV. Gases on the other hand have large volumes. Most gases behave at least approximately like an ideal gas so that we can use PV nrt (5) Bomb calorimeters are also operated in such a way that the overall temperature change is small, typically 2 5 K. The only thing that can change significantly in the right-hand side of the above equation is therefore the number of moles of gas. Combining this with equation 1, we get ΔH = ΔE + RTΔngas (6) Page 3-2
3 Safety and equipment handling You will be using high pressures of oxygen. High concentrations of oxygen can promote combustion so be on the lookout for sources of sparks in your immediate working area. Also be on the lookout for leaks in the equipment. Highly pressurized gases apply large forces to their containers so be careful to follow the instructions below closely to avoid launching dangerous projectiles across the lab. Use a blast shield to protect yourself during the pressurization of the bomb and when the sample is ignited in the calorimeter. Many parts of the calorimeter are electrically live when the ignition switch is pressed so leave the ignition unit unplugged until needed, then unplug it immediately after ignition to minimize shock hazards. The bomb looks sturdy, but it is a precision-built device that can be ruined by careless use. Be particularly careful not to scratch or dent any surfaces involved in sealing the bomb (screws, seals, etc.). The bomb is designed to be closed by hand. Do not use any tools on any part of the bomb. The bomb should never be cleaned with anything but water. The ignition switch is designed to deliver just the right amount of power to ignite a 10 cm fuse wire. Do not use a longer piece. The thermometer provided is a very expensive precision instrument. Be careful with it. The equipment must be carefully cleaned and dried after the experiment to keep it in proper operating condition. Page 3-3
4 Procedure Figure 1. A view of one of our bombs and of a section of the calorimeter. 1. Figure 1 shows a view of one of our bombs and of a section of the calorimeter. Our second bomb is similar in design but has two valves instead of just one. All the equipment should be clean and dry when you get it, but check the following before starting: a. The inside of the calorimeter is reasonably clean. b. The bucket and bomb are thoroughly dry. c. There are no bits of fuse wire attached to the terminals of the bomb. d. You have at least two reasonably clean and dry sample cups. 2. You will begin by calibrating the calorimeter with benzoic acid. Weigh a benzoic Page 3-4
5 acid pellet into a sample cup. (All weights are to be obtained on a balance that can be read at least to a tenth of a milligram.) Also weigh a 10 cm length of fuse wire. Note the (constant volume) heat of combustion of the fuse wire, which is given on the bobbin. Combustion of the fuse wire is exothermic so make sure to get the sign right. 3. Place the cup in the bomb head and attach the fuse wire. The fuse wire should be wrapped tightly two or three complete turns around each terminal. It must be in good contact with the sample but must not touch the sample cup. This is extremely tricky but take the time to do it right. If you don t, the calorimeter will misfire and you will have to start all over again. The easiest way to do this is to first crimp the wire as shown in Figure 2. Once the sample and fuse are in proper position, handle the bomb head carefully as you do not want to disturb the contact of fuse to sample. Figure 2. Crimping of the fuse wire. 4. Put the bomb head carefully into the bomb body. Screw the cap down tightly. 5. You will now flush the bomb with oxygen before filling it. Take the bomb to the oxygen filling station. Arrange things so that you can stand behind a blast shield while filling the bomb. With the bomb shown in Figure 1, remove the venting nut and attach the oxygen filling fitting in its place. For the bomb with two valves, tightly close the pressure-relief needle valve and attach the oxygen filling fitting to the self-sealing valve. Standing behind the blast shield, open the main cylinder valve. Open the supply valve and let the bomb fill slowly to a pressure of 20 atm. Note that when you stop, the pressure gauge will immediately start to drop. This is not an indication of a leak in the system so don t worry. After closing the supply valve, release the pressure in the line with the lever located just below the valve. Remove the oxygen filling fitting. Vent the bomb either by opening the needle venting valve (two-valve design) or by screwing the venting nut on about halfway, then pressing on it (one-valve design). 6. You will now fill the bomb with 20 atm of oxygen. The steps are identical to those above and must be carried out with the same care and caution. At the end however, Page 3-5
