Advertisements
Advertisements
Question
Calculate the mass of Ag deposited at cathode when a current of 2 amperes was passed through a solution of AgNO3 for 15 minutes.
(Given : Molar mass of Ag = 108 g mol−1 lF = 96500 C mol−1)
Advertisements
Solution
t = 900 s
Charge = Current × Time = 2 A × 900 s = 1800 C
According to the reaction:
Ag+(aq) + e– = Ag(s)
We require 1F to deposit 1 mol or 108 g of Ag.
For 1800 C, the mass of Ag deposited = (108 g mol–1 × 1800 C)/(1 × 96500 C mol–1) = 2.0145 g.
APPEARS IN
RELATED QUESTIONS
96500 coulombs correspond to the charge on how many electrons?
How much electricity in terms of Faraday is required to produce 20 g of Ca from molten CaCl2?
(Given: Molar mass of Calcium is 40 g mol−1.)
Suggest a list of metals that are extracted electrolytically.
How much charge is required for the following reduction?
1 mol of \[\ce{MnO^-_4}\] to Mn2+.
Write any two uses of H2SO4
State second law of electrolysis
Following reactions occur at cathode during the electrolysis of aqueous copper(II) chloride solution :
On the basis of their standard reduction electrode potential (E°) values, which reaction is feasible at the cathode and why ?
How much quantity of electricity in coulomb is required to deposit 1.346 × 10-3 kg of Ag in 3.5 minutes from AgNO3 solution?
( Given: Molar mass of Ag is 108 × 10-3 kg mol-1 )
In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur at anode?
Through an aqueous solution of an unknown salt of metal M (M = 200 g/mol) a current of 1.93 A is passed for 50 min. If 4 g of metal is produced at cathode. The charge on metal ion in solution is ______.
