An aqueous solution of `NaCl` on electrolysis gives `H_(2)(g), Cl_(2)(g),` and `NaOH` accroding to the reaction `:`
`2Cl^(c-)(aq)+2H_(2)Orarr2overset(c-)(O)H(aq)+H_(2)(g)+Cl_(2)(g)`
A direct current of `25A` with a current efficiency of `62%` is passed through `20L` of `NaCl` solution `(20%` by weight`)`. Write down the reactions taking place at the anode and cathode. How long will it take to produce `1 kg ` of `Cl_(2)`? `(` Assume no loss due to evaporation . `)`

Explanation

At anode `2C1^(-) to C1_2+2e^(-)`
At cathode
`2H_2O+2e^(-) toH_2+2oH^(-)`
` 1kg Cl_2=100/35.5 ` equivalent of `Cl_2=28.17` equivalent `implies` Therefore electricity requiremnt `=28.17 F`
Q Efficency is only 62%
`therefore` Electricity requirement (experimental)`=(28.17xx10)/(62)=F=45.44f`
`implies 45.44 xx96500=25t` (in second) `implies t=48.72 h`
Also, gram equivalent of `HO^(-)` produced `=28.17`
`implies` Molarity of `HO^(-)=28.17/20=1.4085 M`