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
jamb 2017chemistry

The correct answer is D. 0.10

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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