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An electrolysis cell that deposits gold (from Au+(aq)) operates for 10.0 minutes at a current of...

An electrolysis cell that deposits gold (from Au+(aq)) operates for 10.0 minutes at a current of 2.50 A. What mass of gold is deposited?

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Answer #1

Electrode equation: (-) cathode Au3+(aq) + 3e- ==> Au(s) and Ar(Au) = 197

the quantity of electricity passed in Coulombs= current in A x time in secs (Q = I x t)

= 2.5 x 10 x 60 = 1500 Coulombs,

and 1 mole electrons = 96500 Coulombs

therefore moles of electrons passed through circuit = 1500 / 96500 = 0.01554

it takes three moles of electrons to form one mole of gold

therefore moles gold = 0.01554 / 3=0.00518

mass of gold = moles of gold x atomic mass of gold

= 0.00518 x 197 = 1.02g of gold deposited.

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