JAMB Chemistry 2017 Objective — Question 14
Question 14 of 40 from the Joint Admissions and Matriculation Board (JAMB) Chemistry 2017 Objective paper, with the correct answer and a full explanation.
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Calculate the mass of copper deposited when a current of 0.5 ampere is passed through a solution of copper(II) chloride for 45 minutes in an electrolytic cell (Cu=64, F=96500Cmol⁻¹).
- A. A. 0.300g
- B. B. 0.250g
- C. C. 0.224g
- D. D. 0.448gCorrect
Explanation
Q=It=(0.5x2700)=1350C. Cu²⁺+2e⁻→Cu, so 1 mole Cu (64g) requires 2F=193,000C. Mass deposited = (64/193000)x1350 ≈ 0.448g.
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