Theory Questions – Electrolysis II

1. (a) Sketch to illustrate Faraday’s first law of electrolysis.

(b) Describe how you investigate Faraday’s first law of electrolysis using copper(II) tetraoxosulphate(VI) solution and copper electrodes.

2. Calculate the number of Faraday’s of electricity required to liberate:

(a) 16.2 g of silver 

(b) 14.3 g of aluminum

(c) 2.24 dm³ of oxygen gas at STP

(d) 0.23mole of hydrogen molecule

[Ag = 108, Al = 27, molar volume = 22.4 dm³ at stp]

3. Determine the mass of copper deposited by 4.0 moles of electrons in the reaction represented by the equation: Cu²⁺ + 2e^–  → Cu_(s) [Cu = 64]

4. How long would it take to deposit 0.08 g of copper from CuCl₂ solution by passing a current of 0.5