हिंदी

On Calculating the Strength of Current in Amperes If a Charge of 840c (Coulomb) Passes Through an Electrolyte in 7 Minutes, It Will Be

Advertisements
Advertisements

प्रश्न

On calculating the strength of current in amperes if a charge of 840C (coulomb) passes through an electrolyte in 7 minutes, it will be

  • 1
  • 2
  • 3
  • 4
Advertisements

उत्तर

type 1

A = C/s

∴ A = 840/(7 × 60)

∴ A = 840/420

∴ A = 2

type 2

2
Q =I × t
840= I × 420
I =2 A

shaalaa.com
  क्या इस प्रश्न या उत्तर में कोई त्रुटि है?
2015-2016 (March)

APPEARS IN

वीडियो ट्यूटोरियलVIEW ALL [1]

संबंधित प्रश्न

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.)


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?


If a current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons would flow through the wire?


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+.


On passing 1.5 F charge, the number of moles of aluminium deposited at cathode are _______ [Molar mass of Al = 27 gram mol–1]

(A) 1.0

(B) 13.5

(C) 0.50

(D) 0.75


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


Explain Faraday’s 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 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 )


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.


What will happen during the electrolysis of aqueous solution of CuSO4 in the presence of Cu electrodes?

(i) Copper will deposit at cathode.

(ii) Copper will dissolve at anode.

(iii) Oxygen will be released at anode.

(iv) Copper will deposit at anode.


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


On electrolysis of dilute sulphuric acid using platinum electrodes, the product obtained at the anode will be ______.


The quantity of electricity needed to separately electrolyse 1 M solution of ZnSO4, AlCl3, and AgNO3 completely is in the ratio of ______.


What is the quantity of electricity in Coulombs required to produce 4.8 g of Mg from molten MgCl2? How much Ca will be produced if the same amount of electricity was passed through molten CaCl2? (Atomic mass of Mg = 24 u, atomic mass of Ca = 40 u).


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 ______.


On passing electricity through nitrobenzene solution, it is converted into azobenzene. The mass of azobenzene is ______ mg, if the same quantity of electricity produces oxygen just sufficient to burn 96 mg of fullerene (C60)·


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×