Composition of a Copper Sulfate Hydrate Lab

Hydrate Before and After Heating:
Before heating 

After heating
Calculations:
(Our balance only read up to 3 sig figs for the percent error, so we just used 3 sig figs)

5a) My answer is 0.0144321931 mol for the moles of water evaporated. I found this by multiplying the grams of water evaporated by the conversion factor of 1 mole/18.01528g (the molar mass of H2O).
5b) My answer is 0.0033832679 mol for the moles of CuSO4 that remain in evaporating dish. I found this by first subtracting the mass of the evaporating dish by the mass of the evaporating dish and remaining anhydrous salt, and got 0.54g. I then multiplied the 0.54g by the conversion factor of 1 mol/159.6096g (the molar mass of CuSO4).
5c) To find the ratio of moles of CuSO4 to moles of H2O I divided 0.0144321931 mol and 0.0033832679 mol by the smallest, which was 0.0033832679 mol. 0.0033832679 mol/0.0033832679 mol was 1, while 0.0144321931 mol/0.0033832679 mol was approximately 4. 
5d) Based off of our final calculations in 5c, the empirical formula of the hydrate is 1 CuSO4 x 4 H2O.

Percent Error

Our percent error was 9.72%. We might have made errors due to our rushed experiment because of the limited amount of time we had. I predict that our predicted coefficient on water is lower than the actual value.



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