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zinc iodine will be produced with the mass of the compound remaining largely the same before the reaction with its individual parts. From the masses of the compounds, I will be able to figure out the empirical formula of zinc iodide.Assigned Synthesis NumberInitial Mass of Zinc (g)Initial Mass of Iodine (g)12.03.0Results and DiscussionMass of Zinc metal: 1.981g Mass of elemental Iodine: 2.993gMass of Zinc after dried up from dissolving in a Zinc Iodide mixture and slightly acidic water: 1.247g Mass of dried iodine solution: 4.2g Mass of Zinc + Iodine from part 1: 4.974gMass of Zinc Iodide solution after experiment: 5.447gZn: 22.89%/65.38= 0.35/0.35=1I: 77.11%/126.90= 0.61/0.35=1.74 approx: 2Empirical formula of Zinc Iodide: ZnI2All of the iodine that reacted with zinc had an initial starting phase as a flaky solid and started to change after 9 drops of 6 M acetic acid and 10 mL of deionized water was added to the zinc and iodine mixture with the solution turning into a rust color and heating up. It showed that the reaction was occurring and absorbing energy to help facilitate it. Furthermore the solution later turned nearly colorless after 10 minutes, showing the reaction was completed. The dried product of the zinc iodide solution was a grayish powder after removing the unreacted pieces of zinc. The original form of the elemental iodine was reduced to powder, showing that all of the iodine reacted with zinc to form a zinc iodide compound.
The graphical relationship of the mass of iodine reacted and the mass of zinc reacted is that most of the reactions occur at certain intervals. One gram of Iodine will mostly react with 0.200 to 0.300 grams of zinc, 2 grams of iodine will react mostly with