C q T q C T. Heat is absorbed by the system H > 0 endothermic Heat is released by the system H < 0 exothermic
|
|
- Ruth Wilson
- 6 years ago
- Views:
Transcription
1 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 temperature of the substance being heated. The amount of heat energy required to raise the temperature by 1 depends both upon the amount (mass) of substance and the identity (chemical composition) of the substance. The heat capacity, symbolized by, is the ratio of the heat added (q) to the observed temperature rise () q q hemical reactions are often accompanied by the release or absorption of heat. For example, when hydrogen gas is combined with oxygen gas and heated the reaction produces an enormous amount of heat. Reactions that produce (release) heat are said to be exothermic. Reactions that absorb heat are said to be endothermic. The heat released in a chemical reaction is often determined by measuring the temperature change of the material surrounding the chemical reactants and products. This works because the amount of heat associated with a reaction is equal to the amount of heat that is either transferred to or from its surroundings. The study of heat associated with chemical reactions is called thermochemistry. The measure of temperature changes associated with chemical reactions is called calorimetry. To the right is a diagram of a simple calorimeter, a device in which the heat of a reaction is measured. The calorimeter can be as simple as a styrofoam cup and a thermometer. In a calorimeter the reactants are placed into the container and allowed to react. The reactants and the products of a chemical reaction, are called the system. The materials surrounding the system are called the surroundings. As the reaction proceeds, the temperature of the liquid in which the reaction is occurring changes because heat is transferred between the system and the surroundings. We can measure the change in enthalpy ng the process. We use the system as the reference and use the following sign convention: Heat is absorbed by the system H > 0 endothermic Heat is released by the system H < 0 exothermic If the reaction is exothermic then the temperature of the solvent (surroundings) will increase. If the reaction is endothermic then the temperature of the solvent (surroundings) will decrease. The change in temperature of the solvent can then be used to determine the amount of heat transferred: H = m * s *T where H is the change in enthalpy for the reaction (heat of reaction), m is the mass of the solution in which the reaction is occurring, s is a constant called the specific heat capacity, and is the change in
2 temperature of the solution as the reaction takes place. The specific heat capacity depends on the material used. Values of s are given below for several materials. Material s c J/(g K) J/(mol K) s c Material J/(g K) J/(mol K) Bi Zn Pb o Au Ni Pt Fe Hg (l) Ti Sb a I 2 (s) Si Sn K d Al Ag Mg Se Na Ge Li u Water Experimental Procedure The experimental procedure has three parts. You first obtain the heat capacity of the calorimeter by adding measured portions of hot and cold water. This value is used for the second part of the experiment in which you are given a sample of an unknown metal. This sample must be weighed, heated, and placed in the calorimeter. The observed temperature rise is used to calculate the specific heat capacity of the metal. Part I: alibration of the Temperature Probe lick ALIBRATION OF THE TEMPERATURE PROBE. There is a written set of instructions with pictures that will take you through the steps of calibrating your temperature probe. THE WATER THAT YOU USE FOR ALIBRATION SHOULD BE NEAR THE RANGE OF THE DATA THAT YOU WILL OLLET, SO USE OLD/OOL WATER AROUND 20 DEGREES AND WARM WATER AROUND 40 DEGREES. WARM WATER AN BE OBTAINED FROM THE TAP BY THE BENH WHERE THE LAB MATERIALS AN BE FOUND. Part II: Specific Heat apacity of a Metal 1.) Dry out your calorimeter. 2.) Add some cool water (about 20 ) to your calorimeter. Use about 50 g of water, but record exactly (to 4 decimals) the mass of water you use. 3.) Obtain about 15 g of an unknown metal. Record the mass of the metal that you actually obtain, as well as which unknown you re using. 4.) Put your metal in a large test tube, and put the test tube in a beaker of water. Heat the water on a hot plate to approximately 90. Be careful to place the test tube in the beaker in such a manner that the water cannot splash into the test tube. Be certain that the metal sample is in the hot water for at least 5 minutes. 5.) Extend the time of the run by pressing ontrol D and putting in 500 seconds.
