Answer:
To calculate the amount of Zn that can be deposited at the cathode in the electrolysis of molten ZnCl2, we need to use Faraday's law of electrolysis, which states that the amount of substance deposited at an electrode is proportional to the amount of charge passed through the cell.
The equation for Faraday's law is:
moles of substance = (electric charge passed / Faraday's constant)
where the Faraday's constant is the charge carried by one mole of electrons and is equal to 96500 C/mol.
Now, we can calculate the amount of Zn that can be deposited using the following steps:
Calculate the electric charge passed in one hour:
Electric charge = current × time
Electric charge = 0.01 A × 3600 s = 36 C
Calculate the number of moles of Zn that can be deposited:
moles of Zn = (electric charge passed / Faraday's constant)
moles of Zn = (36 C / 96500 C/mol) = 0.000373 moles of Zn
Calculate the mass of Zn deposited:
mass of Zn = moles of Zn × molar mass of Zn
The molar mass of Zn is 65.38 g/mol
mass of Zn = 0.000373 moles of Zn × 65.38 g/mol = 0.0244 g
Therefore, the amount of Zn that can be deposited at the cathode by the passage of 0.01 ampere for one hour is approximately 0.0244 grams.