An electroplating apparatus is used to reduce metal ions from aqueous solutions onto cathodes in two separate electrolytic cells. In Cell 1, a constant current of \(2.0\text{ A}\) is passed through an aqueous solution of \(\text{AgNO}_3\) for \(15\text{ min}\), depositing \(x\text{ mol}\) of \(\text{Ag}(s)\). In Cell 2, a constant current of \(3.0\text{ A}\) is passed through an aqueous solution of \(\text{Cr(NO}_3)_3\) for \(30\text{ min}\). Assuming that the cathode current efficiency is \(100\%\) in both cells, what is the amount of \(\text{Cr}(s)\) deposited in Cell 2 in terms of \(x\)?