3 6.) Proceed to Part III Part III: Heat of Solution 7.) Nest two clean, dry Styrofoam cups together inside a clean, dry 400 ml beaker. This is your calorimeter. 8.) Put about 50 g of deionized water into the calorimeter. Record the actual mass of water in the calorimeter. 9.) Let the filled calorimeter stand for at least 4 minutes, to allow everything to come to room temperature. 10.) Weigh out approximately 2 g of potassium nitrate (KNO 3 ) and record its mass to the nearest g. Grind the salt finely so it will dissolve uniformly. 11.) Observe the temperature of the calorimeter carefully. Run at least 60 seconds of baseline for the water in the calorimeter. For the dissolution of salts, one of two temperature trends can occur: the temperature may either rise quickly and then fall slowly or fall quickly and then rise slowly. Record the maximum or minimum observed temperature according to the trend observed. 12.) Repeat steps (7.) 11.), using approximately two grams of anhydrous sodium carbonate salt (Na 2 O 3 ) and a fresh portion of water. Part IV: Heat of Neutralization 13.) Assemble a clean, dry calorimeter. 14.) Add 25 ml of sodium hydroxide solution (NaOH) to the calorimeter using a graduated cylinder. over the calorimeter and let it sit for at least 2 minutes with its temperature probe in place. An excess of NaOH is being used in this experiment 15.) Using a graduated cylinder, transfer about 25 ml of hydrochloric acid (Hl) to a dry 100 or 150 ml beaker. Record the exact concentration of the acid, and exactly how much you use. 16.) Run at least 60 seconds of baseline of the temperature of the NaOH. 17.) Use a thermometer to record the temperature of the acid in the beaker to the nearest ) Quickly, but carefully, transfer all the acid from the beaker into the NaOH in the calorimeter. Gently stir the contents, being careful to hold only the rim of the calorimeter. 19.) arefully observe the temperature of the calorimeter. The temperature may either rise quickly and then fall slowly or it may fall quickly and then rise slowly. Record the maximum or minimum observed temperature. Again, do this by extrapolation. 20.) Repeat steps 1 6, adding 25 ml of acetic acid (H 3 OOH) to 25 ml of 1.10 M NaOH previously placed in the calorimeter. Be sure to thoroughly rinse and dry the calorimeter between runs. Make sure you know how much of each solution you use, as well as the concentration of each solution.
4 21.) Write the balanced equations for both reactions, and the net ionic equations for both reactions. Part II: Specific Heat apacity of a Metal (continued) 20. You are now ready to add the hot metal to the water in the calorimeter; first you need to record the temperature of the water bath (This will be the T im for the hot metal); pour the hot metal into the calorimeter and allow the system to equilibrate for at least 2-4 more minutes. Do not delay while transferring the metal to your calorimeter. There are consequences for delay, which you will figure out in the post laboratory questions. As soon as the metal is added, swirl the calorimeter continuously to allow through mixing of the water. 21. You may need to fit a straight line to the final linear part of your data. lick and drag the mouse over a linear segment of the data from the end of your run to allow this section of the line to be measured for slope and intercept. With the line segment selected, click on Analyze and select Linear Fit or click on the Linear Fit icon (ask your TA). 22. To Print, click on File and then on Print Graph. lick on the footer box and add the names and other pertinent information. It is recommended that you add the experimental run (e.g. Run #4) and initials of yourself and your partner. DO NOT THROW YOUR OFFEE UPS AWAY! RINSE OUT AND DRY. DATA ANALYSIS Part II: Specific Heat apacity of a Metal Analyze the calorimeter temperature versus time data as you did in Part II. Again extrapolate to find T f and obtain T, the temperature increase. Use your value for to calculate the heat transfer (q ) to the calorimeter: q m s H2 O Your TA will provide you with the c value. Remember that the heat that the metal lost is equal in magnitude to the heat the calorimeter gained, but opposite in sign. q q H Use T f to find T H, the temperature decrease of the metal sample. The heat transfer (q H ) from the metal sample of mass m M is exactly equal in magnitude (but opposite in sign) to the heat gained by the calorimeter: q H m M s M H Insert your experimental values and solve for the specific heat capacity of the metal.
