The stoichiometry of electrolysis: the relationship between amountsof charge and

Question

The stoichiometry of electrolysis: the relationship between amountsof charge and product

What mass of silver (M.W. 107. 9 g/mole) will be formed when 15.0 Aare passed through molten AgCl for 25.0 minutes?
F= Faraday's constant = 9.65 x 10^4 C/mol e-
current x time = charge

correct answer: 25.2 g

please show me step by step how to solve this problem, explain asmuch as you can thank you :) !! I know you have to start w/writinga half-reaction but already I'm stuck not knowing to write it asoxidation or reduction?

Explanation / Answer

We Know that :    According to Faraday's Ist Law :      m = z x i x t      m = 107.9 g / mol / 1 x 96500 C / mol e * 15.0 A x 25.0 x 60s           = 25.15 g

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