Complete the statements about the redox reaction below. Al*(aq) + 3Ag(s) + 3Cl(aq) + Al(s) + 3AgCl(s) Half-reactions: AP+(aq) + 3e” – Al(s) E° = -1.66 V AgCl(s) + e – Ag(s) + Cl(aq) E = +0.22 V AgCl(s) 0 is being oxidized. 2 is being reduced electrolytic is acting as an reducing agent. Al(s) Ag(s) is acting as an oxidizing agent drag) voltaic AP(aq) moles of electrons are transferred. 3 The reaction is an) cell
The correct answer and explanation is:
Completion of the Statements:
- Al(s) is being oxidized.
- AgCl(s) is being reduced.
- Al(s) is acting as a reducing agent.
- Ag⁺(aq) is acting as an oxidizing agent.
- 3 moles of electrons are transferred.
- The reaction is a voltaic cell.
Explanation (300 Words)
A redox reaction involves the transfer of electrons between two species, where one undergoes oxidation (losing electrons) and the other undergoes reduction (gaining electrons).
In this reaction, Al(s) (solid aluminum) is oxidized to Al³⁺(aq) by losing three electrons: Al(s)→Al³⁺(aq)+3e−\text{Al(s)} \rightarrow \text{Al³⁺(aq)} + 3e⁻
The standard reduction potential of aluminum is -1.66 V, which means it has a strong tendency to lose electrons and act as a reducing agent.
Meanwhile, silver chloride (AgCl(s)) undergoes reduction, as silver ions (Ag⁺(aq)) gain electrons to form solid silver: AgCl(s)+e−→Ag(s)+Cl⁻(aq)\text{AgCl(s)} + e⁻ \rightarrow \text{Ag(s)} + \text{Cl⁻(aq)}
The reduction potential for this half-reaction is +0.22 V, indicating that Ag⁺ prefers to gain electrons and be reduced. Since Ag⁺(aq) is gaining electrons, it is the oxidizing agent.
The number of electrons exchanged per aluminum atom is 3, meaning that 3 moles of electrons are transferred in this reaction.
Since the overall cell potential is positive (calculated as E° = 0.22 V – (-1.66 V) = +1.88 V), the reaction is spontaneous and can function as a voltaic cell (not electrolytic). A voltaic cell generates electrical energy from a spontaneous chemical reaction.
In summary:
- Aluminum is oxidized, acting as the reducing agent.
- Silver ions are reduced, acting as the oxidizing agent.
- The reaction is spontaneous and occurs in a voltaic cell.