6 you screw the venting nut down tightly if using the one-valve bomb. 7. Verify that the ignition switch is unplugged. Put the bucket in the calorimeter and the bomb in the bucket. Plug the ignition lead into the bomb s external terminal post. Using a volumetric flask, add 2 L of distilled water to the bucket. Be careful to pour all the water into the bucket. 8. This calorimeter allows bubbles to come out of the bomb at a fairly steady rate. Despite this, there is more than enough oxygen in the bomb to ensure that this experiment still works. 9. Close the calorimeter, install the thermometer, and start the stirrer. Record the temperature every 30 s for 5 min. For optimal precision, use a telescope to read the thermometer. 10. Place the blast shield between you and the bomb. Plug in the ignition switch. To ignite the sample, you simply press the ignition switch. If all goes well, a red pilot light will come on for a second or so. As soon as the light goes out, release the switch. Record the time of ignition. If the light does not go off within 5 s, there is a short circuit somewhere in your system. Unplug the ignition switch, remove the bomb, vent it, dump out the bucket, dry everything, check the fuse, and go back to step Unplug the ignition switch. Remove the blast shield and start recording the temperature again at 30 s intervals. If the temperature does not rise significantly during the first minute or so, the bomb misfired. Remove the bomb, vent it, dump out the bucket, dry everything, check the fuse and sample, and start over. 12. Continue recording the temperature until the readings level off or the slope becomes constant for 5 min (generally about 10 min observation time post-ignition). 13. Remove the bomb and vent it. Open it up. Make sure that the sample has completely burned. If it hasn t, start over. (This is unlikely if everything else went well.) There will generally be some fuse wire left on the terminals. Carefully remove and weigh these pieces of fuse. Page 3-6
7 14. Clean the sample cup and terminals. Thoroughly dry everything. 15. Repeat with your food sample (pelletized if necessary). 16. When you are finished, leave the bomb completely disassembled, clean and dry. Analysis The most tedious part of the analysis of calorimeter data is determining ΔT. Both the pre-ignition and post-ignition data should have a linear section. You want to extrapolate these linear sections to the time of ignition. Figure 3 illustrates the procedure. Figure 3. Extrapolation of the linear sections of calorimeter data to the time of ignition. Before leaving the laboratory, please enter names, date, and experimental data into the computer. Page 3-7
8 Calculations and Report Remembering that qtotal for each run is equal to the heat released by what was in the cup plus the heat released by the amount of wire combusted, calculate CV for your experiment and use it to calculate the specific combustion energy of your food sample. Calculate the combustion energy per gram for your sample and compare that value to the literature or label value. Remember that nutritional calories (Cal) are equivalent to kcal. Page 3-8
Enthalpy of Combustion via Calorimetry
Enthalpy of Combustion via Calorimetry Introduction This experiment measures the enthalpy change when a system consisting of a known amount of a substance in the presence of excess oxygen is quantitatively
More informationAdiabatic Bomb Calorimetry
CHEM 366 II-1 Adiabatic Bomb Calorimetry Introduction Obtaining energy in the form of heat from the combustion or oxidation of thermodynamically unstable (and often kinetically inert) hydrocarbons and
More informationExperiment 1: Adiabatic Bomb Calorimeter (Dated: September 27, 2010)
Experiment 1: Adiabatic Bomb Calorimeter (Dated: September 27, 2010) I. INTRODUCTION Heat released in a chemical reaction can be determined experimentally by using an adiabatic calorimeter. The reaction
More informationIntroductory Laboratory EST - Experiment 9 Calorimetry - 1 - Introductory Laboratory Energy Science and Technology. Experiment 9. Physical Chemistry
Introductory Laboratory EST - Experiment 9 Calorimetry - 1 - Introductory Laboratory Energy Science and Technology Experiment 9 Physical Chemistry Calorimetry Abstract The heat of combustion of Naphthalene
More informationCombustion Calorimetry
ombustion alorimetry 1 Please Note: Each lab group will be required to pick the compound they use in this experiment. The compound must contain only carbon and hydrogen or carbon, hydrogen and oxygen.
More informationHeat of Combustion PCh 6-99
UMR ChemLabs Heat of Combustion PCh 6-99 Gary L. Bertrand, Professor of Chemistry A calorimeter (calor L = heat + metron Gr = measure) should be literally a device to measure heat. In reality, most calorimeters
More informationThermochemistry: Calorimetry and Hess s Law
Thermochemistry: Calorimetry and Hess s Law Some chemical reactions are endothermic and proceed with absorption of heat while others are exothermic and proceed with an evolution of heat. The magnitude
More informationHEAT OF COMBUSTION BY OXYGEN BOMB CALORIMETER. References: See relevant chapters in undergraduate text.
