Copper Sulfate and Iron Lab Report
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Copper Sulfate and Iron Lab Report
Trevin.G Tue Mar 13, 2012 7:31 pm
This is only for things that have been solved.
For how the iron bonds/what to say about oxidation states:
[solved]: when the iron wants to bond, it loses its electrons, and these become free floating electrons. Then it bonds with the SO4. The electrons lost by the iron get absorbed by the copper, making it neutral. Therefore, this is a redox reaction - the iron gets oxidized (loses electrons) and the copper gets reduced (gains electrons). It is also a single replacement reaction
For MSDS's:
[SOLVED]
MSDS's NEEDED: Water, Iron, Copper sulfate, Copper, Iron (II) Sulfate
INFORMATION NEEDED: What the chemical can do, How to not let it do anything to you, What to do if it does do something to you. Also Disposal and Storage Information.
How did we know how much Copper Sulfate to use?
[SOLVED] It was an arbitrary amount. We used Basic stoich. 1g of iron is about .03 mols of iron. therefore, we need to figure out how many mols of CuSO4 were needed in both reactions. The larger number of mols of CuSO4 was found to be 4.8 grams which was rounded to 5 grams. In order to ensure that it was in excess, we doubled the 5 grams to 10. Another reason we doubled it was because the teachers knew about the hydrate, and we didn't take that into account, so when we doubled we would have excess, even counting the hydrate. The larger number of moles of CuSO4 came from the reaction where Iron (III) was used, because then we had a 2:3 Fe to CuSO4 molar ratio rather than the 1:1 if we had Iron (II)
For how the iron bonds/what to say about oxidation states:
[solved]: when the iron wants to bond, it loses its electrons, and these become free floating electrons. Then it bonds with the SO4. The electrons lost by the iron get absorbed by the copper, making it neutral. Therefore, this is a redox reaction - the iron gets oxidized (loses electrons) and the copper gets reduced (gains electrons). It is also a single replacement reaction
For MSDS's:
[SOLVED]
MSDS's NEEDED: Water, Iron, Copper sulfate, Copper, Iron (II) Sulfate
INFORMATION NEEDED: What the chemical can do, How to not let it do anything to you, What to do if it does do something to you. Also Disposal and Storage Information.
How did we know how much Copper Sulfate to use?
[SOLVED] It was an arbitrary amount. We used Basic stoich. 1g of iron is about .03 mols of iron. therefore, we need to figure out how many mols of CuSO4 were needed in both reactions. The larger number of mols of CuSO4 was found to be 4.8 grams which was rounded to 5 grams. In order to ensure that it was in excess, we doubled the 5 grams to 10. Another reason we doubled it was because the teachers knew about the hydrate, and we didn't take that into account, so when we doubled we would have excess, even counting the hydrate. The larger number of moles of CuSO4 came from the reaction where Iron (III) was used, because then we had a 2:3 Fe to CuSO4 molar ratio rather than the 1:1 if we had Iron (II)
Last edited by Trevin.G on Tue Mar 13, 2012 8:00 pm; edited 1 time in total
Trevin.G- Posts : 1
Join date : 2011-12-12
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