The oxidizing agent gains electrons and is reduced. In the reaction C u + 2 A g N O 3 → 2 A g + C u ( N O 3 ) 2 , silver ( A g ) is reduced from +1 to 0 oxidation state. Therefore, A g N O 3 is the oxidizing agent. The answer is A g N O 3 .
Explanation
Understanding the Problem We are asked to identify the oxidizing agent in the given redox reaction: C u + 2 A g N O 3 → 2 A g + C u ( N O 3 ) 2 . The oxidizing agent is the substance that gains electrons and gets reduced in the reaction.
Determining Oxidation States To identify the oxidizing agent, we need to determine the oxidation states of each element in the reactants and products.
Identifying Changes in Oxidation States In the reaction: C u + 2 A g N O 3 → 2 A g + C u ( N O 3 ) 2 :
Copper (Cu) changes from an oxidation state of 0 to +2.
Silver (Ag) changes from an oxidation state of +1 to 0.
Nitrate ( N O 3 − ) remains as a spectator ion.
Identifying the Oxidizing Agent Since silver (Ag) is reduced (gains electrons, oxidation state decreases from +1 to 0), the substance containing silver, which is A g N O 3 , is the oxidizing agent.
Conclusion Therefore, the oxidizing agent in the given redox reaction is A g N O 3 .
Examples
In redox reactions, identifying oxidizing and reducing agents is crucial in various applications, such as batteries, corrosion prevention, and industrial chemical processes. For example, understanding how silver nitrate acts as an oxidizing agent helps in designing silver-based batteries or in controlling silver deposition processes. This concept is also fundamental in environmental science, where redox reactions are involved in pollutant degradation and water treatment.