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

ur answer would be b hope i let me know if it is right

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