What mass of Ag (At. Mass 108) could be plated on a spoon from electrolysis of `AgNO_(3)` solution by one ampere current for 10 minutes ?

Answer

To solve the problem of how much mass of silver (Ag) can be plated on a spoon from the electrolysis of an AgNO₃ solution using a current of 1 ampere for 10 minutes, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Given Data:**
- Current (I) = 1 A
- Time (t) = 10 minutes = 10 × 60 seconds = 600 seconds
- Atomic mass of Ag = 108 g/mol
- Number of electrons transferred (N) for Ag = 1
- Faraday's constant (F) = 96500 C/mol

2. **Calculate the Total Charge (Q):**
The total charge can be calculated using the formula:
\[ Q = I \times t \]
Substituting the values:
\[ Q = 1 \, \text{A} \times 600 \, \text{s} = 600 \, \text{C} \]

3. **Calculate the Mass of Silver Deposited:**
According to Faraday's law of electrolysis, the mass (m) of the substance deposited is given by:
\[ m = \frac{M \times Q}{N \times F} \]
Where:
- \( M \) = atomic mass of silver = 108 g/mol
- \( Q \) = total charge = 600 C
- \( N \) = number of electrons transferred = 1
- \( F \) = Faraday's constant = 96500 C/mol

Substituting the values:
\[ m = \frac{108 \, \text{g/mol} \times 600 \, \text{C}}{1 \times 96500 \, \text{C/mol}} \]

4. **Perform the Calculation:**
\[ m = \frac{64800}{96500} \approx 0.6715 \, \text{g} \]

5. **Conclusion:**
The mass of silver that could be plated on the spoon is approximately **0.6715 grams**.