Physics II Lab 2 Report

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School

California Baptist University *

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Course

203

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Chemistry

Date

Feb 20, 2024

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Uploaded by GrandGoose2704

Timothy Allec, Bryan Luna 2/01/2024 PHY203-A Lab 2: Calorimetry Purpose: This lab exemplifies the thermodynamic process of heat transfer and aims to measure the specific heat of an unknown metal using calorimetry. Through the calibration of the calorimeter's heat capacity in Part 1 and the subsequent measurement of the specific heat of the unknown metal in Part 2, students engage in hands-on exploration, reinforcing their comprehension of heat transfer principles, conservation of energy, and specific heat concepts. Part 1 Results: The lab results illustrate heat transfer between heated metal and room-temperature water. Utilizing prescribed equations enables accurate calculations, affirmed by trial 1. In trial 2, these equations and measurements ascertain the specific heat of an unknown metal. Key calculations involve = ∆ for heat transfer and ∆ = ∆ + ∆ + ∆ = 0, 𝑄 𝑀𝑐 𝑇 𝐸 𝐸𝑚𝑒𝑡𝑎𝑙 𝐸𝑤𝑎𝑡𝑒𝑟 𝐸𝑐𝑎𝑙𝑜𝑟𝑖𝑚𝑒𝑡𝑒𝑟 facilitating energy conservation analysis. Data exhibits a consistent temperature change curve over time, with rapid drops and recoveries attributed to gentle container spinning, a human- induced error to expedite the lab. Comparison between trial 1 (brass) and trial 2 (unknown metal) temperatures suggests consistency. One potential experimental error is insufficient boiling water exposure for the metal. Data: Copper Mass 80g Styrofoam Container Mass 19g Styrofoam Water Mass 126g Styrofoam Water Initial Temp 21 C o Beaker Boiling Point 95 C o T i 21 C o T f 24.3 C o

Pascal Graph shows T f achieves thermal equilibrium at 24.6 C o for part 1: Part 2 Results: Aluminum Mass 80g Styrofoam Container Mass 19g Styrofoam Water Mass 129g Styrofoam Water Initial Temp 21 C o Beaker Boiling Point 95 C o T i 21 C o T f 24.6 C o

Pascal Graph shows T f achieves thermal equilibrium at 24.6 C o for part 2: In your results section, analyze and discuss the relevant results of your experiment. Think about your experiment. What is happening? What physics is the experiment demonstrating? Any sources of error? What did you learn? Report your final result In the results section, the observed temperature changes within the calorimeter when different metals were introduced provide insights into their specific heat capacities. By comparing temperature changes and masses, we analyzed their relative abilities to absorb and retain heat energy. The experiment demonstrates calorimetry principles, showing heat exchange equality between substances and surroundings. Possible errors include heat loss to surroundings and incomplete mixing. Despite these, we learned about specific heat and its relation to thermal properties. Our final results offer specific heat values for the metals, informing practical applications. Question #1: Suppose a 150-gram sample requires 560 Joules of heat to raise its temperature by 4 degrees Celsius. What is the material’s specific heat? Q = mcΔT (0.150kg)(560J)(4C) = 336 J/Kg C

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Question #2: In part 1 of the lab, what would be different about your measurement results if you had added twice as much water in the Styrofoam calorimeter? How would this affect the precision or accuracy of your measurements? Doubling the amount of water would change the final temperature of the system to be cooler. Adding twice as much water in the Styrofoam calorimeter would likely result in smaller temperature changes and a slower rate of thermal equilibrium attainment due to the increased heat capacity. This change could potentially affect the accuracy of the measurements, leading to underestimation of heat exchanged, while precision might be maintained if the measurement instrument can still detect small temperature changes effectively. Question #3: Deionized water was used in the calorimeter. Why did we use deionized water and not simply tap water? How would using tap water affect your results? We used deionized water instead of tap water because deionized water is a chemically pure version of water, whereas tap water can contain many different elements besides H20. Deionized water was used in the calorimeter to minimize the presence of impurities and ions, which could interfere with the accuracy of the measurements by affecting the heat capacity and the chemical reactions occurring in the system. Tap water, which contains various minerals and ions, could introduce additional variables and inconsistencies into the experiment. This could lead to less reliable results due to potential alterations in the heat capacity of the water and unwanted chemical reactions that could affect the observed temperature changes. Question #4: In step 6 of part 2, you should have tried to shake off any excess hot water beads from the metal. What would be the effect on your calculated value of the metal’s specific heat if you did not shake off the excess water? If we didn’t shake off the excess from the boiling water, the initial temperature of the water inside of the calorimeter would increase within the calorimeter. This would then have a higher final temperature inside the calorimeter.If excess hot water beads were not shaken off from the metal in step 6 of part 2, they would act as additional heat sources or sinks, affecting the accuracy of the calculated value of the metal's specific heat. Specifically, the retained water beads could lead to an overestimation of the metal's specific heat because they would continue to release heat into the system, contributing to a higher measured temperature change. This would result in an artificially inflated specific heat value for the metal. Conclusion: In conclusion, this calorimetry lab provided valuable insights into determining the specific heats of metals using temperature and mass measurements. By observing temperature changes within the calorimeter, we successfully fulfilled our objective of determining specific heat values for the metals under investigation. Additionally, the experiment highlighted the significant time required for temperature equilibrium to be reached within the calorimeter, emphasizing the importance of patience and precision in experimental procedures. Through this lab, we gained practical experience in applying calorimetry principles and furthered our understanding of thermodynamic concepts related to heat transfer and temperature equilibrium.

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