To determine the quantity of electricity required to deposit 180g of Ag (silver) from molten silver trioxonitrate(V), we need to understand the concept of electrolysis. During electrolysis, a metal can be deposited according to Faraday's laws of electrolysis.
The equivalent weight of a substance is calculated by dividing the atomic mass by the valency. For silver (Ag), the atomic mass is given as 108 and the valency of silver in AgNO3 is 1. This makes the equivalent weight of Ag 108 g/equivalent.
According to Faraday's first law of electrolysis:
Mass of substance deposited = (Equivalent weight × Quantity of electricity (in coulombs) ) / Faraday's constant (96500 C/mol)
Let's calculate the number of equivalents of silver deposited:
Number of equivalents of Ag = Mass of Ag / Equivalent weight = 180 g / 108 g/equivalent = 5/3 equivalents
The quantity of electricity required to deposit 1 equivalent of a substance is 1 Faraday (F) = 96500 C.
Therefore, the total quantity of electricity required:
Quantity of electricity = Number of equivalents × Faraday's constant
Quantity of electricity = (5/3 equivalents) × 1 F = 5/3 F = 1.67 F
Therefore, 1.67 Faraday is required to deposit 180g of Ag from a molten silver trioxonitrate(V).