Final answer:
The student's question involves using Faraday's laws of electrolysis to calculate the mass of nickel deposited from a solution during electroplating, based on the given current and time duration.
Step-by-step explanation:
The question is about the amount of nickel metal deposited from a solution containing Ni₂⁺⁺ ions during electroplating when a specific current is applied for a set amount of time. This involves using Faraday's laws of electrolysis to convert the electric charge passed through the solution into moles of nickel, and then into grams. First, we can calculate the total charge (Q) using the formula Q = It, where I is the current in amperes and t is the time in seconds. Here, 0.661 amperes of current is used for 46.5 minutes (which should be converted to seconds).
Once the charge is known, Faraday's constant (96,485 coulombs/mole of electrons) can help us find the number of moles of electrons, using the equation: moles of electrons = Q / (n * F), where n is the number of moles of electrons required to deposit one mole of nickel metal (which is 2 due to the Ni₂⁺⁺ ion). Finally, by knowing the atomic mass of nickel, which is approximately 58.69 grams/mol, we can find the mass of deposited nickel by multiplying the moles of nickel by this atomic mass.