5 The molar heat capacity (c) of a substance is related to its specific heat capacity through the molar mass: c s M Use the Dulong and Petit value of 26 J/(mol * K) for c and your experimental value for s to obtain the molar mass, and hence the atomic mass M of your unknown metal. Part III: Heat of Solution The temperature change of the calorimeter is obtained by comparing its initial temperature (T i ) with the final temperature (T f ) obtained by extrapolation of your data: T f i The amount of heat absorbed during the dissolution can be calculated from this temperature change using: q m s solution solution where is the previously calculated heat capacity of the calorimeter and the mass of the solution is given by m (H2O) + m (salt). The specific heat capacities of the KNO 3 and Na 2 O 3 Remember that the amount of heat absorbed by the calorimeter and water is equal in magnitude to the amount of heat generated by the dissolution of the salt, but opposite in sign. q q rxn Divide q rxn by the mass of the salt to obtain the specific heat of solution; divide q rxn by the number of moles of salt to get the molar heat of solution. Part IV: Heat of Neutralization Find the total temperature change () of the calorimeter as in Part III. Assume a density of 1.00 g/ml to find the mass (m) of the solution in the calorimeter. Assume the specific heat capacity of the solutions to be equal to that of water. Use the known heat capacity ( ) of the calorimeter to calculate the amount of heat evolved during the reaction: q m solution s solution alculate the number of moles of acid contained in 25 ml of the 1.00 M acid solution. Divide the heat of neutralization by this number. This is the molar heat of neutralization of the acid. alculate this quantity for both acids, and include them with your lab report.
Name: Section: Score: /10 PRE LABORATORY ASSIGNMENT EXPERIMENT 7
Name: Section: Score: /10 PRE LABORATORY ASSIGNMENT EXPERIMENT 7 1. Is the sign of Δ r H for an exothermic reaction positive or negative? Why? 2. When 4.21 grams of potassium hydroxide are added to 250.
More informationName: Chemistry 103 Laboratory University of Massachusetts Boston HEATS OF REACTION PRELAB ASSIGNMENT
Name: Chemistry 103 Laboratory University of Massachusetts Boston HEATS OF REACTION PRELAB ASSIGNMENT Chemical and physical changes usually involve the absorption or liberation of heat, given the symbol
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 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 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 informationThermodynamics Enthalpy of Reaction and Hess s Law
P.O. Box 219 Batavia, Illinois 60510 1-800-452-1261 flinn@flinnsci.com Visit our website at: www.flinnsci.com 2003 Flinn Scientific, Inc. All Rights Reserved. Your Safer Source for Science Supplies Thermodynamics
More informationLab #9- Calorimetry/Thermochemistry to the Rescue
Chesapeake Campus Chemistry 111 Laboratory Lab #9- Calorimetry/Thermochemistry to the Rescue Objectives Determine whether a reaction is endothermic or exothermic. Determine the best ionic compound of to
More informationChemistry 212 THE ENTHALPY OF FORMATION OF MAGNESIUM OXIDE LEARNING OBJECTIVES
Chemistry 212 THE ENTHALPY OF FORMATION OF MAGNESIUM OXIDE The learning objectives of this experiment are LEARNING OBJECTIVES A simple coffee cup calorimeter will be used to determine the enthalpy of formation
More informationCOPYRIGHT FOUNTAINHEAD PRESS
Calorimetry: Heats of Solution Objective: Use calorimetric measurements to determine heats of solution of two ionic compounds. Materials: Solid ammonium nitrate (NH 4 NO 3 ) and anhydrous calcium chloride
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 informationCALORIMETRY. m = mass (in grams) of the solution C p = heat capacity (in J/g- C) at constant pressure T = change in temperature in degrees Celsius
CALORIMETRY INTRODUCTION The heat evolved by a chemical reaction can be determined using a calorimeter. The transfer of heat or flow of heat is expressed as the change in Enthalpy of a reaction, H, at
More informationEXPERIMENT 9 ENTHALPY OF REACTION HESS S LAW
EXPERIMENT 9 ENTHALPY OF REACTION HESS S LAW INTRODUCTION Chemical changes are generally accompanied by energy changes; energy is absorbed or evolved, usually as heat. Breaking chemical bonds in reactants
