Asked by sara
Will a reaction occur when solid copper (Cu) is added to a solution of iron sulfate (Fe(SO4))
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Answered by
GPT-5 mini
AI
No — copper metal will not displace iron(II) from FeSO4 under normal conditions.
Reason: the possible redox process would be
Cu(s) → Cu2+ + 2e− (oxidation)
Fe2+ + 2e− → Fe(s) (reduction)
Using standard potentials:
E°(Cu2+/Cu) = +0.34 V
E°(Fe2+/Fe) = −0.44 V
E°cell = E°(cathode) − E°(anode) = (−0.44) − (+0.34) = −0.78 V (negative),
so the reaction Cu(s) + Fe2+ → Cu2+ + Fe(s) is non‑spontaneous.
Note: if Fe(III) (Fe3+) or another oxidizing agent were present, copper can be oxidized (for example Cu + 2 Fe3+ → Cu2+ + 2 Fe2+ is spontaneous). But with plain FeSO4 (Fe2+) solution, no reaction occurs.
Reason: the possible redox process would be
Cu(s) → Cu2+ + 2e− (oxidation)
Fe2+ + 2e− → Fe(s) (reduction)
Using standard potentials:
E°(Cu2+/Cu) = +0.34 V
E°(Fe2+/Fe) = −0.44 V
E°cell = E°(cathode) − E°(anode) = (−0.44) − (+0.34) = −0.78 V (negative),
so the reaction Cu(s) + Fe2+ → Cu2+ + Fe(s) is non‑spontaneous.
Note: if Fe(III) (Fe3+) or another oxidizing agent were present, copper can be oxidized (for example Cu + 2 Fe3+ → Cu2+ + 2 Fe2+ is spontaneous). But with plain FeSO4 (Fe2+) solution, no reaction occurs.
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