Enthalpy of Formation of Magnesium Oxide Calorimetry
After performing the MgO Calorimetry Experiment, you should follow the guidelines for a Quantitative Report as well as this information.
This lab report will be turned in in TWO separate pieces.
- "Everything Except the Discussion" - Staple all of these together
- Cover page
- Sample calculations of cells: C12, C14, C19, C22, D25, C35, C40, C41, C71, C73, C81, D81
- Three MicroLab Plots:
- NCR pages
- Three copies of a Draft of the MgO Calorimetry Discussion - Do not Staple - Do not put your name on the front.
- Again: Do not put your name on the front of the pages. Write your name on the back of the printed copy (after you print it, by hand, is fine).
- In general, follow the guidelines presented for a standard quantitative lab report Discussion. Below are notes that will help you in completing that Discussion.
- Present your results. These should include the quantities that you determined fairly directly (Ccal, ΔH1, ΔH2) as well as those that you derived (enthalpies of formation of Mg2+ and MgO).
- Compare your results for the enthalpies of formation of Mg2+ and MgO to the literature values. In your comparison, be sure to utilize the sizes of your errors and the sizes of your uncertainties (in other words, quantitatively compare your results to literature values).
- Simple calorimetry experiments like this usually yield an enthalpy of reaction value that is too small in magnitude. Give one reason why this might be the case.
- Given that both of your experimental measurements (ΔH1 and ΔH2) are likely to be too small in magnitude, explain why the error in the quantity that involves both experiments (enthalpy of formation of MgO) is usually much smaller than the error in the quantity that involves just one experiment (enthalpy of formation of Mg2+).