How many grams of Ca metal are produced by the electrolysis of molten CaBr₂using a current of
30) 0 amp for 10.0 hours ?

Question

How many grams of Ca metal are produced by the electrolysis of molten CaBr₂using a current of 30)0 amp for 10.0 hours ?

Quizplus · Accepted Answer

The electrolysis of CaBr2 produces Ca metal and Br2 gas. Using Faraday's laws of electrolysis, the amount of substance produced is proportional to the charge passed. The charge (Q) is calculated as current (I) times time (t): Q = I × t = 300 A × 10 hours × 3600 s/hour = 10,800,000 C. The molar mass of Ca is 40.08 g/mol, and it requires 2 moles of electrons (2 Faradays) to produce 1 mole of Ca. Using the Faraday constant (96485 C/mol), the moles of Ca produced is Q / (2 × 96485) = 56.02 mol, and the mass is 56.02 mol × 40.08 g/mol = 2245.6 g, which rounds to 224 g.

How Many Grams of Ca Metal Are Produced by the Electrolysis