What mass of aluminum can be plated onto an object in 755 minutes at 5.80 a of current? what mass of aluminum can be plated onto an object in 755 minutes at 5.80 a of current? 73.5 g 24.5 g 147 g 220. g 8.17 g?

When current * time = mole/molar mass * faraday's constant

when the current = 5.8 a

and time = 755 min

mole 3 (Al+3) = 3 moles

molar mass = 27 g/mol

and Faraday's constant = 96500

by substitution:

∴ mass (g) = 5.8 * 45300 / (3/27 * 96500)

= 24.5 g