HEAT OF COMBUSTION BY OXYGEN BOMB CALORIMETER References: See relevant chapters in undergraduate text. Background: Study text sections on calorimetry and "thermochemistry" carefully. Know definitions of
More informationBomb Calorimetry. Electrical leads. Stirrer
Bomb Calorimetry Stirrer Electrical leads Oxygen inlet valve Bomb Fuse Calorimeter Outer jacket Not shown: heating and cooling system for outer jacket, and controls that keep the outer jacket at the same
More informationBomb Calorimetry and Heat of Combustion
UC Berkeley College of Chemistry Chemistry 125 Physical Chemistry Laboratory Bomb Calorimetry and Heat of Combustion Author: Jonathan Melville Collaborators: David Gygi and Effie Zhou Graduate Student
More informationDetermination of the enthalpy of combustion using a bomb calorimeter TEC
Determination of the enthalpy of TEC Related concepts First law of thermodynamics, Hess s law of constant heat summation, enthalpy of combustion, enthalpy of formation, heat capacity. Principle The bomb
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 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 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 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 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 informationCOMMON LABORATORY APPARATUS
COMMON LABORATORY APPARATUS Beakers are useful as a reaction container or to hold liquid or solid samples. They are also used to catch liquids from titrations and filtrates from filtering operations. Bunsen
More informationDetermination of the enthalpy of combustion using a bomb calorimeter TEC. Safety precautions
Safety precautions Naphthalene is harmful if swallowed. May cause cancer. Is further very toxic to aquatic organisms and can have long-term harmful effects in bodies of water. Equipment 1 Bomb calorimeter
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 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 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 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 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 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 informationThe 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 informationHands-On Labs SM-1 Lab Manual
EXPERIMENT 4: Separation of a Mixture of Solids Read the entire experiment and organize time, materials, and work space before beginning. Remember to review the safety sections and wear goggles when appropriate.
More informationPhys222 W11 Quiz 1: Chapters 19-21 Keys. Name:
Name:. In order for two objects to have the same temperature, they must a. be in thermal equilibrium.
More informationBurn Baby Burn: The Power Within! Feedstock Calorimetry. (by Mary C. Criss & Shannon Ralph)
Burn Baby Burn: The Power Within! Feedstock Calorimetry (by Mary C. Criss & Shannon Ralph) Objective The purpose of this experiment is to determine the amount of chemical energy stored in different biofuel
More informationEXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES
Name Section EXPERIMENT 13: THE IDEAL GAS LAW AND THE MOLECULAR WEIGHT OF GASES PRE-LABORATORY QUESTIONS The following preparatory questions should be answered before coming to lab. They are intended to
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 informationEXPERIMENT 4 THE DETERMINATION OF THE CALORIC CONTENT OF A CASHEW NUT
EXPERIMENT 4 THE DETERMINATION OF THE CALORIC CONTENT OF A CASHEW NUT Textbook reference: pp103-105 Purpose: In this Activity, students determine how many calories are released per gram when cashews burn
More informationApparatus error for each piece of equipment = 100 x margin of error quantity measured
1) Error Analysis Apparatus Errors (uncertainty) Every time you make a measurement with a piece of apparatus, there is a small margin of error (i.e. uncertainty) in that measurement due to the apparatus
More informationPHOTOSYNTHESIS AND RESPIRATION
PHOTOSYNTHESIS AND RESPIRATION STANDARDS: 3.2.10.B.3, 3.2.10.C.4 3.3.10.B.4 Westminster College INTRODUCTION Plants make sugar, storing the energy of the sun as chemical energy, by the process of photosynthesis.
