Calorimetry Measuring Heat of Formation Report

Calorimetry Measuring Heat of Formation Report

Calorimetry Measuring Heat of Formation Report

This exercise asks you to collect, organize, analyze, and evaluate data you collected in the lab. You will type a lab report that includes the following: 

  • Title page
  • Objective
  • Introduction
    • Give the logic of the experiment.
    • Be sure to define key terms and all applied experimental equations (e.g. calorimetry, calorimeter, enthalpy of formation, heat capacity of calorimeter, heat, balanced chemical equations, Hess’ law, and percent error.).
  • Procedure Reference
    • If there are any changes to the published procedure be sure to note them here.
  • Results and Calculations section
    • Table summarizing
      • Your major experimental data (e.g. heat capacity of calorimeter, experimental heat of formation for Mg2+ & MgO, actual heat of formation for Mg2+ & MgO, and percent error)
      • Be sure to include the PDF with the data that you were provided when you turn in your report. 
    • Graphs
      • Since data was given to you, you can use the graphs that were provided.  You do not need to make graphs.  Just paste them into the appropriate section of the report.
  • One sample calculation of each type.
  • Discussion
    • We did not record the boiling and freezing point of water experimentally. But issues with these measurements could possibly be something that would cause error in this experiment.  Perhaps something related to this would provide one of your sources of error?
    • State the heat of formation for MgO and describe any errors that may have led to an incorrect value of either the heat of formation (Mg2+ or MgO) or the calorimeter constant.
  • Conclusion
    • Reiterate the major experimental data.
  • The completed Excel file

5 attachmentsSlide 1 of 5

UNFORMATTED ATTACHMENT PREVIEW

Part A Step 2: Mass of Dry Calorimeter (g) Step 2: Mass of Calorimeter + Tap water (g) o Step 3: Temperature of hot water ( C) Step 3: Mass 250 mL beaker + 50 mL water (g) Step 6: Mass of wet 250 mL beaker (g) Trial 1 Trial 2 Trial 3 30.4433 79.9574 79.2333 79.9998 50.4 51.4 52.2 168.5765 158.6677 164.0002 119.7699 110.2404 115.2630 Part A Trial 1 36 34 Temperature (oC) 32 30 28 26 24 22 20 0 100 200 300 400 500 600 700 800 900 1000 Time (s) Part A Trial 2 38 36 Temperature (oC) 34 32 30 28 26 24 22 20 0 100 200 300 400 Time (s) 500 600 700 800 Part A Trial 3 36 34 Temperature (oC) 32 30 28 26 24 22 20 0 100 200 300 400 Time (s) 500 600 700 Part B Reaction of Mg with HCl Volume of 1 M HCl added (mL) Mass of Mg (g) Trial 1 98.0 0.4921 Trial 2 98.4 0.4937 Reaction of MgO with HCl Volume of 1 M HCl added (mL) Mass of MgO (g) Trial 1 99.1

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This exercise asks you to collect, organize, analyze, and evaluate data you collected in the lab. You will type a lab report that includes the following: 

  • Title page
  • Objective
  • Introduction
    • Give the logic of the experiment.
    • Be sure to define key terms and all applied experimental equations (e.g. calorimetry, calorimeter, enthalpy of formation, heat capacity of calorimeter, heat, balanced chemical equations, Hess’ law, and percent error.).
  • Procedure Reference
    • If there are any changes to the published procedure be sure to note them here.
  • Results and Calculations section
    • Table summarizing
      • Your major experimental data (e.g. heat capacity of calorimeter, experimental heat of formation for Mg2+ & MgO, actual heat of formation for Mg2+ & MgO, and percent error)
      • Be sure to include the PDF with the data that you were provided when you turn in your report. 
    • Graphs
      • Since data was given to you, you can use the graphs that were provided.  You do not need to make graphs.  Just paste them into the appropriate section of the report.
  • One sample calculation of each type.
  • Discussion
    • We did not record the boiling and freezing point of water experimentally. But issues with these measurements could possibly be something that would cause error in this experiment.  Perhaps something related to this would provide one of your sources of error?
    • State the heat of formation for MgO and describe any errors that may have led to an incorrect value of either the heat of formation (Mg2+ or MgO) or the calorimeter constant.
  • Conclusion
    • Reiterate the major experimental data.
  • The completed Excel file

5 attachmentsSlide 1 of 5

UNFORMATTED ATTACHMENT PREVIEW

Part A Step 2: Mass of Dry Calorimeter (g) Step 2: Mass of Calorimeter + Tap water (g) o Step 3: Temperature of hot water ( C) Step 3: Mass 250 mL beaker + 50 mL water (g) Step 6: Mass of wet 250 mL beaker (g) Trial 1 Trial 2 Trial 3 30.4433 79.9574 79.2333 79.9998 50.4 51.4 52.2 168.5765 158.6677 164.0002 119.7699 110.2404 115.2630 Part A Trial 1 36 34 Temperature (oC) 32 30 28 26 24 22 20 0 100 200 300 400 500 600 700 800 900 1000 Time (s) Part A Trial 2 38 36 Temperature (oC) 34 32 30 28 26 24 22 20 0 100 200 300 400 Time (s) 500 600 700 800 Part A Trial 3 36 34 Temperature (oC) 32 30 28 26 24 22 20 0 100 200 300 400 Time (s) 500 600 700 Part B Reaction of Mg with HCl Volume of 1 M HCl added (mL) Mass of Mg (g) Trial 1 98.0 0.4921 Trial 2 98.4 0.4937 Reaction of MgO with HCl Volume of 1 M HCl added (mL) Mass of MgO (g) Trial 1 99.1

Do you similar assignment and would want someone to complete it for you? Click on the ORDER NOW option to get instant services at LindasHelp.com