Question

Which of the following options represents the correct time required for a constant current of 1.00 A to deposit the specified amounts of thallium (Tl)?

(a) 14.0 hours for depositing 0.450 g of Tl(III) as the element on a cathode.
(b) 18.9 hours for depositing Tl(I) as Tl2O3 on an anode.
(c) 20.8 hours for depositing Tl(I) as the element on a cathode.
(d) None of the above

Answer 1

To solve this problem, we need to use Faraday's law of electrolysis to calculate the time required for each scenario. Comparing the calculated times with the given options, we find that none of the options match the calculated times.

Step-by-step explanation:

To solve this problem, we need to use Faraday's law of electrolysis, which states that the amount of substance deposited at an electrode is directly proportional to the quantity of electricity passed through the electrolyte.

(a) To deposit 0.450 g of Tl(III) as the element on a cathode, we need to calculate the time using the equation:
Time = (mass / molar mass) / (charge / Faraday's constant)

(b) To deposit Tl(I) as Tl2O3 on an anode, we need to calculate the time using the equation:
Time = (mass / molar mass) / (charge / Faraday's constant)

(c) To deposit Tl(I) as the element on a cathode, we need to calculate the time using the equation:
Time = (mass / molar mass) / (charge / Faraday's constant)

Comparing the given times with the calculated times, we can determine that option (d) None of the above is the correct answer as none of the options match the calculated times.