Exp 10 Lab.pdf - Calorimetry and Hesss Law Experiment Ten...

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*-Primary Author Calorimetry and Hess’s Law Experiment Ten- November 2, 2016 Section of 565- Tjader De Alba*, Sonia Shah Summary Through this experiment calorimetry and Hess’s Law was used to find the heat of combustion of magnesium metal. Since it would be too hard to measure the heat of the magnesium metal reaction two different reactions were used. Magnesium was mixed with hydrogen chloride for reaction one and magnesium oxide was mixed with hydrogen chloride for reaction 2. These two reactions would be added together to get ∆𝐻 . In Part A of the experiment the calorimeter was set up with the use of two Styrofoam cups inside of each other. After obtaining the weight of the dry calorimeter, with the stir bar added in, 40mL of room temperature distilled water was added in and the calorimeter was reweighed. The calorimeter was then put inside a 250mL beaker and the temperature probe was inserted to monitor the temperature. 60mL of distilled water was then boiled and then added to the calorimeter. The temperature of the calorimeter was monitored the whole time Through LoggerPro a graph of the temperature was obtained over time. In Part B of the experiment an eight to ten inch magnesium ribbon was put into 50mL of 1.0M of hydrogen chloride and the heat of the reaction over time was recorded. The dry calorimeter from Part A was reweighed with the stir bar inside, and then the 50mL of hydrogen chloride was added to the calorimeter. The calorimeter was then reweighed. After obtaining a baseline temperature of the hydrogen chloride the eight to ten inch magnesium ribbon, sanded down, was added into the calorimeter. The temperature of the reaction was then recorded over several minutes through LoggerPro. Part C of the experiment was conducted the same as Part B, but the eight to ten inch magnesium ribbon was replaced with 400mg of magnesium oxide. After obtaining a baseline temperature the 400mg of magnesium oxide was added to the 50mL of 1.0M hydrogen chloride and the temperature of the reaction was observed through LoggerPro. In Part A, it was found that the Calorimeter Constant of the calorimeter used in the experiment was 180.87 J. In Parts B and C,
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