In the electrolysis of molten ZnCl2, how much Zn can be deposited at the cathode by the passage of 0.01 ampere for one hour?
Correct answer: C. 0.012 g
- A. 0.002 g
- B. 0.123 g
- C. 0.012 g
- D. 0.004 g
Explanation
In this scenario, we first find the total number of charges flown through the apparatus. The formula that we are going to be using is Charge= Ampere x Time. 1 mole of Zn is formed when we have two moles of electrons being added to 1 mole of Zn2+. 1 mole of electrons carries a charge of 96500 coulombs. So, 2 moles of electrons would have a charge of 193000C. To find the moles of Zn deposited, we have the charge passed divided by the charge required to form 1 mole of Zn. Once we have the moles, we multiply them by the molar mass. For a better understanding, please see the attached solution.
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