Answer:
Cu(s) + 2Ag⁺(aq) → 2Ag(s) + 2Cu²⁺ (aq)
Explanation:
Electrochemical cell -
Device used for the conversion of chemical energy to electrical energy is called electrochemical cell.
it is based on oxidation reduction reaction.
The electrochemical cell has three components , electrolytes and two electrodes,
Anode electrode is responsible for oxidation, and the cathode electrode is responsible for reduction.
In an electrochemical cell , the cell notation is written in a way , that first is the oxidation half is written followed by the reduction , which are separated by the salt bridge ,
hence , from the question , the cell notation is given as -
Cu ( s ) ∣ ∣ Cu 2 + ( aq , 0.0155 M ) ∥ ∥ Ag + ( aq , 1.50 M ) ∣ ∣ Ag ( s )
Hence , from the above reaction , the oxidation half cell and reduction half cell as given as -
Oxidation -
Cu (s)→ Cu ²⁺ (aq)
Reduction -
Ag⁺(aq) → Ag(s)
Now , balancing the reaction , by adding electrons on the required side -
Oxidation -
Cu(s) → Cu²⁺ (aq) + 2e⁻
Reduction -
Ag⁺(aq) + e⁻ → Ag(s)
The above reaction can also be written as -
2Ag⁺(aq) + 2e⁻ → 2Ag(s)
Now , to overall cell reaction can be written as adding the respective half cells and eliminating the electrons , i.e. ,
Cu(s) + 2Ag⁺(aq) → 2Ag(s) + 2Cu²⁺ (aq)
