When CU reacts with`AgNO_(3)` solution , the reaction takes place is f:

Options

A. Oxidation of Cu
B. Reducing of Cu
C. Oxidation Of Ag
D. Raducing of `No_(3)^(-)`

Explanation

To solve the question "When Cu reacts with AgNO₃ solution, what reaction takes place?", we can follow these steps:

### Step 1: Identify the Reactants
We have two reactants: Copper (Cu) and Silver Nitrate (AgNO₃).

### Step 2: Understand the Electrochemical Series
In the electrochemical series, metals are arranged based on their standard reduction potentials. A higher reduction potential indicates a greater tendency to gain electrons (be reduced). In this case, Copper (Cu) is above Silver (Ag) in the series, which means that Ag⁺ ions have a higher tendency to be reduced compared to Cu²⁺ ions.

### Step 3: Determine the Reaction
When Cu reacts with AgNO₃, the Ag⁺ ions in the solution will be reduced to solid silver (Ag), while Cu will be oxidized to Cu⁺ ions. The half-reactions can be written as:

1. Reduction half-reaction:
\[ Ag^+ + e^- \rightarrow Ag \]

2. Oxidation half-reaction:
\[ Cu \rightarrow Cu^+ + e^- \]

### Step 4: Combine the Half-Reactions
To combine the half-reactions, we ensure that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction. In this case, one electron is involved in both half-reactions, so we can add them directly:

\[ Cu + Ag^+ \rightarrow Cu^+ + Ag \]

### Step 5: Write the Overall Reaction
The overall reaction when Cu reacts with AgNO₃ can be summarized as:
\[ Cu + 2AgNO_3 \rightarrow Cu(NO_3)_2 + 2Ag \]

### Conclusion
The final products of the reaction are Copper(II) Nitrate (Cu(NO₃)₂) and solid Silver (Ag).