Determine the mass of Jupiter if a gravitational force on a scientist whose weight when in earth is 686 N, is Fgrav = 1823 N. Advertisement Advertisement italianbrownsugar italianbrownsugar Answer: the correct answers is 100 22.7 and 24.6. ;?C2w%9iW/k-gN1WiuK; A/rNJTem'mzRUE|QG9^GdXK|oe3IX;{#y?h9b6hFV,^u$e`rm`DqXO]eBuwHUIv33BEh;P7kju~U)S\K}l2($_h(T=>`` V; The specific heat capacities of each metal is displayed to students: Al 0.903 J/gC Pb 0.160 J/gC. Her work was important to NASA in their quest for better rocket fuels. Example #4: 10.0 g of water is at 59.0 C. Electric Motor Alternators The final temperature of the water was measured as 39.9 C. If energy is coming out of an object, the total energy of the object decreases, and the values of heat and T are negative. Training Online Engineering, Fusion - Melting Change of Liquid State Thermodynamics, Critical Temperature and Melting Point for Common Engineering Materials, Atomic Numbers Weights Melting Temperatures. For the example shown in (b), the total energy per 228-g portion is calculated by: So, you can use food labels to count your Calories. Keep in mind that BOTH the iron and the water will wind up at the temperature we are calling 'x.' Specific heat is measured in BTU / lb F in imperial units and in J/kg K in SI units. Where Q is the energy added and T is the change in temperature. But where do the values come from? Many of the values used have been determined experimentally and different sources will often contain slightly different values. FlinnScientific, Batavia, Illinois. The specific heat capacity during different processes, such as constant volume, Cv and constant pressure, Cp, are related to each other by the specific heat ratio, = Cp/Cv, or the gas constant R = Cp - Cv. How much heat was trapped by the water? Thermodynamics .style1 { The calorimeters described are designed to operate at constant (atmospheric) pressure and are convenient to measure heat flow accompanying processes that occur in solution. Helmenstine, Todd. Bomb calorimeters require calibration to determine the heat capacity of the calorimeter and ensure accurate results. Calculate the final temperature of the system. Structural Shapes So the temperature stays flat during that period, throwing off the relationship between energy, temperature and specific heat in that situation. change) (specific heat). 4) The copper loses heat and drops in temperature to the final value of x: 5) The amount of heat lost by the copper equals the heat gained by the water: Notice how the kJ from the ice melting is used as J rather than kJ. Compare the heat gained by the cool water to the heat releasedby the hot metal. Lubrication Data Apps Pressure Vessel With some planning all three representations can be explored (not simultaneously) FROM ALEX JOHNSTONE'S triangle: macroscopic, microscopic, symbolic. This solution uses 0.901 for aluminum and 4.18 for water: Todd Helmenstine is a science writer and illustrator who has taught physics and math at the college level. Assuming the use of copper wire ( = 0.004041) we get: \: \text{J/g}^\text{o} \text{C}\). till what time the balloon expands when the pressure of outside air is greater than than the inside pressure or equal?, Problem 7.4 Two capacitors, each of capacitance 2 F are connected in parallell. In your day-to-day life, you may be more familiar with energy being given in Calories, or nutritional calories, which are used to quantify the amount of energy in foods. Other times, you'll get the SI unit for temperature, which is Kelvin. We will ignore the fact that mercury is liquid. Note that the specific heat for liquid water is not provided in the text of the problem. across them is 120V, calculate the charge on each capacit The specific heat of water is approximately 4.184 J/g C, so we use that for the specific heat of the solution. More recently, whole-room calorimeters allow for relatively normal activities to be performed, and these calorimeters generate data that more closely reflect the real world. Compare the heat gained by the water in Experiment 1 to the heat gained by the water in experiment 2. media.pearsoncmg.com/bc/bc_0media_chem/chem_sim/calorimetry/Calor.php, DC11005Flinn SpecificHeatsOfMetalsDEMO.PDF. Place 50 mL of water in a calorimeter. When we use calorimetry to determine the heat involved in a chemical reaction, the same principles we have been discussing apply. 