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Molten ZnBr2 is electrolyzed by passing a current of 15.0 A through an electrolysis cell for...

Molten ZnBr2 is electrolyzed by passing a current of 15.0 A through an electrolysis cell for a certain length of time. In this process, 45.75g Br2 are deposited_________( anode or cathode). How long does this process require? What is the chemical reaction taking place at the other electrode? What mass of the second product is released at the other electrode?

Solutions

Expert Solution

According to Faraday’s law ,W = (ECt) / 96500

Where W = mass of bromine deposited = 45.75 g

           E = Equivalent weight of Br = 79.9

           C = current = 15.0 A

           t = time taken = ?

Plug the values we get t = 96500 W / EC

                                   = 3684 s

The cell treaction is    : ZnBr2 Zn2+     +   2Br-

                                              (at cathode)   ( at anode)

queen_honey_blossom answered 2 years ago
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