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.
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