How many grams of ca metal are produced by the electrolysis of molten cabr 2 using a current of 30.0 amp for 10.0 hours?

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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 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

the objects have the same charge is correct.

nathan lee