Calculate the quantity of electricity that will be required to liberate `710g` of `Cl`, gas by electrolysing a conc. solution of `NaCl`. What is the amount of `NaOH`and volume.of `H_2` at `27^circ C` and 1 atm pressure is obtained during this process?

Explanation

2Cl- ` Cl_2+2 e^-`
`35.5 ~g Cr` is liberated by passing `96500 C(1 ~F)` of electricity. Hence the quintity of electricity required to liberate `710 ~g Cl_2` `=96500 xx 710^circ/35.5=1930000 C=20 E`
Amount of `NaOH` obtained by using IF `=40 ~g`. (1 g equivalent)``
=40 xx 20 ~g . equ_+=800 ~g cdot NaOH
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IF liberates Ig equiv, of `H`, or `I g H_2` `therefore 20 ~F` gives `20 ~g H_2^prime`
Hen We have, `PV=nRT=w/m RT`
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