Electrolusis involves electronation and de-electronation at the redpective electrodes. Anode of electrolytic cell is the electrode at which de-electronation takes place whereas at cathode electronation is noticed. If two or more ions of same charge are to be electronated or de-electronated, the ion having lesser discharge potential is dischargeed. Discharge potential of an ion refers for `E_(OP)^(@)` or `E_(RP)^(@)` as the case may be. The products formed at either electrode is given in terms of Faraday's laws of electrolysis i.e., `w = (Eit)/(96500)`
A. During electrolysis of `CH_(3)COONa_((aq.))` the mole ratio of gases formed at cathode and anode is :

Options

A. `1:2`
B. `2:1`
C. `3:1`
D. `1:3`

Explanation

Cell constant = `("Sp. Cond of KCl")/("Conductance of KCl") rarr` = `(2.768xx10^3)/(1//250.2)`
`=2.768 xx10^(-3)xx250.2`
For 0.01 M `CuSO_4` solution
Sp. Conductivity = cell constant `xx` Conductance
`2.768xx10^(-3)xx250.2xx1/(8331)`
Molar conductance = Sp. cond. `xx (1000)/C`
= `(2.768xx10^(-3)xx250.2)/(8331xx1000/(1)//(100))` = 8.312 `ohm^-1cm^2mol^-1`