Advertisements
Advertisements
प्रश्न
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
उत्तर
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
संबंधित प्रश्न
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
96500 coulombs correspond to the charge on how many electrons?
Write any four applications of electrochemical series
Using the E° values of A and B, predict which is better for coating the surface of iron [E°(Fe+2/Fe) = -0.44V] to prevent corrosion and why?
Given: E° (A+2/A)=-2.37 V: E°(B+2/B)= -0.14V
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 Al3+ to Al.
How much charge is required for the following reduction?
1 mol of Cu2+ to Cu.
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?
Draw neat labelled diagram of electrolytic refining of blister copper
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)
Electrolytic cell uses electrical energy to bring about ____________.
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.
Consider the figure and answer the following question.
Cell ‘A’ has ECell = 2V and Cell ‘B’ has ECell = 1.1V which of the two cells ‘A’ or ‘B’ will act as an electrolytic cell. Which electrode reactions will occur in this cell?
Time Required to deposite one millimole of aluminium metal by the passage of 9.65 ampere through aqueous solution of aluminium is
The quantity of electricity needed to separately electrolyse 1 M solution of ZnSO4, AlCl3, and AgNO3 completely is in the ratio of ______.
Assertion (A): During electrolysis of aqueous copper sulphate solution using copper electrodes hydrogen gas is released at the cathode.
Reason (R): The electrode potential of Cu2+/Cu is greater than that of H+/H2.
Select the most appropriate answer from the options given below:
