Which substance in this redox reaction is the oxidizing agent?
$Cu+2 AgNO_3 \rightarrow 2 Ag+Cu\left(NO_3\right)_2$
A. N
B. $AgNO _3$
C. Cu
D. $NO _3{ }^{-}$
E. $Cu \left( NO _3\right)_2$
Answer (1)
The oxidizing agent is the substance that is reduced. In the reaction C u + 2 A g N O 3 i g h t ha r p oo n u p 2 A g + C u ( N O 3 ) 2 , silver ions ( A g + ) in A g N O 3 gain electrons and are reduced. Therefore, the oxidizing agent is A g N O 3 .
Explanation
Identifying the Oxidizing Agent In this redox reaction, we need to identify the oxidizing agent. The oxidizing agent is the substance that gets reduced, meaning it gains electrons. Let's analyze the oxidation states of the elements involved.
Analyzing Oxidation States Copper (Cu) starts with an oxidation state of 0 and ends up with +2 in C u ( N O 3 ) 2 . This means copper loses electrons (oxidation). Silver (Ag) in A g N O 3 starts with an oxidation state of +1 and ends up with 0 as elemental Ag. This means silver gains electrons (reduction). Nitrate ( N O 3 − ) remains as N O 3 − , so its oxidation state does not change.
Determining the Oxidizing Agent Since silver ions ( A g + ) in A g N O 3 are reduced, A g N O 3 is the oxidizing agent.
Examples
Redox reactions are crucial in many real-world applications, such as batteries, corrosion, and industrial processes. For example, in a battery, a redox reaction generates electricity through the transfer of electrons from one substance to another. Identifying oxidizing and reducing agents helps us understand and control these processes, leading to innovations in energy storage, material science, and environmental protection.
