During the industrial electro-refining of copper, an electrolytic cell is set up as shown in the diagram below:
A constant current of 5.00 A is passed through the cell for 96.5 minutes96.5\text{ minutes}96.5 minutes.
(Faraday constant, F=96500 C mol−1F = 96500\text{ C mol}^{-1}F=96500 C mol−1; Ar(Cu)=63.5A_r(\text{Cu}) = 63.5Ar(Cu)=63.5; molar volume of gas at RTP = 24.0 dm3 mol-1)
Which of the following statements correctly describes the chemical or physical changes occurring in this electrolytic cell?
The mass of the cathode increases by 9.53 g9.53\text{ g}9.53 g.
The mass of the cathode increases by 19.1 g19.1\text{ g}19.1 g.
The concentration of Cu2+\text{Cu}^{2+}Cu2+ ions in the electrolyte decreases by 0.150 mol dm−30.150\text{ mol dm}^{-3}0.150 mol dm−3.
A volume of 1.80 dm31.80\text{ dm}^31.80 dm3 of oxygen gas (measured at RTP) is evolved at the anode.
Electrolytic processes Questions
Practise Edexcel GCSE Chemistry Electrolytic processes with exam-style questions for Foundation and Higher tier. 100 questions, matched to the Edexcel GCSE Chemistry (1CH0) specification and written in Paper 1 and Paper 2 style. Every question includes a full worked solution and mark scheme, so you can see where marks are awarded rather than just whether you got the answer right.