Lab Report On Calorimeter Lab

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Calorimeter Lab Report Author: Marcos Alberto Lab Partners: Kiley Anselmo, Jacob Bufka General Chemistry III Professor: Dr. M. Ibele April 17, 2015 Introduction: The first law of thermodynamics states that energy cannot be created nor destroyed. Therefore when energy leaves one place it has to have another place to go to, it maintains a constant rate. The equation that proves that statement is: ΔUsystem + ΔUsurroundings = 0 Eq. 1 There are two ways that energy can be transferred from or to a system that will include the transfer of energy in the form of heat (expressed as q) or the ability of the system to do “work”. In this laboratory experiment the change of energy due to…show more content…
It was a Styrofoam cup covered with a piece of cardboard with a hole in the center for the thermometer to be placed in the solution. It may not be as accurate because the solution loses heat since the walls and the lid are not fully impermeable. Throughout this experiment the same calorimeter will be used so the calorimeter constant (Ccal) will not change. So in order to integrate all the variables to relate the change in the system with the change in the surrounding (calorimeter) a new equation is needed: msystem Cp ΔTsystem + Ccal ΔTcal = 0 Eq. 4 This experiment was divided in multiple parts. First the Ccal was found using the specific heat of the system in order to proceed to the second part where this constant will be needed. The purpose of the second part was to find the specific heat of a unknown metal, which will then be compared to known specific heats in order to find out what the unknown metal was. On the second day of the experiment it was necessary to find the new Ccal of the calorimeter because the materials used were different so it could not be assumed to have the same specific heat. On day 2 of the experiment the objective was to find the effect of NaOH reacting with the room temperature water in the calorimeter.
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