An aqueous solution contains 545 g of ThCl3. If the solution is electrolyzed usi

Question

An aqueous solution contains 545 g of ThCl3. If the solution is electrolyzed using inert electrodes, calculate the current needed to remove all of the thorium from the solution in 5.00 hours.

Explanation / Answer

molecular mass of ThCl3 = 338.5 g/mole so no.of moles of ThCl3 = 545/338.5 = 1.61 now 1 mole of ThCl3 contains 1 mole of Th(3+) ions so 1.61 moles of ThCl3 will contain 1.61 moles of Th(3+) ions and the questions says to determine the current needed to remove all these 1.61 moles of Th3+ ions and convert it to Th (solid) i.e. the following reaction : Th(3+) + 3e- ------> Th(s) according to this reaction for depositing 1 mole of Th we recquire 3F of electricity so for 1.61 mole of Th we will recquire 1.61 X 3 = 4.83 F of electricity so Q = 4.83F = 4.83 X 96500 = 466095 C t = 5 hours = 5 x 60 X 60 = 180000 s and as Q = I X t so I = Q/t = 466095/180000 = 2.589 ampere feel free to ask any question

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