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...

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.