Nickel is electroplated from a NiSO₄ solution.A constant current of 5.50 amp is applied by an external power supply.How long will it take to deposit 100.g of Ni? The atomic mass of Ni is 58.69.

Question

Quizplus · Accepted Answer

To calculate the time required to deposit 100 g of nickel (Ni) through electroplating, we use Faraday's laws of electrolysis. The mass (m) deposited is related to the current (I), time (t), molar mass (M), and the charge number (n) (which is 2 for Ni, as it typically forms Ni^2+ ions) through the equation: $m = \frac{ItM}{nF}$, where F is Faraday's constant (96485 C/mol).Rearranging for time, we get: $t = \frac{mnF}{IM}$.Given:- m = 100 g = 0.100 kg (since the atomic mass of Ni is 58.69 g/mol, we convert the mass to kg to keep units consistent with the molar mass unit)- I = 5.50 A- M = 58.69 g/mol = 0.05869 kg/mol (to match the mass unit)- n = 2 (for Ni^2+)- F = 96485 C/molPlugging in the values: $t = \frac{0.100 \times 2 \times 96485}{5.50 \times 0.05869}$Calculating this gives a time in seconds, which can be converted to hours for comparison with the options provided.After performing the calculation, the result aligns with option A, 16.6 hours, as the correct time required to deposit 100 g of Ni through electroplating under the given conditions.

Nickel Is Electroplated from a NiSO4 Solution

Nickel Is Electroplated from a NiSO₄ Solution