The current required to plate out 2.96 g of nickel from the solution of Ni²⁺ in 27.12 minutes is 5.95 A
<h3>Balanced equation </h3>
We'll begin by writing the balanced equation showing the number of faraday required to plate nickel. This is given below
Ni²⁺ + 2e —> Ni
Molar mass of Ni = 59 g/mol
Mass of Ni from the balanced equation = 1 × 59 = 59 g
Number of faraday = 2 F
1 faraday = 96500 C
2 faraday = 2 × 96500 = 193000 C
SUMMARY
From the balanced equation above,
59 g of Nickel was deposited by 193000 C of electricity
<h3>How to determine the quantity of electricity </h3>
From the balanced equation above,
59 g of Nickel was deposited by 193000 C of electricity
Therefore,
2.96 g of Nickel will be deposited by = (2.96 × 193000) / 59 = 9682.71 C of electricity
<h3>How to determine the current </h3>
- Quantity of electricity (Q) = 9682.71 C
- Time (t) = 27.12 mins = 27.12 × 60 = 1627.2 s
- Current (I) =?
I = Q / t
I = 9682.71 / 1627.2
I = 5.95 A
Learn more about Faraday's law:
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