Question

a) Neglect overpotential and determine the minimum potential required to electrolyze molten CrCl3. (answer: 2.3V)

b) How grams of Cr would be deposited and how many liters of Cl₂ gas would be produced at 62 degrees C and 4.93 atm by passing a current of 26.0 A for 11.0 hrs?

Table of Standard Reduction Potentials: http://www.chemeddl.org/services/moodle/media/QBank/GenChem/Tables/EStandardTable.htm

Answer 1

b) How grams of Cr would be deposited and how many liters of Cl₂ gas would be produced at 62 degrees C and 4.93 atm by passing a current of 26.0 A for 11.0 hrs?

: = 26.0 coulomb /s x 11x60x60 s = 1029600 coulombs
1 F = 96500 C
1029600 / 96500 =10.66F

2 Cl- = Cl2 + 2e-

for every 2 faraday one moles of Cl2 is formed

moles Cl2 = 26.0/2 = 13

T =62 +273=335

V = nRT/p = 13 x 0.08206 x 335 K/ 5.00 atm =75.4 L

about the mass of Cr I thing that the ion is Cr3+
moles Cr = 24.0/3 = 8.0
mass Cr = 8.0 x 52 g/mol=416 g