What is the time required for depositing all the silver present in 125 ml of1M agno3 solution by passing a current of 241.25 amperes

Dear Ramakrishna,

Given i=241.25 A

Volume= 125 mL

Molarity= 1M

According to Faraday's first law of electrolysis,      w= z*i*t

where,     w is the mass of metal deposited on the electrode

i is the current passed

t is the time taken

z is the electrochemical equivalent of the metal.

In this problem, the metal is silver.

Molarity= (Weight of metal/Molecular weight)/Vol(L)

1 = (w/108)*1000/125

108=w*8

w= 13.5 g.

Charge passed= it= 241.25*t

Equivalents of charge= 241.25t/96500

Equivalent weight= 13.5*96500/241.25t

= 5400/t

108=5400/t

t= 50 s.

Dear Ramakrishna,

Given i=241.25 A

Volume= 125 mL

Molarity= 1M

According to Faraday's first law of electrolysis,      w= z*i*t

where,     w is the mass of metal deposited on the electrode

i is the current passed

t is the time taken

z is the electrochemical equivalent of the metal.

In this problem, the metal is silver.

Molarity= (Weight of metal/Molecular weight)/Vol(L)

1 = (w/108)*1000/125

108=w*8

w= 13.5 g.

Charge passed= it= 241.25*t

Equivalents of charge= 241.25t/96500

Equivalent weight= 13.5*96500/241.25t

= 5400/t

108=5400/t

t= 50 s.