3) Total heat given off by the metal sample: 4) Determine the specific heat of the metal sample: Go to calculating final temperature when mixing metal and water problems 1 - 15. A different type of calorimeter that operates at constant volume, colloquially known as a bomb calorimeter, is used to measure the energy produced by reactions that yield large amounts of heat and gaseous products, such as combustion reactions. The metals are added to two insulated cups or calorimeters, each containing the same amount of water initially at room temperature. Randy Sullivan, University of Oregon Because the temperature of the iron increases, energy (as heat) must be flowing into the metal. By the end of this section, you will be able to: One technique we can use to measure the amount of heat involved in a chemical or physical process is known as calorimetry. 1.33 kJ; assume that the calorimeter prevents heat transfer between the solution and its external environment (including the calorimeter itself) and that the specific heat of the solution is the same as that for water. At the beginning, the metal is at higher temperature (70.4 C) while the water is at lower temperature (23.6 C). Example #8: A 74.0 g cube of ice at 12.0 C is placed on a 10.5 kg block of copper at 23.0 C, and the entire system is isolated from its surroundings. When considered as the temperature of the reverse change from liquid to solid, it is referred to as the freezing point or crystallization point. If the hand warmer is reheated, the NaC2H3O2 redissolves and can be reused. Keith Nisbett, Copyright 2000 - The question gives us the heat, the final and initial temperatures, and the mass of the sample. The specific heat capacity is the heat or energy required to change one unit mass of a substance of a constant volume by 1 C. You would have to look up the proper values, if you faced a problem like this. Threads & Torque Calcs Multiply the change in temperature with the mass of the sample. For example Carla Prado's team at University of Alberta undertook whole-body calorimetry to understand the energy expenditures of women who had recently given birth. Vibration Engineering In this one, you can see the metal disc that initiates the exothermic precipitation reaction. The Snellen human calorimeter revisited, re-engineered and upgraded: Design and performance characteristics., https://openstax.org/books/chemistry-2e/pages/1-introduction, https://openstax.org/books/chemistry-2e/pages/5-2-calorimetry, Creative Commons Attribution 4.0 International License, Calculate and interpret heat and related properties using typical calorimetry data. This demonstration is under development. Can you identify the metal from the data in Table 7.3 "Specific Heats of Selected Substances"? . Calorimetry measurements are important in understanding the heat transferred in reactions involving everything from microscopic proteins to massive machines. This value for specific heat is very close to that given for copper in Table 7.3. then you must include on every physical page the following attribution: If you are redistributing all or part of this book in a digital format, 6. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Choose a large enough beaker such that both the aluminum metal and lead metal will be submerged in the boilingwater bath. Johnstone, A. H. 1993. Noting that 75/25 = 3, we arrive at: 38.25 0.45x = 12.552x 251.04 then 13.002x = 289.29 The answer is 22.25 C if you aren't too fussy about significant figures. The ability of a substance to contain or absorb heat energy is called its heat capacity. Specific heat calculations are illustrated. << /Length 4 0 R /Filter /FlateDecode >> The amount of heat absorbed by the calorimeter is often small enough that we can neglect it (though not for highly accurate measurements, as discussed later), and the calorimeter minimizes energy exchange with the outside environment. Economics Engineering 3) This problem could have been solved by setting the two equations equal and solving for 'x. It is 0.45 J per gram degree Celsius. After a few minutes, the ice has melted and the temperature of the system has reached equilibrium. He holds bachelor's degrees in both physics and mathematics. First heat a 10 gram aluminum metal in beaker of boiling water for at least 10 minutes so that the metal's . These problems are exactly like mixing two amounts of water, with one small exception: the specific heat values on the two sides of the equation will be different. The OpenStax name, OpenStax logo, OpenStax book covers, OpenStax CNX name, and OpenStax CNX