Concept:A metal can spontaneously displace another metal from its aqueous salt solution if it acts as a stronger reducing agent.
Solution:- The strength of a reducing agent is inversely proportional to its reduction potential. A smaller (more negative) reduction potential means a higher tendency to lose electrons (oxidize).
- Zinc has a standard reduction potential of \( -0.76 \text{ V} \).
- Copper has a standard reduction potential of \( +0.34 \text{ V} \).
- Because Zinc has a smaller reduction potential than Copper, solid Zinc will naturally oxidize, forcing the Copper ions in solution to reduce and precipitate out.
Why other options are incorrect:Option B is factually inverted (Zinc's potential is lower, not higher). Atomic number and general solubility are not the primary thermodynamic drivers for redox displacement.
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