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When an iron nail is dipped into a copper sulphate solution, which substance gets displaced?
Copper
Copper Sulphate
Sulphate
Iron
Copper
When an iron nail is dipped into a blue-coloured copper sulphate solution (CuSO4тАЛ), iron being more reactive than copper displaces copper from the solution. As a result, metallic copper is deposited on the iron nail, and the blue solution turns green due to the formation of ferrous sulphate (FeSO4тАЛ).
When an iron nail is dipped into a blue-coloured copper sulphate solution (CuSO4тАЛ), iron being more reactive than copper displaces copper from the solution. As a result, metallic copper is deposited on the iron nail, and the blue solution turns green due to the formation of ferrous sulphate (FeSO4тАЛ).
Think of a playground game where a stronger, more athletic student (iron) easily replaces a less aggressive student (copper) from a particular spot on the field, forcing the less active student to step aside and wait outside.
Remember the Reactivity Series using the sentence: 'Please Send Cats, Monkeys And Zulus In Lead Cages Securely Managed' (Potassium, Sodium, Calcium, Magnesium, Aluminium, Zinc, Iron, Lead, Copper, Silver, Gold). Iron comes well above copper!
Fe+CuSO4тАЛтЖТFeSO4тАЛ+Cu тАФ Displacement reaction of copper by iron
Reactivity Order: Fe>Cu тАФ Iron is more reactive than copper
This is a classical example of a single displacement reaction (or metal displacement reaction). According to the reactivity series of metals, a more reactive metal can displace a less reactive metal from its salt solution. Since iron (Fe) is placed above copper (Cu) in the reactivity series, it readily loses electrons to form Fe2+ ions, while Cu2+ ions in solution gain those electrons to precipitate as solid copper metal (Cu). The chemical equation is represented as: Fe(s)+CuSO4тАЛ(aq)тЖТFeSO4тАЛ(aq)+Cu(s).
Iron is more reactive than copper, allowing it to undergo a displacement reaction.
The blue color of copper sulphate fades and gradually turns green due to the formation of iron(II) sulphate (FeSO4тАЛ).
A reddish-brown layer of solid copper metal gets deposited on the surface of the iron nail.
This reaction illustrates the principles of oxidation-reduction (redox) chemistry.
Demonstrates the relative reactivities of metals clearly in laboratory settings.
Provides visual confirmation of redox processes through distinct color changes.
Reaction rate depends on surface impurities and concentration of the solution.
Qualitative rather than quantitative for general educational demonstration.
Extraction and purification of metals in metallurgy.
Understanding galvanic and electrochemical cells.
Standard electrode potentials dictate that iron (E0=тИТ0.44┬аV) is a stronger reducing agent than copper (E0=+0.34┬аV).
Option A (Copper) is correct because copper is displaced from its aqueous salt solution by iron.
A is correct тАФ Copper gets displaced from the copper sulphate solution by the more reactive iron nail.
Always verify metal reactivity positions from the electrochemical series before predicting whether a displacement reaction will occur.
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