A steady current of `1.5 A` flows through a copper voltameter for 10 min. If the electrochemical equivalent of copper is `30 xx 10^(-5) gC^(-1)`, the mass of copper deposited on the electrode will be

Options

A. 0.40 g
B. 0.50 g
C. 0.67 g
D. 0.27 g

Answer

To solve the problem of finding the mass of copper deposited on the electrode in a copper voltameter when a steady current flows through it, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Given Values:**
- Current (I) = 1.5 A
- Time (T) = 10 minutes
- Electrochemical equivalent of copper (Z) = \(30 \times 10^{-5} \, \text{g/C}\)

2. **Convert Time to Seconds:**
Since the time is given in minutes, we need to convert it to seconds for consistency with the current in amperes.
\[ T = 10 \, \text{minutes} \times 60 \, \text{seconds/minute} = 600 \, \text{seconds} \]

3. **Calculate the Total Charge (Q):**
The total charge (Q) can be calculated using the formula:
\[ Q = I \times T \]
Substituting the values:
\[ Q = 1.5 \, \text{A} \times 600 \, \text{s} = 900 \, \text{C} \]

4. **Use the Formula for Mass Deposited:**
According to Faraday's law of electrolysis, the mass (m) deposited is given by:
\[ m = Z \times Q \]
Substituting the values:
\[ m = (30 \times 10^{-5} \, \text{g/C}) \times 900 \, \text{C} \]

5. **Perform the Multiplication:**
\[ m = 30 \times 10^{-5} \times 900 = 27000 \times 10^{-5} \, \text{g} \]
Simplifying this:
\[ m = 2.7 \times 10^{-2} \, \text{g} = 0.27 \, \text{g} \]

6. **Final Result:**
The mass of copper deposited on the electrode is:
\[ \boxed{0.27 \, \text{g}} \]