How many Faraday of electricity are required to deposit 0.20 mole of nickel, if 0.10 Faraday of electricity deposited 2.98g of nickel during electrolysis of...
Question 1 Report
How many Faraday of electricity are required to deposit 0.20 mole of nickel, if 0.10 Faraday of electricity deposited 2.98g of nickel during electrolysis of its aqueous solution?(Ni = 58.7, 1F = 96 500 C mol-)
Answer Details
We can use the equation:
moles of substance = electric charge (in Coulombs) / (Faraday's constant x charge per ion)
We are given that 0.10 Faraday of electricity deposited 2.98g of nickel. The molar mass of nickel is 58.7 g/mol, so 2.98g is equivalent to 0.0508 moles of nickel:
moles of Ni = 2.98g Ni / 58.7 g/mol = 0.0508 moles of Ni
Now, we can use the equation above to find out how many Faradays are required to deposit 0.20 moles of nickel:
0.20 moles of Ni = electric charge (in Coulombs) / (96,500 C/mol x 2)
electric charge (in Coulombs) = 0.20 moles of Ni x 96,500 C/mol x 2
electric charge (in Coulombs) = 38,600 C
Therefore, we need 0.40 Faraday of electricity to deposit 0.20 moles of nickel:
0.40 F = 38,600 C / 96,500 C/mol
So the answer is (C) 0.40.
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