complete the statement about the redox reaction below: Al3+(aq)+2Ag(s)+CL-(aq)—-Al(s)+3AgCl(s)
_is being oxidized. ___ is being reduced. is acting as an reducing agent. is acting as an oxidizing agent. _________moles of electrons are transferred. the reaction is an _________cell
The correct answer and explanation is :
Complete the statement:
- Silver (Ag) is being oxidized.
- Aluminum ion (Al³⁺) is being reduced.
- Silver (Ag) is acting as a reducing agent.
- Aluminum ion (Al³⁺) is acting as an oxidizing agent.
- 3 moles of electrons are transferred.
- The reaction is an electrochemical cell (galvanic or voltaic cell).
Explanation:
A redox (reduction-oxidation) reaction involves the transfer of electrons from one species to another. In this reaction:
[
\text{Al}^{3+}(aq) + 2Ag(s) + Cl^-(aq) \rightarrow \text{Al}(s) + 3AgCl(s)
]
we analyze the oxidation states of each species:
- Al³⁺ (aq): The aluminum ion has a +3 oxidation state.
- Ag (s): Silver is in its elemental form, so its oxidation state is 0.
- Cl⁻ (aq): Chloride ion remains -1 in the reaction.
- Al (s): Aluminum in solid form has an oxidation state of 0.
- AgCl (s): Silver chloride consists of Ag⁺ and Cl⁻, where silver has an oxidation state of +1.
Identifying Oxidation and Reduction:
- Oxidation is the loss of electrons. In this reaction, silver (Ag) is oxidized as it goes from Ag (0) → Ag⁺ (+1) in AgCl.
- Reduction is the gain of electrons. Al³⁺ gains electrons to become Al (0), meaning aluminum ions are reduced.
Agents:
- The reducing agent is the substance that loses electrons. Here, Ag (silver) loses electrons, making it the reducing agent.
- The oxidizing agent is the substance that gains electrons. Here, Al³⁺ gains electrons, making it the oxidizing agent.
Number of Electrons Transferred:
- Since Al³⁺ is reduced by gaining 3 electrons to become Al(s), and each Ag atom loses 1 electron, a total of 3 moles of electrons are transferred.
Type of Electrochemical Cell:
This is an electrochemical (galvanic) cell because it is a spontaneous reaction, generating electrical energy.
Now, I will generate an image representing this redox reaction.
Here is an illustrated diagram of the redox reaction, showing the oxidation and reduction processes, electron transfer, and the roles of the oxidizing and reducing agents. Let me know if you need any modifications or further explanations!