Home
Class 11
CHEMISTRY
(A) 1 faraday = 96,500 coulomb. It is ...

(A) 1 faraday = 96,500 coulomb.
It is a charge of 1 mole electrons.
(R) 1 faraday charge liberates one gram equivalent of substance at an electrode.

A

Both (R) and (A) are true and reason is the correct explanation of assertion.

B

Both (R) and (A) are true but reason is not correct explanation of assertion

C

Assertion (A) is true but reason (R) is false

D

Assertion (A) and reason (R) both are false

Text Solution

Verified by Experts

The correct Answer is:
B
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • MISCELLANEOUS (TOPICS OF GENERAL INTEREST)

    OP TANDON|Exercise SET-V: Matching type Questions|37 Videos

  • MISCELLANEOUS (TOPICS OF GENERAL INTEREST)

    OP TANDON|Exercise SET-VI: Problems on graphical aptitude|53 Videos

  • MISCELLANEOUS (TOPICS OF GENERAL INTEREST)

    OP TANDON|Exercise SET-III: Single Digit Answer Type Questions|20 Videos

  • INTRODUCTION TO ORGANIC CHEMISTRY

    OP TANDON|Exercise SINGLE INTEGER ANSWER TYPE|4 Videos

  • OXIDATION AND REDUCTION (REDOX REACTIONS)

    OP TANDON|Exercise SECTION V|3 Videos

Similar Questions

Explore conceptually related problems

1 faraday = _____ coulombs

The electric charge for electrode deposition of one gram equivalent of a substance is:

Knowledge Check

  • One gram equivalent of a substance is liberated at an electrode by

    A
    `6.22xx10^(23)` electrons
    B
    96500 C
    C
    1 amp of current for one second
    D
    1 amp current for 96500 C

  • One gram equivalent of a substance is liberated at an electrode by :

    A
    `6.023 xx 10^(23)` electrons
    B
    `96500 C`
    C
    1 amp current for 1 second
    D
    1 amp current for 96500 sec

  • The charge required to liberate one gram equivalent of an element is

    A
    96 500 F
    B
    1 F
    C
    1 C
    D
    none of these

    • Similar Questions

    Explore conceptually related problems

    The mass and charge of 1 mole electrons will be:

    Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolytic cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly propertional to the amount of charge passed through it. The mass of substance liberated at electrode is calculated using the following relation : m= ("ItE")/(96500) Here, E represents the equivalent mass and 96500 C is called the Faraday constant. Faraday (96500 C) is the charge of 1 mole electron, i.e., 6.023 xx 10^(23) electrons, it is used to liberate one gram equivalent of the substance. On electrolysis of dilute sulphuric acid using platinum electrodes, the product obtained at the anode will be :

    The electric charge for electrode deposition of one gram equivalent of a substance is

    The electric charge for electrode deposition of one gram equivalent of a substance is

    Electrolysis is the process in which electrical energy is converted to chemical energy. In electrolytic cell, oxidation takes place at anode and reduction at cathode. Electrode process depends on the electrode taken for electrolysis. Amount of substance liberated at an electrode is directly propertional to the amount of charge passed through it. The mass of substance liberated at electrode is calculated using the following relation : m= ("ItE")/(96500) Here, E represents the equivalent mass and 96500 C is called the Faraday constant. Faraday (96500 C) is the charge of 1 mole electron, i.e., 6.023 xx 10^(23) electrons, it is used to liberate one gram equivalent of the substance. Calculate the volume of gas liberated at the anode at STP during the electrolysis of a CuSO_(4) solution by a current of 1 A passed for 16 minutes and 5 seconds :

    Home
    Profile