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

b..

is the correct one

explanation:

covalent bonds form as valence electrons are shared between two atoms. lewis structures and structural formulas are common ways of showing the covalent bonding in organic molecules. formal charge describes the changes in the number of valence electrons as an atom becomes bonded into a molecule.