0.1 faraday of electricity deposited 2.95 g of nickel during electrolysis of an aqueous solution. Calculate the number of moles of nickel that will be depos...

The given information states that 0.1 faraday of electricity deposited 2.95 g of nickel during electrolysis of an aqueous solution. So, we can calculate the amount of nickel deposited per unit of electricity (per faraday) as follows: Amount of nickel deposited per faraday = 2.95 g / 0.1 F = 29.5 g/F Now, to calculate the number of moles of nickel deposited by 0.4 faraday, we can use the following formula: Amount of substance (in moles) = Mass / Molar mass where Mass is the amount of nickel deposited and Molar mass is the atomic weight of nickel (Ni = 58.7 g/mol). So, the number of moles of nickel deposited by 0.4 faraday can be calculated as follows: Amount of nickel deposited by 0.4 F = 29.5 g/F × 0.4 F = 11.8 g Number of moles of nickel deposited by 0.4 F = 11.8 g / 58.7 g/mol = 0.20 mol Therefore, the answer is 0.20. In summary, 0.1 faraday of electricity deposited 2.95 g of nickel, which means that 1 faraday will deposit 29.5 g of nickel. To calculate the number of moles of nickel deposited by 0.4 faraday, we multiply the amount of nickel deposited per faraday (29.5 g/F) by 0.4 F, which gives us 11.8 g of nickel. Then, we divide this mass by the molar mass of nickel (58.7 g/mol) to get the number of moles of nickel deposited, which is 0.20 mol.