Question

How many grams of Ca metal are produced by the electrolysis of molten CaBr2 using a current of 10.0 amp for 2.44 hour??​

Answer 1

17.95 g

Step-by-step explanation:

The electrolysis of CaBr₂ → Ca²⁺ + 2Br⁻

Ca₂⁺ + 2e⁻ → Ca

Recall that:

Charge (Q) = current (I) × time (t)

Q = 10.0 × 2.4 × 3600

Q = 86400 C

Number of moles of electron =
`(charge \ Q)/(faraday's \ constant)`

`=(86400)/(96485) \\ \\ =0.8955 \ mol`

No of moles of Ca =
`(1)/(2) * 0.8955`

= 0.44775 moles

Mass of Ca = no of moles × molar mass of Ca

= 0.44775 mol × 40.08 g/mol

= 17.95 g