On passing 10 amperes of current for 50 minutes, 2.4 gm of a metal is deposited . The equivalent weight of the metal is
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The formula for equivalent weight : E
mass of metal deposited on electrode: m = 2.4 gms
current strength i = 10 A
time duration t = 50 min = 3, 000 sec.
charge = i t = 30, 000 Coulombs
96, 500 m = E * i * t
E = 96, 500 * m / ( i t ) = 96, 500 * 2.4 / 30, 000 = 7.72
The atomic weight if the metal is univalent : 7.72
The atomic weight if the metal is divalent : valency 2: 15.42
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alternate way to do the above exercise:
the charge : 10 A * 50 * 60 sec = 30, 000 Coulombs.
equivalent to 30, 000 /1.602 * 10⁻¹⁹ = 1.8726 * 10²³ protons. So this many ions with single charge on them have travelled to the electrode.
If the metal is a single charge carrying one (single valency) then:
weight of a metal ion : 2.4 gm / 1.8726 * 10²³ = 1.253 * 10⁻²³ gm
weight of one mole of metal ions : 1.253 * 10⁻²³ * 6.023 * 10²³ = 7.72
if the metal has valency 2 , then its atomic weight will be : 15.438
mass of metal deposited on electrode: m = 2.4 gms
current strength i = 10 A
time duration t = 50 min = 3, 000 sec.
charge = i t = 30, 000 Coulombs
96, 500 m = E * i * t
E = 96, 500 * m / ( i t ) = 96, 500 * 2.4 / 30, 000 = 7.72
The atomic weight if the metal is univalent : 7.72
The atomic weight if the metal is divalent : valency 2: 15.42
====================
alternate way to do the above exercise:
the charge : 10 A * 50 * 60 sec = 30, 000 Coulombs.
equivalent to 30, 000 /1.602 * 10⁻¹⁹ = 1.8726 * 10²³ protons. So this many ions with single charge on them have travelled to the electrode.
If the metal is a single charge carrying one (single valency) then:
weight of a metal ion : 2.4 gm / 1.8726 * 10²³ = 1.253 * 10⁻²³ gm
weight of one mole of metal ions : 1.253 * 10⁻²³ * 6.023 * 10²³ = 7.72
if the metal has valency 2 , then its atomic weight will be : 15.438
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