Understanding the Concepts
* Redox Reactions: Involve the transfer of electrons. Oxidation is the loss of electrons, and reduction is the gain of electrons.
* Activity Series: A list of metals arranged in order of their reactivity, with the most reactive at the top. This helps predict which metal will be oxidized and which will be reduced.
Applying the Concepts
1. Activity Series: Silver (Ag) is less reactive than copper (Cu). This means copper is more likely to lose electrons (oxidize) and silver is more likely to gain electrons (reduce).
2. Possible Reactions: There are two possible reactions:
* Reaction 1: Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)
* Copper (Cu) is oxidized to Cu²⁺.
* Silver ions (Ag⁺) are reduced to silver metal (Ag).
* Reaction 2: Ag(s) + Cu²⁺(aq) → No reaction
* This reaction is unlikely because silver is less reactive than copper.
Conclusion
The most likely redox reaction is:
Cu(s) + 2Ag⁺(aq) → Cu²⁺(aq) + 2Ag(s)
This reaction will occur because copper is more reactive than silver, and therefore more likely to donate electrons to the silver ions.
