Why would copper (II) sulfate solution react with iron to produce 3 CuSO4(aq) + 2 Fe (s) = 3 Cu (s) + Fe2(SO4)3 (aq)
Because Iron is a more active metal than copper, ie, it is easier to lose its outer electrons.
Copper (II) sulfate solution reacts with iron to produce copper and iron (III) sulfate according to the following chemical equation:
3 CuSO4(aq) + 2 Fe(s) -> 3 Cu(s) + Fe2(SO4)3(aq)
To understand why this reaction occurs, we need to consider the reactivity series of metals. The reactivity series arranges metals in order of their reactivity, with the most reactive metals at the top and the least reactive metals at the bottom.
In this case, copper is less reactive than iron. When copper (II) sulfate solution comes into contact with iron, a redox reaction takes place. The iron atoms react with the sulfate ions in the copper (II) sulfate solution, displacing the copper atoms.
Here's a step-by-step breakdown of the reaction:
1. The iron atoms (Fe) in solid form (s) react with the copper (II) sulfate solution (CuSO4(aq)).
2. The iron (Fe) atoms oxidize, losing two electrons each, and are converted into Fe2+ ions.
Fe(s) -> Fe2+(aq) + 2e-
3. The copper (II) ions (Cu2+) in the solution are reduced and gain two electrons each, forming copper atoms (Cu) as a solid precipitate.
Cu2+(aq) + 2e- -> Cu(s)
4. The sulfate (SO4) ions remain unchanged and stay in solution.
The overall reaction can be summarized as follows:
3 Cu2+(aq) + 2 Fe(s) -> 3 Cu(s) + 2 Fe3+(aq) + 3 SO4^2-(aq)
So, the copper (II) sulfate solution reacts with iron to produce solid copper and iron (III) sulfate in solution.
It's important to note that this reaction occurs because copper is higher in the reactivity series than hydrogen but lower than iron. Therefore, copper can displace iron from its compound, resulting in the formation of copper and a new compound with iron.
I hope this explanation helps! Let me know if you have any further questions.