Question

a current of 3.54 a is passed through a fe(no), solution for 1.60 h. how much iron is plated out of the solution?

Answer 1

To calculate the amount of iron plated out of the solution, we can use Faraday's law of electrolysis. By calculating the number of moles of electrons and multiplying it by the molar mass of iron, we find that approximately 1.64 x 10^-3 g of iron is plated.

Step-by-step explanation:

To determine the amount of iron that is plated out of the solution, we need to calculate the number of moles of electrons that passed through the cell. From the given information, we know that the current is 3.54 A and the time is 1.60 h. We can use Faraday's law of electrolysis to calculate the moles of electrons:

1. Calculate the total charge in coulombs using the formula Q = I * t, where Q is the charge, I is the current, and t is the time. Q = 3.54 A * 1.60 h.
2. Find the number of moles of electrons using the equation moles = Q / (n * F), where n is the number of electrons transferred and F is the Faraday constant (96485 C/mol). In this case, n is the number of moles of electrons required to plate one mole of iron, which is 2.
3. Multiply the number of moles of electrons by the molar mass of iron (55.85 g/mol) to find the mass of iron plated out of the solution.

Calculation:

Q = 3.54 A * 1.60 h = 5.67 C

moles = 5.67 C / (2 * 96485 C/mol) = 2.94 x 10^-5 mol

mass = 2.94 x 10^-5 mol * 55.85 g/mol = 1.64 x 10^-3 g
Therefore, approximately

1.64 x 10^-3 g of iron is plated out of the solution.