Iron reacts with copper ions in solution, such as those found in copper sulfate (CuSO₄), through a single displacement reaction, resulting in the formation of copper metal and iron(II) sulfate (FeSO₄).
Here's a breakdown of the reaction:
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The Reaction: When iron metal (Fe) is placed in a copper sulfate solution (CuSO₄), iron atoms lose electrons and become iron ions (Fe²⁺), while copper ions (Cu²⁺) gain electrons and become copper metal (Cu).
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Chemical Equation: Fe(s) + CuSO₄(aq) → Cu(s) + FeSO₄(aq)
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Observations:
- The solid iron metal will gradually dissolve.
- The blue color of the copper sulfate solution will fade as copper ions are replaced by iron ions.
- A reddish-brown solid, metallic copper, will precipitate out of the solution and deposit on the surface of the iron.
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Why it Happens: This reaction occurs because iron is more reactive than copper. In terms of electrochemical potential, iron has a greater tendency to lose electrons and form ions compared to copper. Therefore, iron can displace copper from its ionic state.
In summary, iron reacts with copper ions in solution to produce copper metal and iron(II) ions in solution. This is a single displacement reaction driven by the difference in reactivity between iron and copper.
