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)`.

Mass of copper deposited by the passage of 2 A of current for 965 s through a 2 M solution of CuSO_(4) is (At. Mass of Cu= 63.5) __________.

What current strength in amperes will be required to produce 2.4 g of Cu from CuSO_4 solution in 1 hour ? Molar mass of Cu = 63.5 g mol^(-1)(2.03 A)

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.

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.

What current strengthinampere will berequired to produce 2.369 xx 10^(-3) kg of Cu from CuSO_4 solution in one hour? How many moles of electrons are required? Molar mass of Cu is 63.5 g mol^(-1) .

Calculate the amounts of Na and chlorine gas produced during the electrolysis of fused NaCl by the passage of an ampere current for 25 minutes. Molarmasses of Naand chlorine gas are 23 g mol^(-1) and 71 g mol^(-1) respectively.