In a certain electrolysis experiment 0.561 g of Zn is deposited in one cell containing `ZnSO_4` solution. Calculate the mass of Cu deposited in another cell containing `CuSO_4` solution in series with `ZnSO_4` cell. Molar masses of Zn and Cu are `65.4 g mol^(-1) and 63.5 g mol^(-1)` respectively.

In a certain electrolysis experiment 4.36 g of Zn are deposited in one cell containing ZnS04 solution. Calculate the mass of Al deposited in another cell containing AICI_3 solution connected in series with ZnSO_4 cell. Molarmassesof Zn and Al are 65.4 g mol^(-1) and 27 g mol^(-1) , respectively.

In a certain electrolysis experiment 0.79 g of Ag was deposited in one cell containing aqueous AgNO_3 solution, while 0.231 g of an unknown metal X was deposited in another cell containing aqueous XCI_2 solution in series with AgNO_3 cell. Calculate the molar mass of X. Molar mass of Ag is 107.9 g mol^(-1) .

The passage of 0.95 A for 40 minutes deposited 0.7493 g of Cu from CuSO_4 solution. Calculate the molar mass of Cu.

The passage of 0.95 A for 40 minutes deposited 0.7493 g of Cu from CuSO_4 solution. Calculate the molar mass of Cu.

Two electrolytic cells one containing AlCl_3 solutionand the other ontaining ZnSO_4 solution are connected in series. The same quantity of electricity is passed between the cells, Calculate the amount of Zn deposited in ZnSO_4 cell if 1.2 g of AI are deposited in AlCl_3 cell. The molar masses of Al and Zn are 27 g mol^(-1) and 65.4 g mol^(-1) respectively.

What is the mass of copper metal produced during thepassageof 5A current through CuSO_4 solution for 100 minutes. The molar mass of Cu is 63.5g mol^(-1) .