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 informationExperiment 6: Using Calorimetry to Determine the Enthalpy of Formation of Magnesium Oxide
Experiment 6: Using Calorimetry to Determine the Enthalpy of Formation of Magnesium Oxide Reading: Chapter sections 5.4 5.7 of your textbook and this lab handout. Ongoing Learning Goals: To use a scientific
More informationThe CCLI Initiative Computers in Chemistry Laboratory Instruction
Experiment Determining the Coordination Number of Ni and Cu The CCLI Initiative Computers in Chemistry Laboratory Instruction by Enthalpy The objectives of this experiment are to... LEARNING OBJECTIVES
More informationThe Enthalpies of Reactions
The Enthalpies of Reactions Collect 2 Styrofoam cups & a cup lid Digital thermometer Stop watch (from TA) Prepare 400 ml beaker 50 ml graduated cylinder * Take the warm water heated in hood (2015/09/20
More informationMOST of the reactions are carried out at atmospheric pressure, hence
MOST of the reactions are carried out at atmospheric pressure, hence heat changes noted for these reactions are enthalpy changes. Enthalpy changes are directly related to the temperature changes by the
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 informationAP Chemistry: Designing an Effective Hand Warmer Student Guide INTRODUCTION
AP Chemistry: Designing an Effective Hand Warmer Student Guide INTRODUCTION AP and the Advanced Placement Program are registered trademarks of the College Entrance Examination Board. The activity and materials
More informationCHEMISTRY 130 General Chemistry I. Thermochemistry
CHEMISTRY 130 General Chemistry I Thermochemistry The burning of a match, shown above [1], is a chemical reaction between oxygen and sulfur. [2] Intuitively, we know that this reaction releases heat enough
More informationAP Chemistry Lab #10- Hand Warmer Design Challenge (Big Idea 5) Figure 1
www.pedersenscience.com AP Chemistry Lab #10- Hand Warmer Design Challenge (Big Idea 5) 5.A.2: The process of kinetic energy transfer at the particulate scale is referred to in this course as heat transfer,
More informationnot to be republished NCERT MOST of the reactions are carried out at atmospheric pressure, hence THERMOCHEMICAL MEASUREMENT UNIT-3
UNIT-3 THERMOCHEMICAL MEASUREMENT MOST of the reactions are carried out at atmospheric pressure, hence heat changes noted for these reactions are enthalpy changes. Enthalpy changes are directly related
More informationExp 09: Heat of Reaction
Your job is to use a calorimeter to determine the heat of reaction for three different chemical reactions. Each of these reactions is an acid-base neutralization reaction. Before using your calorimeter
More informationMatter & Energy: Temperature & Heat in Physical Processes
Matter & Energy: Temperature & Heat in Physical Processes Objectives: 1) To observe changes in temperature and heat energy which occur during physical processes such as dissolving. 2) To become familiar
More informationTHER Mo CHEMISTRY: HEAT OF Ne UTRALIZATION
Experiment 11 Name: 42 THER Mo CHEMISTRY: HEAT OF Ne UTRALIZATION In this experiment, you will use calorimetry to experimentally determine the heat of neutralization of NaOH-HCl, or the enthalpy of the
More informationExperiment 14 - Heats of Reactions
Experiment 14 - Heats of Reactions If a chemical reaction is carried out inside a calorimeter, the heat evolved or absorbed by the reaction can be determined. A calorimeter is an insulated container, and
More informationCalorimetry and Hess s Law Prelab
Calorimetry and Hess s Law Prelab Name Total /10 1. What is the purpose of this experiment? 2. Make a graph (using some kind of graphing computer software) of temperature vs. time for the following data:
More informationIn general, the condition for a process to occur (for it to be "spontaneous") is that G < 0 (i.e. negative) where
EXPERIMENT 9 Enthalpy Measurement in Chemical Reactions INTRODUCTION: Chemical and physical changes are often accompanied by heat evolution or absorption. A process in which heat is released to the surroundings
More informationDetermining the Enthalpy of a Chemical Reaction
Determining the Enthalpy of a Chemical Reaction Computer 13 All chemical reactions involve an exchange of heat energy; therefore, it is tempting to plan to follow a reaction by measuring the enthalpy change
More informationCalorimetric Determination of Reaction Enthalpies