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 informationChemical Changes. Measuring a Chemical Reaction. Name(s)
Chemical Changes Name(s) In the particle model of matter, individual atoms can be bound tightly to other atoms to form molecules. For example, water molecules are made up of two hydrogen atoms bound to
More informationIDEAL AND NON-IDEAL GASES
2/2016 ideal gas 1/8 IDEAL AND NON-IDEAL GASES PURPOSE: To measure how the pressure of a low-density gas varies with temperature, to determine the absolute zero of temperature by making a linear fit to
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 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 informationThe Great Peanut Problem
elearning 2009 Introduction The Great Peanut Problem Calorimetry Publication No. 91259 All human activity requires burning food for energy. How much energy is released when food burns in the body? How
More informationCompressed Gas Cylinder Safety
Compressed Gas Cylinder Safety I. Background. Due to the nature of gas cylinders, special storage and handling precautions are necessary. The hazards associated with compressed gases include oxygen displacement,
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 informationOperating Instruction Manual. No. 204M. Oxygen Bomb Calorimeter
Operating Instruction Manual No. 204M 1341 Oxygen Bomb Calorimeter SCOPE These instructions cover the steps to be taken in setting up and operating a Parr 1341 Plain Oxygen Bomb Calorimeter. The user should
More informationReleasing Energy From Food
13 LESSON Releasing Energy From Food INTRODUCTION In Lesson 12, you explored how oxygen and nutrients react chemically in your cells to release energy. But do all foods release the same amount of energy?
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 informationFAJANS DETERMINATION OF CHLORIDE
EXPERIMENT 3 FAJANS DETERMINATION OF CHLORIDE Silver chloride is very insoluble in water. Addition of AgNO 3 to a solution containing chloride ions results in formation of a finely divided white precipitate
More informationIntroduction to Bomb Calorimetry
No. 483M Introduction to Bomb Calorimetry The information presented here is intended to give Parr Calorimeter users an overview of the basic principals involved in measuring the heat of combustion (calorific
More informationSOLID STATE CHEMISTRY - SURFACE ADSORPTION
SOLID STATE CHEMISTRY - SURFACE ADSORPTION BACKGROUND The adsorption of molecules on the surfaces of solids is a very interesting and useful phenomenon. Surface adsorption is at the heart of such things
More informationMOLECULAR WEIGHT BY BOILING POINT ELEVATION
MOLECULAR WEIGHT BY BOILING POINT ELEVATION BACKGROUND This experiment demonstrates the use of colligative properties. The goal is to measure the molecular weight of a non-volatile solute by determining
More informationExp 13 Volumetric Analysis: Acid-Base titration
Exp 13 Volumetric Analysis: Acid-Base titration Exp. 13 video (time: 47:17 minutes) Titration - is the measurement of the volume of a standard solution required to completely react with a measured volume
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 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 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 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 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 informationPREPARATION AND PROPERTIES OF A SOAP
(adapted from Blackburn et al., Laboratory Manual to Accompany World of Chemistry, 2 nd ed., (1996) Saunders College Publishing: Fort Worth) Purpose: To prepare a sample of soap and to examine its properties.
More informationEvaluation copy. Energy Content of Foods. computer OBJECTIVES MATERIALS
Energy Content of Foods Computer 10 Energy content is an important property of food. The energy your body needs for running, talking, and thinking comes from the food you eat. Energy content is the amount
More informationAcid Base Titrations
Acid Base Titrations Introduction A common question chemists have to answer is how much of something is present in a sample or a product. If the product contains an acid or base, this question is usually
More informationPROCEDURES PREVENTION OF ACCIDENTAL IGNITION
Page No: 1 of 7 6.0 PURPOSE (192.751) All possible precautions shall be exercised to prevent the accidental escape and ignition of gas. Whenever possible, potential sources of ignition should be eliminated
More information(S&G 5th ed. Expt 27, 6th, 7th & 8th eds. Expt 26)
Chem 367-2/ Physical Adsorption 63 PHYSICAL ADSORPTION (S&G 5th ed. Expt 27, 6th, 7th & 8th eds. Expt 26) The sample used in this experiment needs to be conditioned for at least two hours before the experiment;
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 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 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 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 informationClass A - Wood, paper, cloth, trash, plastics Solid combustible materials that are not metals. (Class A fires generally leave an Ash.
