Question

Calculate the time required in second to deposit 5.85 g Ni from \(\text{NiCl}_{2}\) solution by passing 10 A current (molar mass of Ni \(=58.5\ \text{g mol}^{-1}\))

• A. \(19.3\)
• B. \(193\)
• C. \(1930\)
• D. \(19300\)

Hint:

Find the moles of nickel, the charge needed at 2 faradays per mole, and then divide by the current.

Answer 1

The Correct Option is C

Step 1: Understanding the Concept
The reduction is \(\text{Ni}^{2+} + 2e^{-}\rightarrow\text{Ni}\), so 2 faradays deposit 1 mole of Ni.

Step 2: Charge needed
Moles of Ni \(= \dfrac{5.85}{58.5} = 0.1\ \text{mol}\).
Charge \(Q = 0.1\times 2\times 96500 = 19300\ \text{C}\).

Step 3: Calculation
\(t = \dfrac{Q}{I} = \dfrac{19300}{10} = 1930\ \text{s}\).

Final Answer:
The time required is 1930 seconds. \[ \boxed{\text{(C) }1930} \]