logo If this occurs in a calorimeter, ideally all of this heat transfer occurs between the two substances, with no heat gained or lost by either its external environment. Engineering Mathematics "Calculating the Final Temperature of a Reaction From Specific Heat." (b) The foods nutritional information is shown on the package label. Plug the given values into your equation: 75.o J = 2.0 g x (4.184 J/gC) x (87 C - t0). In these cases, the units for specific heat will either be Joules/gram C or else Joules/gram K. The same could happen with grams versus kilograms for the mass, or Joules to Bmu for energy. Relatively inexpensive calorimeters often consist of two thin-walled cups that are nested in a way that minimizes thermal contact during use, along with an insulated cover, handheld stirrer, and simple thermometer. Civil Engineering The specific heat of a substance is the amount of energy that must be transferred to or from 1 g of that substance to change its temperature by 1. 1. If you examine your sources of information, you may find they differ slightly from the values I use. Nutritional labels on food packages show the caloric content of one serving of the food, as well as the breakdown into Calories from each of the three macronutrients (Figure 5.18). Determine the specific heat and the identity of the metal. These calorimeters are used to measure the metabolism of individuals under different environmental conditions, different dietary regimes, and with different health conditions, such as diabetes. The process NaC2H3O2(aq)NaC2H3O2(s)NaC2H3O2(aq)NaC2H3O2(s) is exothermic, and the heat produced by this process is absorbed by your hands, thereby warming them (at least for a while). The temperature change, along with the specific heat and mass of the solution, can then be used to calculate the amount of heat involved in either case. More expensive calorimeters used for industry and research typically have a well-insulated, fully enclosed reaction vessel, motorized stirring mechanism, and a more accurate temperature sensor (Figure 5.13). The heat that is either absorbed or released is measured in joules. The carbohydrate amount is discounted a certain amount for the fiber content, which is indigestible carbohydrate. are not subject to the Creative Commons license and may not be reproduced without the prior and express written The pellet is burned inside a bomb calorimeter, and the measured temperature change is converted into energy per gram of food. with rxn and soln used as shorthand for reaction and solution, respectively. What was the initial temperature of the metal bar, assume newton's law of cooling applies. Note that the iron drops quite a bit in temperature, while the water moves only a very few (2.25 in this case) degrees. If the p.d. Friction Engineering if an object is orbiting the sun with an orbital period of 15 years, what is its average distance from the sun? What is the radius of the moon when an astronaut of madd 70kg is ha By continuing to view the descriptions of the demonstrations you have agreed to the following disclaimer. (23.0 x) (4042.5) = 26578.18 + 309.616x, x = 15.2 C (to three sig figs, I followed the rule for rounding with 5), Example #9: How many grams of water can be heated form 25.0 C to 35.0 C by the heat released from 85.0 g of iron that cools from 85.0 C to 35.0 C? The direction of heat flow is not shown in heat = mcT. Question: Computation of Specific Heat for Unknown Metal Table view List View Trial 1 21.90 Trial 2 21.90 1.90 1.90 47.44 Mass of unknown metal (g) Mass of calorimeter cup (g) Mass of calorimeter and water (g) Temperature of boiling water bath ("C) Initial temperature of calorimeter water (C) Final temperature of water and metal ("C) 46.10 100.14 99.92 22.52 22.33 Every substance has a characteristic specific heat, which is reported in units of cal/gC or cal/gK, depending on the units used to express T. The temperature change of the metal is given by the difference between its final temperature and its initial temperature: And the negative sign means the temperature of the metal has decreased. What is the final temperature of the metal? Record the temperature of the water. The calibration is generally performed each time before the calorimeter is used to gather research data. The final temperature (reached by both copper and water) is 38.7 C. Materials and Specifications When using a calorimeter, the initial temperature of a metal is 70.4C. Mechanical Tolerances Specs This specific heat