H + (aq) + OH - q H 2 O Calorimetric Determination of Reaction Enthalpies Purpose: Determine the enthalpy of dissociation of CH 3 COOH CH 3 COOH (aq) CH 3 COO - (aq) + H + (aq) Techniques: Calorimetry
More informationCHM201 General Chemistry and Laboratory I Laboratory 7 Thermochemistry and Hess s Law May 2, 2018
Purpose: CHM201 General Chemistry and Laboratory I Laboratory 7 Thermochemistry and Hess s Law May 2, 2018 In this laboratory, you will measure heat changes arising from chemical reactions. You will use
More informationJust a reminder that everything you do related to lab should be entered directly into your lab notebook. Calorimetry
Just a reminder that everything you do related to lab should be entered directly into your lab notebook. Objectives: Calorimetry After completing this lab, you should be able to: - Assemble items of common
More informationThermodynamics of Salt Dissolution
1 Thermodynamics of Salt Dissolution ORGANIZATION Mode: Part A groups of 3 or 4; Part B individual work; Part C back to groups Grading: lab notes, lab performance, and post-lab report Safety: goggles,
More informationDETERMINING AND USING H
DETERMINING AND USING H INTRODUCTION CHANGES IN CHEMISTRY Chemistry is the science that studies matter and the changes it undergoes. Changes are divided into two categories: physical and chemical. During
More informationThermodynamics. Equations to use for the calculations:
Thermodynamics Introduction: Gibbs Free Energy, G, can be used to determine if a reaction is spontaneous or not. A negative value of G indicates that a given reaction is spontaneous at the measured conditions
More informationThermodynamics. Equations to use for the calculations:
Thermodynamics Introduction: Gibbs Free Energy, G, can be used to determine if a reaction is spontaneous or not. A negative value of G indicates that a given reaction is spontaneous at the measured conditions
More informationCalorimetry Measurements of Fusion, Hydration and Neutralization - Hess Law
Calorimetry Measurements of Fusion, Hydration and Neutralization - Hess Law EXPERIMENT 9 Prepared by Edward L. Brown, Lee University and Verrill M. Norwood, Cleveland State Community College To become
More informationTHE ENERGY OF PHASE CHANGES
C H E M I S T R Y 1 5 0 Chemistry for Engineers THE ENERGY OF PHASE CHANGES DEPARTMENT OF CHEMISTRY UNIVERSITY OF KANSAS The Energy of Phase Changes Introduction Consider heating a solid: as the solid
More informationHEATS OF REACTION EXPERIMENT
16 Text Reference Section 11.4 HEATS OF REACTION EXPERIMENT PURPOSE To measure the heats of reaction for three related exothermic reactions and to verify Hess s law of heat summation. Time Required 50
More informationCalorimetry: Heat of Solution
Calorimetry: Heat of Solution When a substance undergoes a change in temperature, the quantity of heat lost or gained can be calculated using the following relationship: (heat) = m s T (1) The specific
More informationModification of Procedure for Experiments 17 and 18. everything with distilled water and dry thoroughly. (Note: Do not use acetone to rinse cups.
Modification of Procedure for Experiments 17 and 18 I. Calorimeter Constant Obtain two polystyrene cups, a lid for one of the cups and a magnetic stirrer. Rinse everything with distilled water and dry
More informationHESS S LAW: ADDITIVITY OF HEATS OF REACTION
HESS S LAW: ADDITIVITY OF HEATS OF REACTION LAB THC 1.COMP From Chemistry with Computers, Vernier Software & Technology, 2000 INTRODUCTION In this experiment, you will use a Styrofoam-cup calorimeter to
More informationPearson Education Limited Edinburgh Gate Harlow Essex CM20 2JE England and Associated Companies throughout the world
Pearson Education Limited Edinburgh Gate Harlow Essex CM20 2JE England and Associated Companies throughout the world Visit us on the World Wide Web at: www.pearsoned.co.uk Pearson Education Limited 2014
More informationLab 5 Enthalpy of Solution Formation
Chemistry 3202 Lab 5 Enthalpy of Solution Formation Page 1 of 9 Lab 5 Enthalpy of Solution Formation Introduction This lab activity will introduce you to the measurement of energy change associated with
More informationThermochemistry. Introduction. Pre-lab. Safety
Introduction Thermochemistry All chemical reactions and phase changes involve energy. One form of energy is heat: when a change in the energy of a system results in a temperature difference, we say that
More informationThe Hand Warmer Design Challenge: Where Does the Heat Come From?
