96.5 C of electricity is used to completely deposit silver metal (Ag) from an aqueous solution in which the silver ion is present as Ag+(aq) - VCE - SSCE Chemistry - Question 9 - 2004 - Paper 1

To determine the relationship between the silver and copper deposited, we use Faraday's laws of electrolysis. Given that 96.5 C of electricity is required to deposit silver and copper ions, we find the moles of each metal deposited.

1. Moles of Silver Deposited: The silver ion (Ag+) has a valency of +1. Hence, the amount of silver deposited can be calculated using: $n(Ag) = \frac{Q}{F} = \frac{96.5}{96500} \approx 0.0010 \, \text{mol} \text{ (where } F = 96500 \, C/mol \text{)}$

2. Moles of Copper Deposited: The copper ion (Cu2+) has a valency of +2. Thus, for the same charge (96.5 C), the moles of copper deposited are: $n(Cu) = \frac{Q}{2F} = \frac{96.5}{2 \times 96500} \approx 0.0005 \, \text{mol}$

3. Comparison: From the calculations, the moles of silver deposited (0.0010 mol) is twice that of the moles of copper deposited (0.0005 mol). Therefore, the amount of silver metal deposited is indeed twice the mole of the copper deposited, leading us to conclude that the correct choice is:

D. be twice the mole of the copper deposited.