Not all fires are the same, and they are classified according to the type of fuel that is burning. If you use the wrong type of fire extinguisher on the wrong class of fire, you can, in fact, make matters
More informationCARING FOR YOUR WATER HEATER
http://waterheatertimer.org/troubleshoot-rheem-tankless-water-heater.html Water Heater Inspections CARING FOR YOUR WATER HEATER Venting System (Direct Vent Only) The venting system should be inspected
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 informationCompressed Gas Cylinder Storage and Handling Guide
Overview Compressed gas cylinders are used in many workplaces to store gases that vary from extremely flammable (acetylene) to extremely inert (helium). Many compressed gas cylinders are stored at extremely
More informationScott Batcheller Manager Research & Development. Milwaukee, WI
Transferring Air-Sensitive Reagents Scott Batcheller Manager Research & Development Aldrich Chemistry Milwaukee, WI Background August 3, 2009, Vol. 87, Issue 3 Users of these materials should be technically
More informationDesigning An Experiment Using Baking Soda and Vinegar
Designing An Experiment Using Baking Soda and Vinegar Introduction: Kinetics is the study of chemical reaction rates. It is the study of how fast different chemicals react with one another to form new
More informationDetermining the Quantity of Iron in a Vitamin Tablet. Evaluation copy
Determining the Quantity of Iron in a Vitamin Tablet Computer 34 As biochemical research becomes more sophisticated, we are learning more about the role of metallic elements in the human body. For example,
More informationCOMBUSTION. In order to operate a heat engine we need a hot source together with a cold sink
COMBUSTION In order to operate a heat engine we need a hot source together with a cold sink Occasionally these occur together in nature eg:- geothermal sites or solar powered engines, but usually the heat
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 informationSTANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION EXPERIMENT 14
STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION EXPERIMENT 14 OBJECTIVE The objective of this experiment will be the standardization of sodium hydroxide using potassium hydrogen phthalate by the titration
More informationHeat of Solution. Purpose To calculate the heat of solution for sodium hydroxide (NaOH) and ammonium nitrate (NH 4 NO 3 )
Heat of Solution Purpose To calculate the heat of solution for sodium hydroxide (NaOH) and ammonium nitrate (NH 4 NO 3 ) Background For a given solute, the heat of solution is the change in enerrgy that
More informationAbsorbance Spectrophotometry: Analysis of FD&C Red Food Dye #40
Absorbance Spectrophotometry: Analysis of FD&C Red Food Dye #40 Note: there is a second document that goes with this one! 2046 - Absorbance Spectrophotometry - Calibration Curve Procedure. The second document
More informationOsmosis. Evaluation copy
Osmosis Computer 5 In order to survive, all organisms need to move molecules in and out of their cells. Molecules such as gases (e.g., O 2, CO 2 ), water, food, and wastes pass across the cell membrane.
More informationStoichiometry Limiting Reagent Laboratory. Chemistry 118 Laboratory University of Massachusetts, Boston
Chemistry 118 Laboratory University of Massachusetts, Boston STOICHIOMETRY - LIMITING REAGENT -----------------------------------------------------------------------------------------------------------------------------
More informationthermometer as simple as a styrofoam cup and a thermometer. In a calorimeter the reactants are placed into the
Thermochemistry Readin assinment: Chan, Chemistry 10 th edition, pp. 249-258. Goals We will become familiar with the principles of calorimetry in order to determine the heats of reaction for endothermic
More informationInstructions For SF 6 Refill Kit
S&C Vista Underground Distribution Switchgear UnderCover, Vault-Mounted, and Pad-Mounted Styles Instructions For SF 6 Refill Kit TABLE OF CONTENTS Section Page Section Page INTRODUCTION..................................
More informationChapter 18 Temperature, Heat, and the First Law of Thermodynamics. Problems: 8, 11, 13, 17, 21, 27, 29, 37, 39, 41, 47, 51, 57
Chapter 18 Temperature, Heat, and the First Law of Thermodynamics Problems: 8, 11, 13, 17, 21, 27, 29, 37, 39, 41, 47, 51, 57 Thermodynamics study and application of thermal energy temperature quantity
More informationExperiment 12- Classification of Matter Experiment
Experiment 12- Classification of Matter Experiment 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.
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 informationWHAT YOU DON T KNOW ABOUT ACCUMULATORS CAN KILL YOU!
