A `35%` solution of `LiCl` was electrolyzed by using a `2.5 A` current for `0.8 h. ` Assuming the current efficiency of `90%` , find the mass of `LiOH` produced at the end of electrolysis. `(` Atomic mass of `Li=7)`

A `35%` solution of `LiCl` was electrolyzed by using a `2.5 A` current

1.	A `35%` solution of `LiCl` was electrolyzed by using a `2.5 A` current for `0.8 h. ` Assuming the current efficiency of `90%` , find the mass of `LiOH` produced at the end of electrolysis. `(` Atomic mass of `Li=7)`
Answer» Number of Faradays `=(90)/(100)((2.5xx0.8xx3600)/(96500))` `=0.067F` `Ew=Mw` of `LiOH=7+16+1=24g mol^(-1)` `(n` factor `=1)` `W_(LiOH)=EwxxEq` `=24 xx 0.067=1.61g`

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A `35%` solution of `LiCl` was electrolyzed by using a `2.5 A` current for `0.8 h. ` Assuming the current efficiency of `90%` , find the mass of `LiOH` produced at the end of electrolysis. `(` Atomic mass of `Li=7)`

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