Copper Iron Stoichiometry Lab Report
Copper-Iron Stoichiometry
Lab Report
10/3/12
Abstract:
The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-
CuSO4(aq) + Fe(s) Cu(s) + FeSO4(aq)
Introduction:
There were several purposes of this lab, the main ones were limiting reagent analysis, quantitative and analytical analysis, and techniques like vacuum filtration and weighing by difference. The main focus of the lab was the oxidation-reduction reaction between Copper Sulfate and Iron Powder and there were two possible reactions based on the charge of iron once it gets oxidized by copper. The two possible balanced reactions are –
CuSO4 (aq) + Fe(s) Cu(s) + FeSO4 (aq) [I]
3CuSO4 (aq) + 2Fe(s) 3Cu(s) + Fe2(SO4)3(aq) [II]
Through the possible reactions, one of the best way to determine which one is the correct reaction pertaining to the lab is limiting reagent analysis, where mass of copper is quantitatively determined or by observations. Through the process of weighing by difference as suggested by the lab manual, anhydrous copper sulfate and iron powder were weighed out. Anhydrous copper sulfate was then dissolved in water on a hot plate and iron was added after the solution of copper sulfate had cooled down to room temperature. The addition of iron took place under the fume hood so as to avoid inhalation of sulfur fumes which were released as a side-product of this reaction. Copper precipitate was then collected by the use of a vacuum
Lab Report
10/3/12
Abstract:
The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-
CuSO4(aq) + Fe(s) Cu(s) + FeSO4(aq)
Introduction:
There were several purposes of this lab, the main ones were limiting reagent analysis, quantitative and analytical analysis, and techniques like vacuum filtration and weighing by difference. The main focus of the lab was the oxidation-reduction reaction between Copper Sulfate and Iron Powder and there were two possible reactions based on the charge of iron once it gets oxidized by copper. The two possible balanced reactions are –
CuSO4 (aq) + Fe(s) Cu(s) + FeSO4 (aq) [I]
3CuSO4 (aq) + 2Fe(s) 3Cu(s) + Fe2(SO4)3(aq) [II]
Through the possible reactions, one of the best way to determine which one is the correct reaction pertaining to the lab is limiting reagent analysis, where mass of copper is quantitatively determined or by observations. Through the process of weighing by difference as suggested by the lab manual, anhydrous copper sulfate and iron powder were weighed out. Anhydrous copper sulfate was then dissolved in water on a hot plate and iron was added after the solution of copper sulfate had cooled down to room temperature. The addition of iron took place under the fume hood so as to avoid inhalation of sulfur fumes which were released as a side-product of this reaction. Copper precipitate was then collected by the use of a vacuum
References: 1Agrawal, Abhinash; Tratnyek, Paul, Reduction of Nitro Aromatic Compounds by Zero-Valent Iron Metal, Environ. Sci. Technol., 1995, 30 (1), pg. 153–160 http://pubs.acs.org/doi/abs/10.1021/es950211h. 2 An Introduction to Chemical Systems in the Laboratory, Hayden-McNeil, University of Illinois, Urbana-Champaign, 2012, Pg. 9-16 3 An Introduction to Chemical Systems in the Laboratory, Hayden-McNeil, University of Illinois, Urbana-Champaign, 2012, Pg. 11 4Donaldson, Ian, How to make Copperas (Iron Sulfate) from Pyrites, Encyclopedia Chemistry, http://www.juliantrubin.com/encyclopedia/chemistry/copperas.htm (accessed 9/29/12)