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A solution of a salt of metal was electr...

A solution of a salt of metal was electrolysed for 150 minutes with a current of 0.15 amperes. The mass of the metal deposited at the cathode is 0.783g. Calculate the equivalent mass of the metal.

Text Solution

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Given, `I=0.15` amperes
`t=150" mins" rArr t=150xx60 sec rArr t=9000 sec`
`Q=It rArr Q=0.15xx9000" coulombs" rArr Q=1350` coulombs
Hence, 135 coulombs of electricity deposit is equal to 0.783g of metal.
`therefore` 96500 coulombs of electricity, `(0.783xx96500)/(1350)=55.97g` of metal
Hence equivalent mass of the metal is 55.97
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