Question

38. -10.1 points 0/4 Submissions Used Metallic iron can be made by the electrolysis of molten f os (a) What mass of fe is formed by passing a current of 605 A through molte s for 3.0 days? The unbalanced chemical reaction representing this electrolysis is shown below. Fe Oy --Fe+ of fe is formed by this electrolysis D) How many minutes are needed to plate out 6.00 of fe from molten fe, using current? minutes are needed

Answer 1

1. equation of electrolysis : Fe³⁺ + 3e $\rightarrow$ Fe

Coulombs of charge = no. of electrons * 1 F = 3 * 96500 = 2.90 * 10⁵ C

Charge produced by current = current * time in s = 6.05 * 3.4 * 24 * 60 * 60 = 1.78 * 10⁶ C

Moles of Fe produced = Charge produced / Charge per mole of Fe = 1.78 * 10⁶ / (2.90 * 10⁵ ) = 6.138 moles

Mass of Fe = moles * molar mass = 6.138 * 55.8 = 342.50 g

2. Moles of Fe = mass / molar mass = 8 / 55.8 =0.143 moles

Charge needed = moles * 2.90 * 10⁵ = 0.143 * 2.90 * 10⁵ = 4.15 * 10^{4 _C}

Time taken = Charge / current = 4.15 * 10⁴ / 8.79 = 4.72 * 10³ s = 4720 / 60 min = 78.67 min