When two samples of matter that are initially at different temperatures are placed in thermal contact, the samples undergo heat transfer until reaching thermal equilibrium at some new, final temperature.  Transferred heat (q) can be measured based on the initial and final temperatures (Tinitial and Tfinal) of a sample that is placed into a known volume of water inside the insulated chamber of a calorimeter.Figure 1  Analysis of a heated sample using a calorimeterAccording to the first law of thermodynamics, the transferred heat energy is conserved, and the heat lost from the sample (indicated by a negative sign) must be equal to the sum of the heat gained by the water and the calorimeter, as expressed by Equation 1.−qsample = qwater + qcalorimeterEquation 1In a perfectly efficient system, qcalorimeter = 0, and all the heat released from the sample is retained by the water.  In real systems, some heat is absorbed by the calorimeter itself.  Based on the amount of heat transferred from the sample and the change in temperature, the heat capacity (C) of the entire sample can be determined.  Expressing the heat capacity per unit mass yields the specific heat capacity (Cp) of the substance comprising the sample.Table 1  Measured specific heat capacities of several selected substancesSample Specific heatcapacity (J/g·°C)Lead 0.129Tungsten 0.132Silver 0.235Strontium 0.315Zinc 0.388Cobalt 0.421Titanium 0.525Wood 2.00Paraffin wax 2.5Water 4.184Experiment 1A sample of water (10.0 mL at 75 °C) was stirred into a calorimeter containing 100.0 mL of water initially at 21 °C.  At thermal equilibrium, the system was found to have a temperature of 25 °C.Experiment 2The water in the calorimeter from Experiment 1 was discarded and replaced with 100.0 mL of fresh water at 25 °C.  An unidentified 100.0 g sample of one of the metals from Table 1 was heated to an initial temperature of 80 °C and then placed into the water.  At thermal equilibrium, the system was found to have a temperature of 30 °C. Question 58Based on the results of the calorimetry experiments, a lab technician concludes that the specific heat capacity of the unidentified metal sample is 0.42 J/g·°C.  Is this conclusion correct?A.Yes; qwater ≈ qmetal in Experiment 2 because Experiment 1 shows that the heat lost from the water and absorbed by the calorimeter is negligible (qcalorimeter ≈ 0).B.Yes; qwater < qmetal in Experiment 2 because Experiment 1 shows that the sample absorbs a small amount of heat from the calorimeter (qcalorimeter < 0).C.No; qwater < qmetal in Experiment 2 because Experiment 1 shows that a significant amount of heat from a sample is lost from the water and absorbed by the calorimeter (qcalorimeter > 0).D.No; qwater > qmetal in Experiment 2 because Experiment 1 shows that the calorimeter adds a small amount of heat to the water (qcalorimeter < 0).