The Hand Warmer Design Challenge: Where Does the Heat Come From? LSNED Learn Something New Every Day About Sharing and Contributions Interesting Facts Science In Your Mittens: The Chemistry Of Hand Warmers
More information2 nd Semester Study Guide 2016
Chemistry 2 nd Semester Study Guide 2016 Name: Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More informationChemistry 3202 Lab 6 Hess s Law 1
Chemistry 3202 Lab 6 Hess s Law 1 Lab 6 Hess's Law Introduction Chemical and physical changes are always accompanied by a change in energy. Energy changes may be observed by detecting heat flow between
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 informationAdditivity of Heats of Reaction: Hess s Law
Additivity of Heats of Reaction: Hess s Law Experiment In this experiment, you will use a Styrofoam-cup calorimeter to measure the heat released by three reactions. One of the reactions is the same as
More informationExperiment 4 Stoichiometry: The Reaction of Iron with Copper(II) Sulfate
CEAC 105 GENERAL CHEMISTRY Experiment 4 Stoichiometry: The Reaction of Iron with Copper(II) Sulfate Purpose: To enhance the understanding of stoichiometry, a reaction between iron and copper (II) sulfate
More informationThe Energy of Phase Changes
The Energy of Phase Changes Introduction Consider heating a solid: as the solid is warmed, energy from the source of heat is "put into" the solid, and the solid gains energy. If the heating is continued,
More informationIn this activity, you will observe and predict products for some simple
Chemistry Not Chemistry My Type Not My Type Classifying Chemical Reactions In this activity, you will observe and predict products for some simple chemical reactions. You will classify the reactions as
More informationHess' Law: Calorimetry
Exercise 9 Page 1 Illinois Central College CHEMISTRY 130 Name: Hess' Law: Calorimetry Objectives The objectives of this experiment are to... - measure the heats of reaction for two chemical reactions.
More information3.2 Calorimetry and Enthalpy
3.2 Calorimetry and Enthalpy Heat Capacity Specific heat capacity (c) is the quantity of thermal energy required to raise the temperature of 1 g of a substance by 1 C. The SI units for specific heat capacity
More informationSpecific Heat of a Metal
Specific Heat of a Metal Purpose The objective of this experiment is to determine the specific heat of zinc sample using coffeecup calorimeter. Theory In a chemical reaction, the quantity of heat that
More informationSolution Calorimetry
Experiment 7 Solution Calorimetry Prepared by Stephen E. Schullery and Ross S. Nord, Eastern Michigan University PURPOSE Measure the heats of two simple reactions and use Hess's Law to theoretically predict
More informationTable 1. Data for Heat Capacity Trial 1 Trial 2
Thermochemistry: Measuring Enthalpy Change in Chemical Reactions Experiment created by the UMaine InterChemNet Team. Adapted with permission. Print this form and bring it with you to lab. You will complete
More information#30 Thermochemistry: Heat of Solution
#30 Thermochemistry: Heat of Solution Purpose: You will mix different salts with water and note any change in temperature. Measurements using beakers will be compared to measurements using polystyrene
More informationHow bad is that snack anyway?
Physical Sciences 11 Experiment 1 How bad is that snack anyway? Monday, 2/10 Wednesday, 2/12 Science Center Room 117 Please read this entire document and complete the attached prelab before your lab. This
More informationLab Report. Dystan Medical Company - Cold Packs and Hot Packs. Colin Hancock. Wolfgang Allred #202
Lab Report Dystan Medical Company - Cold Packs and Hot Packs Colin Hancock Wolfgang Allred 1225 - #202 18 March 2017 Introduction In this lab, we are employed by the Dystan Medical Supply Company. Our
More informationHESS S LAW: ADDITIVITY OF HEATS OF REACTION
HESS S LAW: ADDITIVITY OF HEATS OF REACTION From Chemistry with Calculators, Vernier Software & Technology In this experiment, you will use a Styrofoam-cup calorimeter to measure the heat released by three
More informationAdditivity of Heats of Reaction: Hess s Law
Additivity of Heats of Reaction: Hess s Law Experiment 21 In this experiment, you will use a Styrofoam-cup calorimeter to measure the heat released by three reactions. One of the reactions is the same
More informationExperiment 7: ACID-BASE TITRATION: STANDARDIZATION OF A SOLUTION
Experiment 7: ACID-BASE TITRATION: STANDARDIZATION OF A SOLUTION Purpose: Determine molarity of a solution of unknown concentration by performing acid-base titrations Performance Goals: Apply the concepts
