The Specific Heat of a Liquid
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1 The Purpose: To experimentally determine the specific heat of ethyl alcohol. Principles: Heat is a form of energy which can pass spontaneously from an object at a higher temperature to an object at a lower temperature. One of the properties of matter is that when heat flows into a substance, the temperature is raised; if heat is withdrawn, the temperature is lowered (provided that there is no change in state. Traditionally, the unit of heat is the calorie (cal which is defined as the quantity of heat required to raise the temperature of 1 gram of water by 1 degree Celsius. In keeping with the gradual trend toward SI units, the Joule (J is now being used increasingly in chemistry. The conversion factor between these units is 1 cal = J. The quantity of heat Q required to cause a temperature change in a substance depends on the nature of the substance and is proportional to the mass of the substance (m and the temperature change (Δt: Q ( S. ( m ( t S.W. stands far specific heat, which is a physical constant far a given substance. The specific heat s value depends greatly on the nature of the substance and very little on the temperature. The specific heat can be defined the quantity of heat energy required to raise the temperature of 1 gram of a substance by 1 degree Celsius. The units for specific heat are: cal g C Specific heat is an important quantity because it can be used to calculate the number of calories required to heat a known mass of a substance from one temperature to another. The higher the specific heat of a substance, the less its temperature will change when it absorbs a given amount of heat. Conversely, the lower the specific heat of a substance, the more its temperature will change when it absorbs a given amount of heat. Among common substances that are part of our environment, water has a relatively high specific heat (1.00 cal/g C: it is thus a very effective coolant. The water in oceans, lakes and swimming pools can absorb large amounts of heat without undergoing extreme temperature changes, whereas the dry land surrounding these bodies of water changes its temperature drastically when it absorbs a comparable amount of heat. This is why large bodies of water act as natural temperature moderators; as a result coastal areas enjoy mild winters and cool summers unlike desert areas which are well known for their extreme high and low temperatures. The specific heat of a liquid can readily be measured in a well insulated container which gains or loses very little heat to the surroundings. A container of this sort is called a calorimeter. In this experiment a small thermos (Snack-Jar will be used as a calorimeter.
2 If this is not available two Styrofoam sups, one placed inside the other (placed into a 250 ml beaker for stability and covered with a piece of cardboard may be used instead. A thermometer is then inserted through a hole in the cover of the calorimeter. When using the Snack-Jar, a split rubber stopper will be used. When using Styrofoam cups a cardboard cover will be used. The thermometer will be used to measure the temperature of the calorimeter contents. Part I of this experiment, the specific heat of deionized water at room temperature will be determined. Part II of this experiment, the specific heat of ethyl alcohol at room temperature will be determined. In both parts of the experiment a precisely massed amount of deionized water and ethyl alcohol at room temperature (cooler liquids will be mixed with precisely massed warm water. The warm water will be poured into the cooler liquids. At this time the heat flows from the warm water into the cooler liquid. The temperature of the warm water decreases and the temperature of the cooler liquid increases until they both reach the same temperature. By determining the temperature of the warm water, the temperature of the cooler liquid and the temperature of' the mixture at the time of mixing, the specific heat of the cooler liquid may be determined. Temperature measurements at the exact time of mixing are rather difficult to obtain since no reliable temperature readings can be taken while the two liquids are being mixed. But we can determine this temperature at the time of mixing using Microsoft Excel which will be explained in the calculation section of this experiment. During the mixing of the two liquids a small amount of heat is lost to the calorimeter which absorbs some of the heat lost by the hot water. In this experiment the