Advertisements
Advertisements
Question
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 )
Advertisements
Solution
Given:
Mass of Ag deposited = 1.346 x 10-3 kg
Time (t) = 3.5 min = 3.5 x 60s
Molar mass of Ag = 108 x 10-3 kg mol-1
To find:
Quantity of electricity required in coulomb:
Formulae:
1. Mole ratio = `"Moles of product formed in half reaction"/"Moles of electrons required in half reaction"`
2. Mass of the substance produced = `["I(A)" xx"t(s)"]/[96500"(C/mol e-)" xx "Mole ratio" xx "Molar mass of substance"]`
3. Quantity of electricity in coulomb (Q) = I ( in amp ) x t( in sec )
Calculation:
The half reaction for the formation of Ag is,
\[\ce{ Ag_(aq)^+ + e^- -> Ag_(s)}\]
From formula (1),
Mole ratio = `"Moles of Ag"/"Moles of electrons"`
= `[1( "mol Ag" )]/[1 ("mol" e^-)]`
= 1 mol Ag/mol e-
From formula (2),
1.346 x 10-3
= `(I xx 3.5 xx 60)/( 96500 ) xx 1 xx 108 xx 10^-3`
∴ I = `( 1.346 xx 10-3 xx 96500)/(3.5 xx 60 xx 108 xx 10^-3)`
= `[ 129889 xx 10^-3]/[22680 xx 10^-3]`
= 5.727 A
From formula (3),
Q = It = 5.727 x 3.5 x 60 = 1202.67 C
∴ The quantity of electricity required is 1202.67 C.
APPEARS IN
RELATED QUESTIONS
The charge of how many coulomb is required to deposit 1.0 g of sodium metal (molar mass 23.0 g mol-1) from sodium ions is -
- 2098
- 96500
- 193000
- 4196
Write any four applications of electrochemical series
Following reactions occur at cathode during the electrolysis of aqueous sodium chloride solution:
Na+(aq) + e− ⟶ Na (s) E0 = 2.71 V
H+(aq) + e− ⟶ `1/2` H2 (g) E0 = 0.00 V
On the basis of their standard reduction electrode potential (E0) values, which reaction is feasible at the cathode and why?
Suggest a list of metals that are extracted electrolytically.
How much charge is required for the following reduction?
1 mol of Cu2+ to Cu.
How much charge is required for the following reduction:
1 mol of \[\ce{MnO^-_4}\] to Mn2+?
A solution of Ni(NO3)2 is electrolysed between platinum electrodes using a current of 5 amperes for 20 minutes. What mass of Ni is deposited at the cathode?
Write any two uses of H2SO4
What is the ratio of volumes of H2 and O2 liberated during electrolysis of acidified water?
(A) 1 : 2
(B) 2 : 1
(C) 1 : 8
(D) 8 : 1
State second law of electrolysis
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)
Write the name of the cell which is generally used in transistors. Write the reactions taking place at the anode and the cathode of this cell.
How many faradays of electricity are required to produce 13 gram of aluminium from aluminium chloride solution? (Given: Molar mass of Al = 27.0-gram mol–1)
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 ?
Solve the following question.
A steady current of 2 amperes was passed through two electrolytic cells X and Y connected in series containing electrolytes FeSO4 and ZnSO4 until 2.8 g of Fe deposited at the cathode of cell X. How long did the current flow? Calculate the mass of Zn deposited at the cathode of cell Y.
(Molar mass : Fe = 56 g mol–1, Zn = 65.3 g mol–1, 1F = 96500 C mol–1)
According to Faraday’s First Law of Electrolysis, the amount of chemical reaction which occurs at any electrode during electrolysis by a current is proportional to the ____________.
In the electrolysis of aqueous sodium chloride solution which of the half cell reaction will occur at anode?
What will happen during the electrolysis of aqueous solution of \[\ce{CuSO4}\] by using platinum electrodes?
(i) Copper will deposit at cathode.
(ii) Copper will deposit at anode.
(iii) Oxygen will be released at anode.
(iv) Copper will dissolve at anode.
Aqueous copper sulphate solution and aqueous silver nitrate solution are electrolysed by 1 ampere current for 10 minutes in separate electrolytic cells. Will the mass of copper and silver deposited on the cathode be same or different? Explain your answer.
Assertion: Electrolysis of NaCl solution gives chlorine at anode instead of O2.
Reason: Formation of oxygen at anode requires overvoltage.
Time Required to deposite one millimole of aluminium metal by the passage of 9.65 ampere through aqueous solution of aluminium is
When during electrolysis of a solution of AgNO3, 9650 coulombs of charge pass through the electroplating bath, the mass of silver deposited on the cathode will be ______.
Given `1/a` = 0.5 CM–1, R = 50 ohm, N = 1.0 then equivalent conductance of electrolytic cell is
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 ______.
How much electricity in terms of Faraday is required to produce 40.0 g of Al from molten Al2O3?
(Given: Molar mass of Aluminium is 27 g mol−1.)
