A current of 1.25 amperes was passed for sixty minutes through a solution of a metal Chloride (At. mass of metal = 119) and 2.8 gms of metal was deposited. Correct statements are

(1) $\text{ Coulombs passed }=1.25\times 60\times 60=4500$

$\text{ Weight of metal deposited per Faraday }=\frac{2.8\times 96,500}{4500}=\mathbf{60}\text{ gms }$

$\therefore$Equivalent weight of metal = 60

$\text{ Oxidation state of metal }=\frac{119}{60}\approx 2$

$\text{ Moles of }\overline{e}\text{ used }=\frac{4500}{96,500}=0.047$

(4) $\text{ E.C.E. of metal }=\frac{60}{96,500}=6.22\times {10}^{-4}\text{ gms per coulomb. }$