More informationENTHALPY OF FORMATION OF MgO
ENTHALPY OF FORMATION OF MgO ELECTRONIC LABORATORY NOTEBOOK (ELN) INSTRUCTIONS All work for this experiment must be recorded, attached, or answered in the ELN. Create a pre & inlab page in the Experiment
More information6 Acid Base Titration
E x p e r i m e n t Acid Base Titration Experiment : http://genchemlab.wordpress.com/-titration/ objectives To understand the concept of titration. To explain the difference between the analyte and standard
More informationDesigning a Hand Warmer AP* Chemistry Big Idea 5, Investigation 12 An Advanced Inquiry Lab
Introduction Designing a Hand Warmer AP* Chemistry Big Idea 5, Investigation 12 An Advanced Inquiry Lab Catalog No. AP7654 Publication No. 7654 WEB Put your chemistry skills to commercial use! From instant
More informationIf you need to reverse a reaction, the enthalpy is negated:
In the previous experiment you explored the heat of solution of potassium hydroxide. Using Hess s law, you will now use those results in conjunction with the data collected in this experiment to determine
More informationEXPERIMENT 14 SPECIFIC HEAT OF WATER. q = m s T
EXPERIMENT 14 SPECIFIC HEAT OF WATER INTRODUCTION: Heat is a form of energy which can pass from an object of relatively high temperature to an object of relatively low temperature. One physical property
More informationDr. White Chem 1B Saddleback College 1. Experiment 15 Thermodynamics of the Solution Process
Dr. White Chem 1B Saddleback College 1 Experiment 15 Thermodynamics of the Solution Process Objectives To learn about the relationship between K and ΔG. To learn how the van't Hoff equation can be used
More informationEXPERIMENT A8: CALORIMETRY. Learning Outcomes. Introduction. Upon completion of this lab, the student will be able to:
1 EXPERIMENT A8: CALORIMETRY Learning Outcomes Upon completion of this lab, the student will be able to: 1) Measure the heat of a reaction under constant pressure conditions. 2) Calculate the enthalpy
More informationReaction Stoichiometry
Reaction Stoichiometry PURPOSE To determine the stoichiometry of acid-base reactions by measuring temperature changes which accompany them. GOALS To learn to use the MicroLab Interface. To practice generating
More informationSolution Calorimetry
Experiment 7 Solution Calorimetry Prepared by Stephen E. Schullery and Ross S. Nord, Eastern Michigan University PURPOSE Measure the heats of two simple reactions and use Hess's Law to theoretically predict
More informationExperiment 15 - Heat of Fusion and Heat of Solution
Experiment 15 - Heat of Fusion and Heat of Solution Phase changes and dissolving are physical processes that involve heat. In this experiment, you will determine the heat of fusion of ice (the energy required
More informationThermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes
Thermochemistry Thermochemistry: the study of energy (in the from of heat) changes that accompany physical & chemical changes heat flows from high to low (hot cool) endothermic reactions: absorb energy
More informationFlushing Out the Moles in Lab: The Reaction of Calcium Chloride with Carbonate Salts
Flushing Out the Moles in Lab: The Reaction of Calcium Chloride with Carbonate Salts Pre-lab Assignment: Reading: 1. Chapter sections 3.3, 3.4, 3.7 and 4.2 in your course text. 2. This lab handout. Questions:
More informationMeasuring Enthalpy Changes
Measuring Enthalpy Changes PURPOSE To observe changes in enthalpy in chemical processes. GOALS To identify exothermic and endothermic processes. To relate enthalpy changes and entropy changes to changes
More informationDensity of Aqueous Sodium Chloride Solutions
Experiment 3 Density of Aqueous Sodium Chloride Solutions Prepared by Ross S. Nord and Stephen E. Schullery, Eastern Michigan University PURPOSE Determine the concentration of an unknown sodium chloride
More informationChapter 6: Thermochemistry
Chapter 6: Thermochemistry 1. Light the Furnace: The Nature of Energy and Its Transformations a. Thermochemistry is the study of the relationships between chemistry and energy i. This means that we will
More informationThermochemistry. Questions to ponder. Because 4/20/14. an ice-cube? an ice-cube? Part 2: Calorimetry. But I KNOW. Q=mc T, but T=0
Thermochemistry Part 2: Calorimetry p p If you leave your keys and your chemistry book sitting in the sun on a hot summer day, which one is hotter? Why is there a difference in temperature between the
More informationExperiment 12 Determination of an Enthalpy of Reaction, Using Hess s Law
