मराठी
महाराष्ट्र राज्य शिक्षण मंडळएचएससी विज्ञान (सामान्य) इयत्ता १२ वी

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
  या प्रश्नात किंवा उत्तरात काही त्रुटी आहे का?
2015-2016 (March)

APPEARS IN

व्हिडिओ ट्यूटोरियलVIEW ALL [1]

संबंधित प्रश्‍न

Number of faradays of electricity required to liberate 12 g of hydrogen is:


Consider the reaction:

\[\ce{Cr2O^{2-}_7 + 14H+ + 6e- -> 2Cr^{3+} + 7H2O}\]

What is the quantity of electricity in coulombs needed to reduce 1 mol of  \[\ce{Cr2O^{2-}_7}\]?


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 \[\ce{MnO^-_4}\] 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


State second law of electrolysis


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 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 ?


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 )


Electrolytic cell uses electrical energy to bring about ____________.


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 ____________.


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.


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


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 ______.


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


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:


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.)


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×