Answer: -
224 g of Ca metal are produced by the electrolysis of molten CaBr₂ using a current of 30.0 amp for 10.0 hours.
Explanation: -
Total time t = 10.0 hours = 10.0 x 60 x 60 s
Charge supplied = Q = i x t
= 30.0 A x 10.0 x 60 x 60 s
= 1080000 C
Number of moles of electrons = Charge supplied / Faraday constant
= 1080000 C / 96500 C
= 11.2 mol
We know the ionic equation for Ca deposition is
Ca²⁺ 2 e⁻ → Ca
We see that
2 mol of electron give 1 mol of Ca²⁺
11.2 mol of electron gives [tex] \frac{1 mol Ca2+}{2 mol electron} [/tex] x 11.2 mol electron
= 5.6 mol of Ca
Molar mass of Ca = 40 g/ mol
Mass deposited = Number of moles of Ca x molar mass
= 5.6 mol x 40 g/ mol
=224 g of Ca