Experiment 12 Determination of an Enthalpy of Reaction, Using Hess s Law Object: To measure the standard heat of formation, f, of MgO (s), and to become familiar with calorimetry as a toll for measuring
More informationName Date Class SECTION 16.1 PROPERTIES OF SOLUTIONS
SOLUTIONS Practice Problems In your notebook, solve the following problems. SECTION 16.1 PROPERTIES OF SOLUTIONS 1. The solubility of CO 2 in water at 1.22 atm is 0.54 g/l. What is the solubility of carbon
More informationCh. 17 Thermochemistry
Ch. 17 Thermochemistry 17.1 The Flow of Energy Energy Transformations Thermochemistry: study of energy changes in chemical reactions and changes in state Chemical potential energy: energy stored in bonds
More informationCHEMISTRY 135 General Chemistry II. Energy of Phase Changes [1]
CHEMISTRY 135 General Chemistry II Energy of Phase Changes [1] Water at its triple point, where 3 phases coexist, looks unfamiliar a bit like boiling water and ice. [2] Coexistence of two phases, such
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 informationChapter 6: Thermochemistry
Chapter 6: Thermochemistry Section 6.1: Introduction to Thermochemistry Thermochemistry refers to the study of heat flow or heat energy in a chemical reaction. In a study of Thermochemistry the chemical
More information2 nd Semester Study Guide 2017
Chemistry 2 nd Semester Study Guide 2017 Name: KEY Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More informationChemistry. Understanding Water V. Name: Suite 403, 410 Elizabeth St, Surry Hills NSW 2010 (02)
Chemistry Understanding Water V Name: Suite 403, 410 Elizabeth St, Surry Hills NSW 2010 (02) 9211 2610 info@keystoneeducation.com.au keystoneeducation.com.au Water has a higher heat capacity than many
More informationEnergy and Energy Conversion Minneapolis Community and Tech. College Principles of Chemistry 1 v q water = m water C water T water (Equation 1)
Energy and Energy Conversion Minneapolis Community and Tech. College Principles of Chemistry 1 v.6.13 Energy Energy is defined by most textbooks as the capacity to do work. However, the true usefulness
More informationGases. Properties of Gases Kinetic Molecular Theory of Gases Pressure Boyle s and Charles Law The Ideal Gas Law Gas reactions Partial pressures.
Gases Properties of Gases Kinetic Molecular Theory of Gases Pressure Boyle s and Charles Law The Ideal Gas Law Gas reactions Partial pressures Gases Properties of Gases All elements will form a gas at
More informationThermodynamics and the Solubility of Sodium Tetraborate Decahydrate
Thermodynamics and the Solubility of Sodium Tetraborate Decahydrate In this experiment you, as a class, will determine the solubility of sodium tetraborate decahydrate (Na 2 B 4 O 7 10 H 2 O or Na 2 [B
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 informationApply the ideal gas law (PV = nrt) to experimentally determine the number of moles of carbon dioxide gas generated
Teacher Information Ideal Gas Law Objectives Determine the number of moles of carbon dioxide gas generated during a reaction between hydrochloric acid and sodium bicarbonate. Through this investigation,
More informationCALORIMETRY: Heat of Fusion of Ice
Pre-Lab Discussion CALORIMETRY: Heat of Fusion of Ice When a chemical or physical change takes place, heat is either given off or absorbed That is, the change is either exothermic or endothermic It is
More informationEnergy Changes in Reactions p
Energy Changes in Reactions p.126 210 Heat vs. temperature: Heat is a form of energy, it is transferred from one system to another Temperature is an indication of the intensity of heat, it measures the
More informationCalorimetry Measurements of Fusion, Hydration and Neutralization - Hess Law
Calorimetry Measurements of Fusion, Hydration and Neutralization - Hess Law EXPERIMENT 7 Prepared by Edward L. Brown, Lee University To become familiar with energy changes and the use of a calorimeter
More informationQuiz I: Thermodynamics
Quiz I: Thermodynamics SCH4U_2018-2019_V2 NAME: (Total Score: / 30) Multiple Choice (12) 1. What can be deduced from the following reaction profile? A. The reactants are less stable than the products and
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 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 information17.2 Thermochemical Equations
17.2. Thermochemical Equations www.ck12.org 17.2 Thermochemical Equations Lesson Objectives Define enthalpy, and know the conditions under which the enthalpy change in a reaction is equal to the heat absorbed
More information