Iron and Cupric Sulfate
Lab Report
A Mole Lab That Actually Works!
Conducted by: Tyler Bishop and Erica Bowman
2nd Period
April 27th 2015
Ashland County West Holmes Career Center
Mrs. Bender
1
Background
Iron powder will react with cupric sulfate in a onetoone ratio (1 mole to 1 mole). The students will also be able to more easily visualize the size of a mole of iron and copper. The result obtained in this lab usually have less than a one percent error.
Fe(s) +
CuSO4 (aq)
> FeSO4(aq) + Cu(s)
Iron powder cupric sulfate ferrous sulfate copper
In the reaction, iron will be the limiting reagent; it will be completely used up in the reaction.
Cupric sulfate will be in excess; not all of it will be used up in the reaction. The number of moles of iron that react will equal the number of moles of copper produced. The reaction indicates the
1:1 ratio between the iron and copper.
The occurrence of the reaction will be obvious since the blue cupric sulfate solution turns green due to the iron going into the solution. Copper metal is noticeably forming on the bottom.
If the cupric sulfate solution is warm, the reaction occurs almost instantaneously.
This lab can also be used to illustrate a single replacement reaction and oxidationreduction. As a single replacement reaction, iron replaces the copper in cupric sulfate to produce ferrous sulfate and copper metal. As a oxidationreduction reaction, the copper in cupric sulfate is reduced and the iron powder is oxidized. (Copper goes from a +2 oxidation state to a zero oxidation state while iron goes from a zero oxidation state to a +2 oxidation state.)
2
Purpose Statement We will determine the meaning of a mole and stoichiometry relations using oxidationreduction and single replacement reaction. We will determine the reaction that iron powder has with cupric sulfate in a onetoone ratio.
Materials
Cupric Sulfate pentahydrate, (CuSO4 x 5H2O,
A Mole Lab That Actually Works!
Conducted by: Tyler Bishop and Erica Bowman
2nd Period
April 27th 2015
Ashland County West Holmes Career Center
Mrs. Bender
1
Background
Iron powder will react with cupric sulfate in a onetoone ratio (1 mole to 1 mole). The students will also be able to more easily visualize the size of a mole of iron and copper. The result obtained in this lab usually have less than a one percent error.
Fe(s) +
CuSO4 (aq)
> FeSO4(aq) + Cu(s)
Iron powder cupric sulfate ferrous sulfate copper
In the reaction, iron will be the limiting reagent; it will be completely used up in the reaction.
Cupric sulfate will be in excess; not all of it will be used up in the reaction. The number of moles of iron that react will equal the number of moles of copper produced. The reaction indicates the
1:1 ratio between the iron and copper.
The occurrence of the reaction will be obvious since the blue cupric sulfate solution turns green due to the iron going into the solution. Copper metal is noticeably forming on the bottom.
If the cupric sulfate solution is warm, the reaction occurs almost instantaneously.
This lab can also be used to illustrate a single replacement reaction and oxidationreduction. As a single replacement reaction, iron replaces the copper in cupric sulfate to produce ferrous sulfate and copper metal. As a oxidationreduction reaction, the copper in cupric sulfate is reduced and the iron powder is oxidized. (Copper goes from a +2 oxidation state to a zero oxidation state while iron goes from a zero oxidation state to a +2 oxidation state.)
2
Purpose Statement We will determine the meaning of a mole and stoichiometry relations using oxidationreduction and single replacement reaction. We will determine the reaction that iron powder has with cupric sulfate in a onetoone ratio.
Materials
Cupric Sulfate pentahydrate, (CuSO4 x 5H2O,