If a student wants to plate 6.55g of nickel using a nickel sulfate solution, but has only 14 minutes to do so. What current is required to achieve this?
To calculate the required current, we need to know the Faraday's constant. The Faraday's constant (F) represents the charge of one mole of electrons, which is equal to 96,485 Coulombs.
First, we need to determine the number of moles of nickel that need to be plated. We can use the molar mass of nickel (Ni) to do this calculation. The molar mass of Ni is 58.69 g/mol.
moles of Ni = mass of Ni / molar mass of Ni
moles of Ni = 6.55 g / 58.69 g/mol
moles of Ni = 0.1116 moles
Next, we need to determine the charge required to plate this amount of nickel. Since each mole of nickel requires two moles of electrons, we multiply the number of moles by 2.
charge required = 0.1116 moles * 2 * F
charge required = 0.2232 * 96,485 Coulombs
charge required = 21,639 Coulombs
Finally, we can calculate the current required using the formula:
current = charge / time
current = 21,639 Coulombs / 14 minutes
current = 21,639 Coulombs / 840 seconds
current ≈ 25.7 Amperes
Therefore, a current of approximately 25.7 Amperes is required to plate 6.55g of nickel using a nickel sulfate solution in 14 minutes.