Nickel can be plated from aqueous solution according to the following half reaction. How long would it take (in min) to plate 29.6 g of nickel at 4.7 A?

Ni2 + (aq) + 2 e - - -> Ni (s) 3.5*10^2 min

(A) 5.9 * 10^2 min

(B) 1.7 * 10^2 min

(C) 6.2 * 10^2 min

(D) 4.8 * 10^2 min

It take 3.5 * 10² min

Explanation:

Step 1: Data given

Mass of the nickel = 29.6 grams

4.7A

Step 2: The balanced equation

Ni2 + (aq - + 2e - → Ni (s)

Step 3: Calculate time

W = (ItA) / (n*F)

⇒ W = weight of plated metal in grams = 29.6

⇒ I = current in coulombs per second. = 4.7

⇒ t = time in seconds.

⇒ A = atomic weight of the metal in grams per mole. = 58.69

⇒ n = valence of dissolved metal in solution in equivalents per mole. = 2

⇒ F = Faraday's constant in coulombs per equivalent. F = 96,485.309 coulombs/equivalent.

29.6 = (4.7 * t * 58.69) / (2*96485309)

t = 20707 seconds

t = 345 minutes = 3.5 * 10² min

It take 3.5 * 10² min