How many coulombs of electricity would liberate 1.08g of Ag from a solution of silver salt?

[Ag = 108.0; 1F = 96500 C]

Mopest

1 year ago

To solve this problem, we need to use the concept of Faraday's law of electrolysis.

First, let's calculate the number of moles of silver (Ag) deposited:

Moles of Ag = mass of Ag / molar mass of Ag
= 1.08 g / 108.0 g/mol
= 0.01 mol

Since 1 mole of electrons (1 Faraday, F) deposits 1 mole of a monovalent ion like silver, we need:

1 Faraday (F) = 96500 C to deposit 1 mole of Ag

So, to deposit 0.01 moles of Ag:

Coulombs required = 0.01 mol × 96500 C/mol
= 965 C

The correct answer is:

C. 965 C