0
You visited us 0 times! Enjoying our articles? Unlock Full Access!
Question

The electric charge for electrode deposition of 1gm. Equivalent of a substance is:


  1. 96,500 coulombs
  2. one ampere for one hour
  3. one ampere per sec
  4. charge in faradays

A
96,500 coulombs
B
charge in faradays
C
one ampere per sec
D
one ampere for one hour
Solution
Verified by Toppr

According to Faraday's laws, for deposition of 1 gm of an equivalent weight of a substance, amount of charge required is equal to the charge on one mole of electrons.
i.e., the Electric charge required = Electric charge on one mole of electrons
= Charge on one electron x Avagadro's number
= 1.6×1019×6.023×1023
= 96500 C/mol

Was this answer helpful?
0
Similar Questions
Q1

The electric charge for electrode deposition of 1gm. Equivalent of a substance is:


View Solution
Q2
The electric charge for electrode deposition of one gram equivalent of a substance is:
View Solution
Q3
(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.
View Solution
Q4
The electrochemical equivalent can be defined as the mass of the substance in grams produced/consumed at the electrode by one coulomb of charge or by one ampere of current passed for one second.

View Solution
Q5
Match the column I with column II and mark the appropriate choice.
Column I
Column II
(A)Electrochemical equivalent(i)Potential difference x Quantity of charge
(B)Faraday(ii)Mass of substance deposited by one coulomb of charge
(C)Ampere(iii)Charge carried by one mole of electrons
(D)Electrical energy(iv)One coulomb of electric charge passed through one second

View Solution