The mass of silver deposited when a current of 10A is passed through a solution of silver salt for 4830s is
[Ag = 108, 1F = 96500 Cmol-1]
108.0g
54.0g
27.0g
13.5g
Explanation
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Answer= B;
Q=It, Q=10×4830, Q=48300 coulombs
Ag(positive) + e(negative) --->Ag
If -->108g ie.96500c=180g
therefore, 48300c will deposit = 108/96500 × 48300/1
=108×483/965
=54.06g
To solve this problem, we need to use the concept of electroplating and the relationship between the amount of substance deposited, the current, and the time.
The formula to calculate the mass of substance deposited is:
m = (Q x M) / (n x F)
where:
m = mass of substance deposited (in grams)
Q = total charge passed (in coulombs)
M = molar mass of the substance (in grams per mole)
n = number of electrons transferred per molecule
F = Faraday's constant (96500 C/mol)
Given values:
I = 10 A (current)
t = 4830 s (time)
M = 108 g/mol (molar mass of silver)
F = 96500 C/mol (Faraday's constant)
n = 1 (since silver is deposited as Ag+ ions, one electron is transferred per ion)
First, calculate the total charge passed:
Q = I x t = 10 A x 4830 s = 48300 C
Now, calculate the mass of silver deposited:
m = (Q x M) / (n x F)
= (48300 C x 108 g/mol) / (1 x 96500 C/mol)
= 54.0 g
The correct answer is B: 54.0g.
Guys check out this fomul.. In case of exam conditions.
M=RAM * T * I/Q * F
M = 108*4830*10/1*96500
M=54.06g.
Dear admin,point of correction sir:since silver(Ag)is divalent den it will require 2 * 96500=193,000c. Also using Q=IT,with d parameterz we were gven in d question Q=4830*10=48300c...since 193,000c deposit 108g(molar mass of silver),48300 will deposit 108 * 48300 everytin divided by 193,000.wc is equals to 27.0g.the only mistake u make is dat u dn't consider Ag(silver)to be divalent in order to multiply its heat required by 2
m/mm = it/nF
m=?
mm=108
I=10
t= 4830
n= Ag+1 = 1
F= 96500
m/108 = 4830× 10/96500×1
=m/108 = 48300/96500
CROSS MULTIPLY ✖️
96500m = 5,216,400
DBS by 96500
=5,216,400/96500
=54.0g(ANS)
