JAMB Chemistry 2018 Objective — Question 23
Question 23 of 36 from the Joint Admissions and Matriculation Board (JAMB) Chemistry 2018 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 was passed through a solution of copper (II) chloride for 45 minutes in an electrolytic cell [Cu=64, F=96500 Cmol⁻¹]
- A. 0.300g
- B. 0.250g
- C. 0.224gCorrect
- D. 0.448g
Explanation
Charge Q = It = 0.5×(45×60) = 1350C. Moles of electrons = Q/F = 1350/96500. Cu²⁺+2e⁻→Cu, so moles Cu = ½×(1350/96500). Mass = moles×64 ≈ 0.224g.
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