0.2 moles of electrons are possed through three electrolytic cells in series that contain silver ions zinc and iron (III) ions.How many grams of each metal will be deposited at cathode?
To find out how many grams of each metal will be deposited, we need to calculate the amount of each metal using Faraday's law of electrolysis.
First, we convert moles of electrons to coulombs using Faraday's constant:
1 mole of electrons = 96,485.3 coulombs
Therefore, 0.2 moles of electrons = 0.2 * 96,485.3 = 19,297.06 coulombs
Next, we calculate the amount of silver deposited:
1 mole of silver = 1 mole of electrons (from the balanced equation)
Therefore, the amount of silver deposited = 0.2 moles
To find the mass of silver deposited, we need to multiply the moles by its molar mass:
Molar mass of silver = 107.87 g/mol
Mass of silver deposited = 0.2 moles * 107.87 g/mol = 21.574 g
Next, we calculate the amount of zinc deposited:
1 mole of zinc = 2 moles of electrons (from the balanced equation)
Therefore, the amount of zinc deposited = 0.2 moles * 2 = 0.4 moles
To find the mass of zinc deposited, we need to multiply the moles by its molar mass:
Molar mass of zinc = 65.38 g/mol
Mass of zinc deposited = 0.4 moles * 65.38 g/mol = 26.152 g
Finally, we calculate the amount of iron deposited:
1 mole of iron (III) ions = 3 moles of electrons (from the balanced equation)
Therefore, the amount of iron deposited = 0.2 moles * 3 = 0.6 moles
To find the mass of iron deposited, we need to multiply the moles by its molar mass:
Molar mass of iron = 55.85 g/mol
Mass of iron deposited = 0.6 moles * 55.85 g/mol = 33.51 g
Therefore, at the cathode, 21.574 grams of silver, 26.152 grams of zinc, and 33.51 grams of iron will be deposited.