A silver wire is immersed in a solution containing ions of CU2 + what is expected in this situation?
A) no reaction occurs.
b) The silver wire is oxidized.
c) Copper is deposited on the silver wire.
D) The ions Cu2 + are reduced.
In this situation, we are dealing with a redox reaction, where oxidation and reduction occur simultaneously. To determine the expected outcome, we can use the standard reduction potentials of the two metals involved, silver (Ag) and copper (Cu).
The half-reaction for the reduction of Cu2+ to Cu is:
Cu2+ + 2e- → Cu(s)
The half-reaction for the oxidation of Ag to Ag+ is:
Ag(s) → Ag+ + e-
Comparing the standard reduction potentials of Cu2+ and Ag+, we find that Cu2+ has a greater tendency to be reduced (lower reduction potential) compared to Ag+. This means that Cu2+ ions will be more likely to accept electrons and get reduced.
Therefore, when a silver wire is immersed in a solution containing Cu2+ ions:
- The silver wire will be oxidized, as Ag atoms lose electrons and form Ag+ ions. This occurs because Cu2+ ions have a greater tendency to be reduced.
- Copper ions (Cu2+) from the solution will accept the electrons released from the silver wire and get reduced, resulting in the deposition of copper onto the silver wire.
Based on this information, the correct answer is (c) Copper is deposited on the silver wire.
In this situation, the expected outcome is that the ions Cu2+ will be reduced. Therefore, the answer is option (D) "The ions Cu2+ are reduced."
Look up the activity series.
A metal ABOVE in the activity series will deposit the metal (present as the ion) below it. If the reverse then there is no reaction.