WHAT YOU DON T KNOW ABOUT ACCUMULATORS CAN KILL YOU! Atlanta (Monroe) GA 770-267-3787 gpm@gpmhydraulic.com www.gpmhydraulic.com What You Don t Know About Hydraulic Accumulators Can Kill You TABLE OF CONTENTS
More informationph Measurements of Common Substances
Chem 100 Section Experiment 10 Name Partner s Name Introduction ph Measurements of Common Substances The concentration of an acid or base is frequently expressed as ph. Historically, ph stands for the
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 informationEnergy and Chemical Reactions. Characterizing Energy:
Energy and Chemical Reactions Energy: Critical for virtually all aspects of chemistry Defined as: We focus on energy transfer. We observe energy changes in: Heat Transfer: How much energy can a material
More informationCHEM 2423 Recrystallization of Benzoic Acid EXPERIMENT 4 - Purification - Recrystallization of Benzoic acid
EXPERIMENT 4 - Purification - Recrystallization of Benzoic acid Purpose: a) To purify samples of organic compounds that are solids at room temperature b) To dissociate the impure sample in the minimum
More informationTA INSTRUMENTS DIFFERENTIAL SCANNING CALORIMETER (DSC) Insert Nickname Here. Operating Instructions
TA INSTRUMENTS DIFFERENTIAL SCANNING CALORIMETER (DSC) Insert Nickname Here Operating Instructions Table of Contents 1 INTRODUCTION Safety 2 Sample Preparation 3 2 BACKGROUND Background Information 4 Resources
More informationStudents will be able to identify popping corn as a physical change.
TO POP OR NOT TO POP THAT IS THE QUESTION. Written by Amy Rowley and Jeremy Peacock Annotation In this laboratory exercise, students will demonstrate science process skills as they use moisture content
More informationPhysical Chemistry Laboratory I CHEM 445 Experiment 6 Vapor Pressure of a Pure Liquid (Revised, 01/09/06)
1 Physical Chemistry Laboratory I CHEM 445 Experiment 6 Vapor Pressure of a Pure Liquid (Revised, 01/09/06) The vapor pressure of a pure liquid is an intensive property of the compound. That is, the vapor
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 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 informationExperiment 2: Using Bomb Calorimetry to Determine the Resonance Energy of Benzene
Experiment 2: Using Bomb Calorimetry to Determine the Resonance Energy of Benzene Reading: SGN: p.145-151 (152-157 may also be useful) Quanta: Benzene, Resonance Benzene was historically a very difficult
More informationThe Determination of an Equilibrium Constant
The Determination of an Equilibrium Constant Computer 10 Chemical reactions occur to reach a state of equilibrium. The equilibrium state can be characterized by quantitatively defining its equilibrium
More informationUNIVERSITY OF MINNESOTA DULUTH DEPARTMENT OF CHEMICAL ENGINEERING ChE 3211-4211 ABSORPTION OF CARBON DIOXIDE INTO WATER
UNIVERSITY OF MINNESOTA DULUTH DEPARTMENT OF CHEMICAL ENGINEERING ChE 3211-4211 ABSORPTION OF CARBON DIOXIDE INTO WATER OBJECTIVE The objective of this experiment is to determine the equilibrium line,
More informationBomb Calorimetry. Example 4. Energy and Enthalpy
Bomb Calorimetry constant volume often used for combustion reactions heat released by reaction is absorbed by calorimeter contents need heat capacity of calorimeter q cal = q rxn = q bomb + q water Example
More informationStoichiometry: Baking Soda and Vinegar Reactions
Stoichiometry: Baking Soda and Vinegar Reactions California Science Content Standards: Teacher Version 3. Conservation of Matter and Stoichiometry: The conservation of atoms in chemical reactions leads
More informationSOLUBILITY, IONIC STRENGTH AND ACTIVITY COEFFICIENTS
SOLUBILITY, IONIC STRENGTH AND ACTIVITY COEFFICIENTS References: 1. See `References to Experiments' for text references.. W. C. Wise and C. W. Davies, J. Chem. Soc., 73 (1938), "The Conductivity of Calcium
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 informationPART I SIEVE ANALYSIS OF MATERIAL RETAINED ON THE 425 M (NO. 40) SIEVE
Test Procedure for PARTICLE SIZE ANALYSIS OF SOILS TxDOT Designation: Tex-110-E Effective Date: August 1999 1. SCOPE 1.1 This method covers the quantitative determination of the distribution of particle
More information