is close to that of either gold or lead. Our mission is to improve educational access and learning for everyone. Students are asked to predict what will happen to the temperature of water and the temperature of the metals. Initial temperature of water: 22.4. Heat the metals for about 6 minutes in boiling water. (The specific heat of brass is 0.0920 cal g1 C1.). Manufacturing Processes This site is using cookies under cookie policy . There is no difference in calculational technique from Example #1. Which metal will reach 60C first? Click on this link to access the US Department of Agriculture (USDA) National Nutrient Database, containing nutritional information on over 8000 foods. Place 50 mL of water in a calorimeter. Apply the First Law of Thermodynamics to calorimetry experiments. m m c m DT m = m w c w DT w. For water, c w = 4.2 J/g/degree Celsius = 1 calorie per gram per degree Celsius. Applications and Design , ving a gravitational force The temperature change measured by the calorimeter is used to derive the amount of heat transferred by the process under study. The temperature of the water changes by different amounts for each of the two metals. In reality, the sample may vaporize a tiny amount of water, but we will assume it does not for the purposes of the calculation. Engineering Materials. So it takes more energy to heat up water than air because water and air have different specific heats. Contact: Randy Sullivan,smrandy@uoregon.edu. Most ferrous metals have a maximum strength at approximately 200C. Two different metals, aluminum and lead, of equal mass are heated to the same temperature in a boiling water bath. and The result has three significant figures. The temperature change of the water is given by the difference between its final temperature and its initial temperature: And the positive sign means that the temperature of the water has increased. You can use this value to estimate the energy required to heat a 500 g of aluminum by 5 C, i.e., Q = m x Cp x T = 0.5 * 897* 5 = 2242.5 J. Answer: initial temperature of metal: 100. However, the observation that the metal is silver/gray in addition to the value for the specific heat indicates that the metal is lead. Use the tongs and grab the hot aluminum metal and place it in the second calorimeter containing 50mLof room temperature water. Journal of Chemical Education, 70(9), p. 701-705. Make sure you check with your teacher as to the values of the various constants that he/she wishes for you to use. | Contact, Home (credit: modification of work by Science Buddies TV/YouTube). Substitute the known values into heat = mcT and solve for amount of heat: \[\mathrm{heat=(150.0\: g)\left(0.108\: \dfrac{cal} {g\cdot {^\circ C}}\right)(48.3^\circ C) = 782\: cal} \nonumber \]. A \(15.0 \: \text{g}\) piece of cadmium metal absorbs \(134 \: \text{J}\) of heat while rising from \(24.0^\text{o} \text{C}\) to \(62.7^\text{o} \text{C}\). 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Use the graph of temperature versus time to find the initial temperature of the water and the equilibrium temperature, or final temperature, of the water and the metal object after the object warms up and the water cools . The final temperature is:, \[T_f = 23.52^\text{o} \text{C} - 3.24^\text{o} \text{C} = 20.28^\text{o} \text{C} \nonumber \]. "Do not do demos unless you are an experienced chemist!" The temperature change produced by the known reaction is used to determine the heat capacity of the calorimeter. Strength of Materials (Cp for Hg = 0.14 J per gram degree Celsius.). This is what we are solving for. If we place the metal in the water, heat will flow from M to W. The temperature of M will decrease, and the temperature of W will increase, until the two substances have the same temperaturethat is, when they reach thermal equilibrium (Figure 5.14). For example: Say you add 75.0 Joules of energy to 2.0 grams of water, raising its temperature to 87 C. Solution Key Number Two: the energy amount going out of the warm water is equal to the energy amount going into the cool water. The specific heat of iron is 0.450 J/g C, q = (mass) (temp. If the sample gives off 71.7 cal, it loses energy (as heat), so the value of heat is written as a negative number, 71.7 cal. A chilled steel rod (2.00 C) is placed in the water. A sample of food is weighed, mixed in a blender, freeze-dried, ground into powder, and formed into a pellet. Substitute the known values into heat = mcT and solve for c: \(c \,\mathrm{=\dfrac{-71.7\: