Get the information you need with the help of IDNLearn.com's expert community. Get comprehensive and trustworthy answers to all your questions from our knowledgeable community members.
The current required to plate out 2.96 g of nickel from the solution of Ni²⁺ in 27.12 minutes is 5.95 A
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
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
I = Q / t
I = 9682.71 / 1627.2
I = 5.95 A
Learn more about Faraday's law:
https://brainly.com/question/24795850
The current required to plate out 2. 96 g of nickel from a solution of ni2 in 27. 12 minutes is 5.95 ampere.
Current is a charged particle moving through an electrical conductor.
The equation is [tex]\rm Ni^2^+ + 2e = Ni[/tex]
step 1: calculate the mass of Ni
Molar mass of Ni is 59 g/mol
59 × 1 = 59 g
Step2: calculate the number of Faraday
no. of Faraday is 2F
1 Faraday = 96500 C
then, 2 Faraday is equal to 2 × 96500 = 193000 C
Step 3: calculate the quantity of electricity
59 g of Nickel is deposited by, 193000 C of electricity
So, for 2.96 g of nickel
[tex]\dfrac{2. 96\;g \times 193000}{59} = 9682.71 \;C[/tex]
Step4: calculate the current:
Electricity Q = 9682.71 C
Time = [tex]27.12 \times 60 = 1627.2 \;s[/tex]
To find current
[tex]I = \dfrac{Q}{t} \\\\I = \dfrac{9682.71 }{1627.2}\\I = 5.95 A[/tex]
Thus, the current required is 5.95 ampere.
Learn more about current
https://brainly.com/question/13076734
#SPJ4