In a zinc manganese dioxide dry cell, the anode is made up of zinc and cathode of a carbon rod surrounded by a mixture of `MnO_(2)`, carbon `NH_(4)Cl
In a zinc manganese dioxide dry cell, the anode is made up of zinc and cathode of a carbon rod surrounded by a mixture of `MnO_(2)`, carbon `NH_(4)Cl and ZnCl_(2)` in aqueous base.
The cathodic reaction may be represented as:
`2MnO_(2) (s) + Zn^(2+) + 2e^(-) rarr ZnMn_(2) O_(4) (s)`
Let there be 8g `MnO_(2)` in the cathodic compartment. How many days will the dry cell continue to give a current of `4 xx 10^(-3)` ampere ?
1 Answers
When `MnO_(2)` will be used up in cathodic process, the dry cell will stop to produce current.
Cathodic process:
`overset(+4)(2MnO_(2))(s) + Zn^(2+) + 2e^(-) rarr overset(+3)(ZnMn_(2)O_(4))`
Equivlanet mass of `MnO_(2) = ("Molecular mass")/("Change in oxidation state")`
`= (87)/(1) = 87`
From first law of electrolysis, `W = (I tE)/(96500)`
`8 = ( 4 xx 10^(-3) xx t xx 87)/(96500)`
`t = 2218390.8` second
`= (2218390.8)/(3600 xx 24) = 25.675` days