cal}{(10.3\: g)(-75.5^\circ C)}}\). Record the temperature of the water. If you are redistributing all or part of this book in a print format, Example #3: Determine the final temperature when 20.0 g of mercury at 165.0 C mixes with 200.0 grams of water at 60.0 C. 2. It produces 2.9 kJ of heat. Engineering Forum So, if we want to determine the units for specific heat, we'll just isolate the term in the above formula to get c = q m T. When working or playing outdoors on a cold day, you might use a hand warmer to warm your hands (Figure 5.15). Use the formula: Q = mcT, also written Q = mc (T - t0) to find the initial temperature (t 0) in a specific heat problem. then you must include on every digital page view the following attribution: Use the information below to generate a citation. As an Amazon Associate we earn from qualifying purchases. The values of specific heat for some of the most popular ones are listed below. q = (50.0 g) (10.0 C) (0.092 cal g1 C1). if you aren't too fussy about significant figures. Noting that since the metal was submerged in boiling water, its initial temperature was 100.0 C; and that for water, 60.0 mL = 60.0 g; we have: Comparing this with values in Table 5.1, our experimental specific heat is closest to the value for copper (0.39 J/g C), so we identify the metal as copper. Example #1: Determine the final temperature when a 25.0 g piece of iron at 85.0 C is placed into 75.0 grams of water at 20.0 C. The university shall not be liable for any special, direct, indirect, incidental, or consequential damages of any kind whatsoever (including, without limitation, attorney's fees) in any way due to, resulting from, or arising in connection with the use of or inability to use the web site or the content. The mass is given as 150.0 g, and Table 7.3 gives the specific heat of iron as 0.108 cal/gC. Plastics Synthetics A computer animation depicting the interaction of hot metal atoms at the interface with cool water molecules can accompany this demonstration (see file posted on the side menu). Comment: none of the appropriate constants are supplied. What is the specific heat of the metal sample? See the attached clicker question. Pumps Applications Most values provided are for temperatures of 77F (25C). Studies like this help develop better recommendations and regimens for nutrition, exercise, and general wellbeing during this period of significant physiological change. (credit a: modification of work by Harbor1/Wikimedia commons), (a) Macaroni and cheese contain energy in the form of the macronutrients in the food. How about water versus metal or water versus another liquid like soda? The EBSD images of phase distribution of as-HPed FG (unimodal) and bimodal Mo-Si-B alloys are shown in Figs. The specific heat of water is 4179 J/kg K, the amount of heat required to raise the temperature of 1 g of water by 1 Kelvin. That last paragraph may be a bit confusing, so let's compare it to a number line: To compute the absolute distance, it's the larger value minus the smaller value, so 85.0 to x is 85.0 minus x and the distance from x to 20.0 is x minus 20.0. If the materials don't chemically react, all you need to do to find the final temperature is to assume that both substances will eventually reach the same temperature. Two different metals, aluminum and lead, of equal mass are heated to the same temperature in a boiling water bath. This link shows the precipitation reaction that occurs when the disk in a chemical hand warmer is flexed. Heat capacity is an extensive propertyit depends on the amount or mass of the sample. What is the final temperature of the crystal if 147 cal of heat were supplied to it? This type of calorimeter consists of a robust steel container (the bomb) that contains the reactants and is itself submerged in water (Figure 5.17). Answer: 1-initial temperature of metal =100 2- initial temperature of water = 22.4 3- final temperature of both = 27.1 Explanation: I just did it Advertisement New questions in Chemistry Along with energy obtained from fossil fuels, nuclear sources, and water, environmentalists are encouraging the use of energy from wind. Salt in the hand warmer catalyzes the reaction, so it produces heat more rapidly; cellulose, vermiculite, and activated carbon help distribute the heat evenly. In this demonstration, heat energy is transferred from a hot metal sample to a cool sample of water: qlost+qgain= 0. The caloric content of foods can be determined by using bomb