How many minutes will it take to plate out 2.19 g of chromium metal from a solution of Cr³⁺using a current of 35.2 amps in an electrolyte cell ?

Question

Quizplus · Accepted Answer

First, we need to calculate the amount of charge required to plate out 2.19 g of chromium. Using the molar mass of chromium (52 g/mol), the number of moles of chromium present in 2.19 g is:

n = m/M = 2.19 g / 52 g/mol = 0.0421 mol

Now, we can use Faraday's law of electrolysis to calculate the amount of charge required:

Q = nF = 0.0421 mol x 96485 C/mol = 4068 C

Finally, we can use the formula for current (I = Q/t) to calculate the time required to deliver this amount of charge at a current of 35.2 amps:

t = Q/I = 4068 C / 35.2 A = 115.3 seconds = 5.77 minutes

How Many Minutes Will It Take to Plate Out 2