Respuesta :
Answer: Copper is getting oxidized and is a reducing agent. Silver is getting reduced and is oxidizing agent.
Explanation:
Oxidation reaction is defined as the reaction in which an atom looses its electrons. Here, oxidation state of the atom increases.
[tex]X\rightarrow X^{n+}+ne^-[/tex]
Reduction reaction is defined as the reaction in which an atom gains electrons. Here, the oxidation state of the atom decreases.
[tex]X^{n+}+ne^-\rightarrow X[/tex]
Oxidizing agents are defined as the agents which oxidize other substance and itself gets reduced. These agents undergoes reduction reactions.
Reducing agents are defined as the agents which reduces the other substance and itself gets oxidized. These agents undergoes reduction reactions.
For the given chemical reaction:
[tex]Cu(s)+2AgNO_3(aq.)\rightarrow 2Ag(s)+Cu(NO_3)_2(aq.)[/tex]
The half reactions for the above reaction are:
Oxidation half reaction: [tex]Cu(s)\rightarrow Cu^{2+}(aq.)+2e^-[/tex]
Reduction half reaction: [tex]2Ag^+(aq.)+2e^-\rightarrow 2Ag(s)[/tex]
From the above reactions, copper is loosing its electrons. Thus, it is getting oxidized and is considered as a reducing agent.
Silver is gaining electrons and thus is getting reduced and is considered as an oxidizing agent.
In the given redox reaction,
The oxidized substance is Cu(s)
The reduced substance is AgNO₃
The oxidizing agent is AgNO₃
The reducing agent is Cu(s)
From the question,
The given redox reaction is
Cu(s)+2AgNO3(aq)⟶2Ag(s)+Cu(NO3)2(aq)
The equation for the reaction can be written properly as
Cu(s) + 2AgNO₃(aq)⟶2Ag(s) + Cu(NO₃)₂(aq)
In order to identify the oxidized substance, the reduced substance, the oxidizing agent, and the reducing agent in the redox reaction,
First, we will define some of terms
Oxidizing agent
An oxidizing agent is substance which oxidizes something else. It gains electrons and is reduced in a chemical reaction. Therefore, an oxidizing agent is the reduced substance in a given chemical reaction.
Reducing agent
A reducing agent reduces other substances and loses electrons. It is oxidized in a chemical reaction. Therefore, a reducing agent is the oxidized substance in a given chemical reaction.
Oxidation
Oxidation can be defined as gain of oxygen. It can also be defined as an increase in oxidation state
Reduction
Reduction can be defines as loss of oxygen. It can also be defines as a decrease in oxidation state.
From the given reaction
The oxidation state of Cu increased from 0 to +2. This means Cu was oxidized.
(NOTE: The oxidation state of Cu in Cu(NO₃)₂ is +2)
∴ Cu(s) was oxidized and is the reducing agent
Also,
The oxidation state of Ag reduced from +1 to 0. This means Ag was reduced.
(NOTE: The oxidation state of Ag in AgNO₃ is +1)\
∴ AgNO₃ was reduced and it is the oxidizing agent
Hence, in the given redox reaction
The oxidized substance is Cu(s)
The reduced substance is AgNO₃
The oxidizing agent is AgNO₃
The reducing agent is Cu(s)
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