heat lost to the calorimeter is vey small and will be assumed to be negligible. This provides the following equation: Q Q lost by warm water gained by cool liquid Understanding that Q ( S. ( m ( t the following equation is acheived: ( S. warmwater ( mwarmwater twarmwater ( S. coolliquid mcoolliquid tcoolliquid t warmwater is the temperature change of the warm water. This is calculated from the temperature of the warm water at mixing minus the temperature of the mixture at mixing. These temperatures are only obtainable from the graph. t cool liquid is the temperature change of the cool liquid. This is calculated from the temperature of the mixture at mixing minus the temperature of the cool liquid at mixing. These temperatures are only obtainable from the graph. In the above equation the specific heat of warm water S.. is given as 1.00 cal/g C (this is true for water between 60 C and 90 C. The warmwater experimentally. This allows for the calculation of the m ( H warm water, t, m and t are determined warmwater S. cool liquid. coolliquid coolliquid
3 PART I: THE SPECIFIC HEAT OF WATER AT ROOM TEMPERATURE 1. Heat the warm water a. Place a 250 ml beaker on a ring stand supported by a wire gauze. b. Add between 150 to 200 ml of deionized water. c. Heat the water 2. Prepare cool water. a. Measure about 70 ml of deionized water using your graduated cylinder. b. Place your cool liquid calorimeter on the centigram balance c. Tare the balance with the calorimeter on it. d. Add the 70 ml of water from your graduated cylinder. e. Record the mass of cool water in your notebook to the nearest 0.01g. 3. Prepare warm water. a. Heat the water from step one above to about 85 C b. Place the hot water calorimeter on the centigram balance c. Tare the balance with the calorimeter on it. d. Add about 70g of hot water to the calorimeter. e. Record the mass of the hot water in your notebook to the nearest 0.01g. 4. Time = 0 minutes; Temperature Measurement 5. Time = 1 minute; Temperature Measurement 6. Time = 2 minutes; Temperature Measurement 7. Time = 3 minutes; Temperature Measurement 8. Time = 4 minutes; Temperature Measurement 9. Time = 5 minutes; mix a. Pour the contents of the cold water calorimeter into the hot water calorimeter. 10. Time = 6 minutes; Temperature Measurement 11. Time = 7 minutes; Temperature Measurement 12. Time = 8 minutes; Temperature Measurement 13. Time = 9 minutes; Temperature Measurement 14. Time = 10 minutes; Temperature Measurement 15. Discard the water down the drain.
4 PART II: THE SPECIFIC HEAT OF ETHYL ALCOHOL AT ROOM TEMPERATURE 1. Prepare ethyl alcohol. a. Measure about 70 ml of ethyl alcohol using your graduated cylinder. b. Place your cool liquid calorimeter on the centigram balance c. Tare the balance with the calorimeter on it. d. Add the 70 ml of ethyl alcohol from your graduated cylinder. e. Record the mass of cool water in your notebook to the nearest 0.01g. 2. Prepare warm water. a. Place a 250 ml beaker on a ring stand supported by a wire gauze. b. Add between 150 to 200 ml of deionized water. c. Heat the water to about 85 C d. Place the hot water calorimeter on the centigram balance e. Tare the balance with the calorimeter on it. f. Add about 70g of hot water to the calorimeter. g. Record the mass of the hot water in your notebook to the nearest 0.01g. 3. Time = 0 minutes; Temperature Measurement 4. Time = 1 minute; Temperature Measurement 5. Time = 2 minutes; Temperature Measurement 6. Time = 3 minutes; Temperature Measurement 7. Time = 4 minutes; Temperature Measurement 8. Time = 5 minutes; mix a. Pour the contents of the hot water calorimeter into the cool liquid calorimeter. 9. Time = 6 minutes; Temperature Measurement 10. Time = 7 minutes; Temperature Measurement 11. Time = 8 minutes; Temperature Measurement 12. Time = 9 minutes; Temperature Measurement 13. Time = 10 minutes; Temperature Measurement 14. Discard the water and alcohol in an appropriate waste container.
5 Calculations using Microsoft Excel Use the Microsoft Excel workbook called Chem 51.xls for this section. Enter your data in the highlighted yellow boxes as shown below. Print the worksheet and attach it to your datasheets. Transfer the grayed data into your notebook and your datasheets. NOTE: The calculations performed by Microsoft Excel uses the function called TREND. TREND returns values along a linear trend. It fits a straight line (using the method of least squares to the arrays known_y's and known_x's. It returns the y-values along that line for the array of new_x's that are specified.
