Electroplating uses electrolysis to coat one metal with another. In a copper-plating bath, copper ions with a charge of 2ee move through the electrolyte from the copper anode to the cathode; the metal object to be plated.
If the current through the system is 1.2 A, how many copper ions reach the cathode each second?

1.2 A of current will send (3.744 × 10¹⁸) ions to the cathode per second.

Explanation:

According to Faraday's second law of electrolysis, the amount of ions/mass of substance deposited at an electrode depends on its equivalent weight.

For a divalent ion, it will require 2F of electricity per mole.

1 F = 96500 C

Amount of electricity that passes through the electrolyte per second = (magnitude of current) × (time) = It = (1.2 × 1) = 1.2 C

2F (2×96500C) of electricity will deposit 1 mole of Copper ions

That is,

193000 C of electricity will deposit 1 mole of Copper.

1.2 C will deposit (1.2×1/193000); 0.0000062176 mole of Copper.

1 mole of Copper contains (6.022 × 10²³) ions according to the Avogadro's constant.

0.0000062176 mole of Copper will contain (0.0000062176 × 6.022 × 10²³) ions = (3.744 × 10¹⁸) ions.

Therefore, 1.2 A of current will send (3.744 × 10¹⁸) ions to the cathode per second.

Hope this Helps!!!

6 cos 34, 6 sin 34 trig