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

A solution of a salt of metal was electrolysed for 15 minutes with a current of 0.15 amperes. The mass of the metal deposited at the cathode is 0.783 g. Calculate the equivalent mass of the metal.

Text Solution

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`I=0.15` amperes
times `t=15 times 60s=900s`
mass `m=0.783g`
`m=2It`
`z=m/(It)`
`Q=I times t=0.15 times 900 C`
Amount of the metal deposited by 1 C `=0.783/135=0.0058`
Electrochemical equivalent `Z=5.8 times 10^(-3)gc^(-1)`.
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