Cell \\\\(B\\\\): \\\\(\\displaystyle Ag^+ + e^- \\rightleftharpoons Ag\\\\) at cathode.\\\\(1\\\\) mole (\\\\(108\\\\) g) of Ag is deposited by \\\\(96500\\\\) \\\\(C\\\\).\\\\(1.45\\\\) g of Ag will be deposited by \\\\(\\displaystyle \\dfrac {96500 \ imes 1.45}{108} = 1295.6 \\: C\\\\).Now,\\\\(\\displaystyle Q = It \\\\)\\\\(\\displaystyle 1295.6 = 1.5 \ imes t \\\\)\\\\(\\displaystyle t = 864 \\: s\\\\)Cell \\\\(A\\\\): \\\\(\\displaystyle Zn^{2+} + 2e^- \\rightarrow Zn\\\\)\\\\(2\\\\) moles of electrons (\\\\(\\displaystyle 2 \ imes 96500\\\\) C of current) produces \\\\(1\\\\) mole (\\\\(63.5\\\\) g) of zinc.\\\\(1295.6\\\\) \\\\(C\\\\) of electricity will deposit \\\\(\\displaystyle \\dfrac {65.3}{2 \ imes 96500} \ imes 1295.6 = 0.438\\\\) g of zincCell \\\\(C\\\\): \\\\(\\displaystyle Cu^{2+} + 2e^- \\rightarrow Cu\\\\)\\\\(2\\\\) moles of electrons (\\\\(\\displaystyle 2 \ imes 96500\\\\) \\\\(C\\\\)) of current will produce \\\\(1\\\\) mole (\\\\(63.5\\\\) g) of \\\\(Cu\\\\). \\\\(1295.6\\\\) \\\\(C\\\\) of current will deposit \\\\(\\displaystyle \\dfrac {63.5 \ imes 1295.6}{2 \ imes 96500} = 0.426 \\: g\\\\) of copper