1. Use Faraday’s law of electrolysis
   For the same quantity of electricity passing through the cell, the mass deposited or dissolved is proportional to the electrochemical equivalent:

$m = ZQ$

So, for zinc and copper in the Daniell cell,

$\frac{m_{Cu}}{m_{Zn}} = \frac{Z_{Cu}}{Z_{Zn}}$

2. Given data

• Loss in mass of zinc pole: $m_{Zn} = 0.13\,g$
• Electrochemical equivalent of zinc: $Z_{Zn} = 32.5$
• Electrochemical equivalent of copper: $Z_{Cu} = 31.5$

We need mass gained by copper pole:

$m_{Cu} = m_{Zn}\cdot \frac{Z_{Cu}}{Z_{Zn}}$

3. Substitute values

$m_{Cu} = 0.13 \times \frac{31.5}{32.5}$

$m_{Cu} = 0.13 \times 0.96923$

$m_{Cu} \approx 0.126\,g$

4. Match with options The correct option is:

$\boxed{\text{C: }0.126\,g}$

5. Comparison with stored answer
   Stored correct answer: C
   Derived answer: C
   They agree.