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...

Answer Details

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.