How much time is needed to deposit 1.0 g of chromium metal from an aqueous solution of crcl3 using a current of 1.5 a?

The metal component of the given compound, CrCl3, is chromium. The number of moles per 1 g of chromium is calculated through the equation below,

n = (1 g Cr) (1 mol Cr/51.996 g Cr)

n = 0.0192 mol Cr (3 electrons/1 mol Cr)

n = 0.0577 e-

Determine the number in charge by multiplying with Faraday's constant,

C = (0.0577 mol Cr) ((1 F/1 mol e-) (96485 C / 1F)

C = 5,566.87 C

Then, calculate time by dividing the charge with the current,

t = 5566.87 C/1.5 A

t = 3711.25 minutes

t = 61.84 hours

Answer: 61.84 hours