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 answer is minerals.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.