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)`

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) .

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) .

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.

How much electricity in terms of Faraday is required to produce? (a) 20 g of Ca from molten CaCl_2 (b) 40 g of Al from molten Al_2O_3 Given: Molar mass of Ca = 40 g mol^(-1) Molar mass of Al-27 g mol^(-1)

How many Faradays of electricity are required to deposit 10 g of calcium from molten calcium chloride using inert electrodes ? (molar mass of calcium = 40 g mol^(-1) )