Question on: JAMB Chemistry - 2017
Calculate the amount in moles of silver deposited when 9650C of electricty is passed through a solution of silver salt [= 96500 Cmol-1]
A
0.05
B
10.80
C
10.00
D
0.10
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Correct Option: D
m = (\frac{Mm \times Q}{96500n
})
where Q = IT
M = Mm × (\frac{Q}{96500n})
where m = mass
Mm = Molar mass
Q = Quantity of electricity
n = number of change= +1
(\frac{M}{Mm}) = mole = (\frac{mass}{Molarmass})
(\frac{M}{Mm}) = (\frac{Q}{96500n})
= (\frac{9650}{96500n}) × 1
= (\frac{1}{10}) = 0.1mol
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