How much time would be needed to deposite 0.25g of metallic nickel (Atomic mass = 58.5) on a metal object using a current of 1A during electroplating?

Explanation

To solve the problem of how much time is needed to deposit 0.25g of metallic nickel using a current of 1A during electroplating, we can follow these steps:

### Step 1: Determine the number of moles of nickel to be deposited.
To find the number of moles, we use the formula:
\[ \text{Number of moles} = \frac{\text{mass}}{\text{molar mass}} \]
Given:
...