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7 Mass of cold water g Mass of hot water g Datasheet Part I Name: Date: Partner: Time 0 minutes... Cold water temperature C... Hot water temperature C Time 1 minute... Cold water temperature C... Hot water temperature C Time 2 minutes... Cold water temperature C... Hot water temperature C Time 3 minutes... Cold water temperature C... Hot water temperature C Time 4 minutes... Cold water temperature C... Hot water temperature C Time 6 minutes... Mixture temperature C Time 7 minutes... Mixture temperature C Time 8 minutes... Mixture temperature C Time 9 minutes... Mixture temperature C Time 10 minutes... Mixture temperature C From Microsoft Excel: Time 5 minutes... Cold water temperature C... Hot water temperature C Time 5 minutes... Mixture temperature C Calculations: Heat lost by warm water: Q S. m t lost by warmwater ( warm water warm water warmwater Heat gained by cold water: Q Q gained bycoolliquid lostby warmwater Specific heat of cold water: Q S. m t gained by cool liquid ( cool liquid cool liquid cool liquid
8 Mass of Ethyl Alcohol water g Mass of hot water g Datasheet Part II Name: Date: Partner: Time 0 minutes... Ethyl Alcohol temperature C... Hot water temperature C Time 1 minute... Ethyl Alcohol temperature C... Hot water temperature C Time 2 minutes... Ethyl Alcohol temperature C... Hot water temperature C Time 3 minutes... Ethyl Alcohol temperature C... Hot water temperature C Time 4 minutes... Ethyl Alcohol temperature C... Hot water temperature C Time 6 minutes... Mixture temperature C Time 7 minutes... Mixture temperature C Time 8 minutes... Mixture temperature C Time 9 minutes... Mixture temperature C Time 10 minutes... Mixture temperature C From Microsoft Excel: Time 5 minutes... Cold water temperature C... Hot water temperature C Time 5 minutes... Mixture temperature C Calculations: Heat lost by warm water: Q S. m t lost by warm water ( warm water warm water warm water Heat gained by ethyl alcohol: Q Q gained bycoolliquid lostby warmwater Specific heat of ethyl alcohol: Q S. m t gained by cool liquid ( cool liquid cool liquid cool liquid
9 Questions Name: Date: Partner: 1. Calculate the Percentage Error in your experiment. (The theoretical value for the ethanol is 0.46 cal/g C 2. What assumption did you make that could explain the reason for your percent error? 3. The ΔT for alcohol is (greater, lesser than the ΔT for water. (Circle the correct answer. 4. The calculated specific heat of alcohol is (greater, lesser that the specific heat of water. (Circle the correct answer. 5. ΔT and specific heat are (directly, inversely proportional. (Circle the correct answer.
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So what kind of intuition do we have about heat and temperature and energy? Discuss the DCI. DCI15.1. Two containers of water are at 20 C initially. One contains 50 mls and the other 100 mls. They are
The 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
Topic 5: Energetics. Heat & Calorimetry. Thursday, March 22, 2012
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HEATS 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
11B, 11E Temperature and heat are related but not identical.
Thermochemistry Key Terms thermochemistry heat thermochemical equation calorimeter specific heat molar enthalpy of formation temperature enthalpy change enthalpy of combustion joule enthalpy of reaction
Chapter 11. Energy in Thermal Processes
Chapter 11 Energy in Thermal Processes Energy Transfer When two objects of different temperatures are placed in thermal contact, the temperature of the warmer decreases and the temperature of the cooler
Experiment 3. Electrical Energy. Calculate the electrical power dissipated in a resistor.
Experiment 3 Electrical Energy 3.1 Objectives Calculate the electrical power dissipated in a resistor. Determine the heat added to the water by an immersed heater. Determine if the energy dissipated by
Part II. Cu(OH)2(s) CuO(s)
The Copper Cycle Introduction In this experiment, you will carry out a series of reactions starting with copper metal. This will give you practice handling chemical reagents and making observations. It
Energy, Heat and Temperature. Introduction
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What Do You Think? Investigate GOALS. Part A: Freezing Water
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Chapter 5 Thermochemistry. 許富銀 ( Hsu Fu-Yin)
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Calorimetry - Specific Heat and Latent Heat
Chapter 3 Calorimetry - Specific Heat and Latent Heat Name: Lab Partner: Section: 3.1 Purpose The purpose of this experiment is to study the relationship between heat and temperature. Calorimetry will
Experiment 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
CHEMISTRY: Chapter 10 Prep-Test
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CHEMISTRY & YOU Chapter 17 Thermochemistry 17.1 The Flow of Energy 17. Measuring and Expressing Enthalpy Changes 17.3 in Changes of State 17.4 Calculating s of Reaction Why does lava cool faster in water