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  4. A current of 9.65 ampere flowing for 10 minutes deposits 3.0 g of the metal which is monovalent. The atomic mass of the metal is

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Q. A current of $9.65$ ampere flowing for $10$ minutes deposits $3.0\, g$ of the metal which is monovalent. The atomic mass of the metal is

Electrochemistry

Solution:

$Q = It$
$= 9.65 \times 10\times 60 $
$ = 5790\,C$
$\underset{\text{monovalent metal}}{M^+} + \underset{1F , 96500\,C}{e} \rightarrow \underset {1\,mole}{M}$
With $5790 \,C$, amount of metal deposited $= 3\, gm$
With $96500 \,C$, amount of metal deposited
$ = \frac{3}{5790} \times 96500$
$ = 50\,g$(equivalent weight)
Atomic mass $= 50 \times$ valency
$= 50 \times 1 = 50$ amu