Asked by sara
Will this reaction take place?
Ag + Fe(SO4) -->
All Answers 1
Answered by
GPT-5 mini
AI
No — no reaction will occur.
Reason: Ag is less reactive than Fe, so solid silver cannot displace Fe2+ from FeSO4. Using standard potentials:
- Ag+ + e− → Ag(s) E° = +0.80 V
- Fe2+ + 2e− → Fe(s) E° = −0.44 V
For the putative reaction Ag(s) + Fe2+ → Ag+ + Fe(s), E°cell = E°(reduction at cathode) − E°(reduction at anode) = (−0.44) − (+0.80) = −1.24 V (negative), so it is non‑spontaneous.
The spontaneous reaction is the reverse: Fe(s) + 2Ag+ → Fe2+ + 2Ag(s), which would occur if you put iron metal into a silver‑ion solution.
Reason: Ag is less reactive than Fe, so solid silver cannot displace Fe2+ from FeSO4. Using standard potentials:
- Ag+ + e− → Ag(s) E° = +0.80 V
- Fe2+ + 2e− → Fe(s) E° = −0.44 V
For the putative reaction Ag(s) + Fe2+ → Ag+ + Fe(s), E°cell = E°(reduction at cathode) − E°(reduction at anode) = (−0.44) − (+0.80) = −1.24 V (negative), so it is non‑spontaneous.
The spontaneous reaction is the reverse: Fe(s) + 2Ag+ → Fe2+ + 2Ag(s), which would occur if you put iron metal into a silver‑ion solution.
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