calorimetry; that is, by burning the food and measuring the energy it contains. The thermal expansion coefficients employed are highly dependent on initial temperatures and may undergo significant change. J.u dNE5g0;rj+>2 JeB9"jcX`$V|LpwhT.oQ"GwNQ#Y;(y*rDFXzL=L,joXEP&9!mEu0 EgW,g>sqh4mbf0+[[!hw9;Q6 Y,CY|faGA'_Hxd DH3 Example #5: 105.0 mL of H2O is initially at room temperature (22.0 C). In our previous studies, the approximation of the infinite absorption coefficient of the sensor nanolayer was considered by the example of gold. It would be difficult to determine which metal this was based solely on the numerical values. bfW>YunEFPH/b\#X K0$4Sa#4h1~b1i$QXg^k14{IqU5k1xK_5iHUmH1I "_H 2) Use 35.334 kJ and the heat of vaporization of water to calculate moles and then mass of water vaporized: mass H2O = (0.869225 mol) (18.015 g/mol) = 15.659 g, Bonus Example: A 250. gram sample of metal is heated to a temperature of 98.0 C. In Fig. 5) As the gold ring and the silver ring cool down, they liberate energy that sums to 102.2195 J. What is the specific heat of the metal? 1) The basic equation to be used is this: 2) The two masses associated with the gold and the silver rings: The 1.8 is arrived at thusly: 23.9 22.1. 2011. Calculate the temperature from the heat transferred using Q = Mgh and T = Q mc T = Q m c , where m is the mass of the brake material. The colder water goes up in temperature, so its t equals x minus 20.0. "Calculating the Final Temperature of a Reaction From Specific Heat." D,T(#O#eXN4r[{C'7Zc=HO~ Th~cX7cSe5c Z?NtkS'RepH?#'gV0wr`? Note that the water moves only 0.35 of one degree. Since most specific heats are known (Table \(\PageIndex{1}\)), they can be used to determine the final temperature attained by a substance when it is either heated or cooled. After 5 minutes, both the metal and the water have reached the same temperature: 29.7 C. The Heat is on: An inquiry-based investigation for specific heat. UO Libraries Interactive Media Group. A simple calorimeter can be constructed from two polystyrene cups. You can plug in all the other values that you're given, then solve for t0. Retrieved from https://www.thoughtco.com/heat-capacity-final-temperature-problem-609496. \[c_p = \dfrac{q}{m \times \Delta T} = \dfrac{134 \: \text{J}}{15.0 \: \text{g} \times 38.7^\text{o} \text{C}} = 0.231 \: \text{J/g}^\text{o} \text{C} \nonumber \]. g (302.0 C) (0.900 J g1 C1) = 35334 J = 35.334 kJ. When using a calorimeter, the initial temperature of a metal is 70.4C. (The term bomb comes from the observation that these reactions can be vigorous enough to resemble explosions that would damage other calorimeters.) The change in temperature is given by \(\Delta T = T_f - T_i\), where \(T_f\) is the final temperature and \(T_i\) is the initial temperature. Since the initial temperature usually . A calorimeter is a device used to measure the amount of heat involved in a chemical or physical process. What was the initial temperature of the water? The formula for specific heat capacity, C, of a substance with mass m, is C = Q /(m T). Having this information, you can also calculate how much energy you need to supply to a sample to increase or decrease its temperature. It is 0.45 J per gram degree Celsius. This means: Please note the use of the specific heat value for iron. This book uses the T = 20 C T = T final - T initial T final = T inital + T T final = 10 C + 20 C T final = 30 C Answer: The final temperature of the ethanol is 30 C. At 20 Celsius, we get 12.5 volts across the load and a total of 1.5 volts (0.75 + 0.75) dropped across the wire resistance. In fact, water has one of the highest specific heats of any "common" substance: It's 4.186 joule/gram C. Calculate the value of q for this reaction and explain the meaning of its arithmetic sign. Hardware, Metric, ISO to find the initial temperature (t0) in a specific heat problem. Explanation: Edguinity2020. Compare the heat gained by the water in Experiment 1 to the heat gained by the water in experiment 2. water bath. URL:https://media.pearsoncmg.com/bc/bc_0media_chem/chem_sim/calorimetry/Calor.php. You need to look up the specific heat values (c) for aluminum and water. We recommend using a Have students predict what will happen to the temperature of the water in the two calorimeters when hot lead is added to one and hot aluminum is added to the other. This demonstration assess students' conceptual understanding of specific heat capacities of metals. The copper mass is expressed in grams rather than kg.