How many moles of Pt may be deposited on the cathode when 0.80F of electricity is passed through a 1.0M solution of Pt4+?
A
0.1 mol
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B
0.2 mol
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C
0.4 mol
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D
0.6 mol
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Solution
The correct option is C0.2 mol
Faraday's First Law of Electrolysis states that only, According to this law, the chemical deposition due to the same flow of current through an electrolyte is directly proportional to the quantity of electricity (coulombs) passed through it.
We have the reaction,
Pt4++4e−→Pt
So, 4 moles of electricity or 4F of electricity is required to deposit 1 mole of Pt
⟹0.80F of electricity will deposit 14×0.80=0.20mol