# Exercise 2 | Electrochemistry

What mass of nickel could be electroplated from a solution of nickel(II) chloride by a current of 0.480 A flowing for 12 hours?

m = $\frac{\mathrm{It}}{\mathrm{F}}$ x $\frac{\mathrm{M}}{{\mathrm{\nu }}_{\mathrm{e}}}$

m = mass deposited as Ni (in g)
I = current (in A)
t = time (in s) ⇒ 12 hours = 4.32 x 104 s
F = Faraday’s constant = 96485 C.mol-1
M = molar mass (in g.mol-1) ⇒ MNiCl2 = 129.6 g.mol-1
νe = stoichiometric coefficient of the electrons in the half reaction equation

Half reaction: Ni2+ (aq) + 2 e- → Ni (s)      [νe = 2]

m = $\frac{\mathrm{It}}{\mathrm{F}}$ x $\frac{\mathrm{M}}{{\mathrm{\nu }}_{\mathrm{e}}}$

m =

m = 6.31 g of NiCl2