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3 marksMole Concept

CSEC Chemistry · January 2007 · Paper 2 · Question 2(d)(ii)

A current of 5 amperes is passed for 2 hours during the electrolysis. Calculate the following:

Calculate the mass of copper deposited. [Relative Atomic Mass of Cu = 64, Faraday's constant = 96500 coulombs]

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Other parts of this question

  1. 2(a)(i)In order to adapt the electrolytic cell in Figure 1 for the purification of copper, what material may be used as the cathode?[3 marks]
  2. 2(a)(ii)In order to adapt the electrolytic cell in Figure 1 for the purification of copper, what material may be used as the anode?[1 mark]
  3. 2(a)(iii)In order to adapt the electrolytic cell in Figure 1 for the purification of copper, what material may be used as the electrolyte?[1 mark]
  4. 2(b)(i)As electrolysis proceeds, describe the changes expected to be observed at the cathode.[3 marks]
  5. 2(b)(ii)As electrolysis proceeds, describe the changes expected to be observed at the anode.[1 mark]
  6. 2(b)(iii)As electrolysis proceeds, describe the changes expected to be observed in the electrolyte.[1 mark]
  7. 2(c)(i)Write half-equations for the reactions occurring at the cathode.[2 marks]
  8. 2(c)(ii)Write half-equations for the reactions occurring at the anode.[1 mark]
  9. 2(d)(i)Calculate the quantity of electricity passed in coulombs.[2 marks]
  10. 2(e)In addition to extraction of metal from their compounds, electrolytic processes are also widely used to protect metals from corrosion, as well as to make them…[2 marks]

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