A current of 2.0 A passed for 5 hours through a molten metal salt deposits 22.2g of metal $(Atwt.=177).$ The oxidation state of the metal in the metal salt is

$\mathrm{Q}=2\times 5\times 60\times 60=36000C$

Thus, $36000C$ deposit metal $=22.2g$

$\therefore 96500C$ will deposit metal $=\frac{22.2}{36000}\times 96500g=59.5g$

Thus, Eq.wt. of the metal $=59.5$

Valency or ox. state $=At.wt./Eq.wt.=177/59.5=3$