A solution of is electrolyzed between platinum electrodes using 0.1 Faraday electricity. How many mole of Ni will be deposited at the cathode?

Question

A solution of  is electrolyzed between platinum electrodes using 0.1 Faraday electricity. How many mole of Ni will be deposited at the cathode?

Canvas Classes · Accepted Answer

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

Step 1: Determine the charge on Nickel
From , the nickel ion is .
The reduction half-reaction is:

This means 2 moles of electrons () are required to deposit 1 mole of Nickel.

Step 2: Calculate moles for 0.1 Faraday

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