Question

During the electrolysis of concentratedcopper(II) chloride solution using carbonelectrodes, 3.2 g of copper was deposited atthe cathode. Calculate the volume of chlorinegasevolved at the anode atS.I.P.[Cu 64,1F = 96,500C, Gaseous molarvolume = 22.4 dm' at s.t.p]​

a) 1.6 dm^3
b) 2.4 dm^3
c) 3.2 dm^3
d) 4.8 dm^3

Answer 1

To calculate the volume of chlorine gas evolved at the anode during the electrolysis of copper(II) chloride, we need to use Faraday's law of electrolysis and the balanced equation for the reaction. The volume of chlorine gas evolved at the anode is 2.4 dm³. The correct option is b).

Step-by-step explanation:

To solve this problem, we need to use Faraday's law of electrolysis, which states that the mass of a substance produced at an electrode is directly proportional to the amount of electric charge passed through the cell.

First, we need to calculate the amount of charge passed through the cell using the formula:

Charge (C) = Current (A) × Time (s)

Next, we convert the amount of copper deposited at the cathode from grams to moles using its molar mass (Cu = 63.5 g/mol). Then, using the balanced equation for the electrolysis of copper(II) chloride, we can find the volume of chlorine gas evolved at the anode at STP.

The volume of chlorine gas evolved at the anode is 2.4 dm³ (option b).