A solution of Ni(NO3)2 is electrolyzed between platinum electrodes using 0.1 Faraday electricity. How many mole of Ni…

Strategy: Use Faraday's Law to relate the amount of electricity (in Faradays) to the moles of metal deposited. Identify the valen\ce ($z$) of the Nickel ion from the given formula.

Step 1: Determine the charge on Nickel From $\ce{Ni(NO3)_2}$, the nickel ion is $\ce{Ni^{2+}}$. The reduction half-reaction is: $\ce{Ni^{2+} + 2e^- \rightarrow Ni(s)}$ This means 2 moles of electrons ($2\ \mathrm{F}$) are required to deposit 1 mole of Nickel.

Step 2: Calculate moles for 0.1 Faraday $n_{\ce{Ni}} = \frac{\text{Quantity of electricity}}{\text{Valen\ce of ion}} = \frac{0.1\ \mathrm{F}}{2\ \mathrm{F/mol}}$ $n_{\ce{Ni}} = 0.05\text{ mol}$

$\boxed{\text{Answer: (c) 0.05}}$