Note: The blue bar graph represents the initial mass of Copper Sulfate and the red graph represents the final mass in grams.Trials 1-5 are displayed in the x-axis and mass on the y-axis.
Data Analysis
5). Judging from the observation of the data collection in Part I (table 1.2) it appears that there were several reactions that were reversible and some that weren’t. Copper Sulfate showed the most prevalent reversible reaction by returning to its natural blue color. However, the texture of the hydrate had transformed from small blue crystals to a smaller grain size. Cobalt Sulfate had similar characteristics beginning with large purple crystals which after being re-hydrated gained its original color back but also conceived several blue specs. Ferrous Sulfate underwent a complete transformation from a mix of white and green crystals to a purple/blue color. Sucrose perhaps was the most easily burnt substance and wasn’t able to rehydrate after the pressure and blockage that occurred while heating it.
7.) The trends that appear in the data table appear to have the final mass of Copper Sulfate be ⅔ the amount of the initial mass (refer to table 1.4 and 1.3).
8.) In trials 1-3, the mass lost by dehydrating averaged 45.33% and the mean is 36% (refer to graph
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This was achieved by comparing the different outcomes of heated hydrates once water was added to them. A reversible hydration resulted in a transition back to the same color, while an irreversible substance would have transitioned into something else or unchanged after being heated. By heating Copper Sulfate in three trials (and compared the results from two other groups as well) the mass lost by water was able to be calculated. With precise accuracy two trials showed just over 35% while the exact percent of water in Copper Sulfate is