The purpose should be comprehensive for both part I and part II. This section should include the various topics covered throughout the experiment. The procedure section must cite the lab manual, since this is where someone wanting to repeat your experiment could get all needed information.

Now that the lab manual is online there is a slightly different method of citation:

In MLA style, the components are arranged this way:

Author. "Document Title." Publication or Web site title . Date of publication. Date of access <URL>.

Example of MLA style:
Dillon, Stephanie. “A Submarine Adventure: Density Saves the Day.” CHM1045L Online Manual. Fall 2006. 24 January 2007 <http://www.chem.fsu,edu/chemlab/chm1045lmanual/density/index.html>.

Also be sure to note any changes that are made during lab to the procedure in the lab manual.

The data section should include the following for part I: In table format, (a) the five DT values for the unknown liquids studied (DT= T_final – T_initial), where the initial temperature is room temperature and the final temperature is that recorded for each liquid. (b) based on the DT value, the rankings of the unknown liquids in terms of their intermolecular forces from strongest to weakest. Recall from the background section for this lab that evaporation is an endothermic process that results in a drop in temperature; therefore the compounds with the largest temperature decrease or have the lowest minimum temperature exhibit the weakest intermolecular forces. (c) Finally be sure to identify the five unknown liquids using your knowledge of intermolecular forces and the heat of vaporization values you found in the pre-lab.

For part II, report all of the observations made during lab of the CO₂ alone and inside your micro gauge. Report the triplet point of CO₂ found during lab. 

There are no calculations for part I. For part II you must determine the experimental value for the triplet point of CO₂. The triple point of CO₂ can be found using Boyle’s Law, a variation of the ideal gas law, and solving for P₂.

                                         

Boyle's Law                 P₁V₁ = P₂V₂

 

In this equation P₁is the pressure of the room, measured using the barometer in the balance room. V₁ is the total volume (length) of the micro gauge and V₂ is the final volume read from the micro gauge at the triplet point (the distance of the food coloring from the top of the gauge). Both V₁ and V₂ in this experiment can be used in the Boyle’s Law equation as distances (see Background for explanation), therefore V₁ is the total length of the micro gauge and V2 is the measured distance of the food coloring from the top of the micro gauge..  P₂ is the unknown variable, the pressure at the observed triplet point. In order to solve for P₂ you must rearrange Boyle’s Law in terms of P₂.

Once the value of P₂ is known the percent error of your micro gauge can be determined using the following:

     

The experimental value is P₂ and the accepted value is the triplet point found on the phase diagram of CO₂. Make sure the units for both triplet points are the same before calculating percent error. The conclusion section should be several paragraphs addressing the following: For part I, the identity of the five unknown liquids with an explanation supporting the identification made. A discussion of the similarities and differences of your rankings compared to the heat of vaporization ranking done in the pre-lab. For Part II, summarize the observations of CO₂ made; state and compare the actual and experimental values for the triplet point of CO₂ including the percent error. Finally discuss any errors in the experiment.

QUESTIONS:

2. In our use of the microgauge to determine the triple point pressure of CO₂, we only measure the height change (distance the dye moves) in the gauge not the actual volume. Why does this approximation not ruin our results?