Question
Elemental calcium is produced by the electrolysis of molen CaCl2.
What mass of calcium can be produced by this process if a current of 8500 A is applied for 39 h? Assume that the electrolytic cell is 65% efficient. I found the mass to equal 1.6 x10^5g Ca, and that is correct.
It’s part B that I’m struggling with. What is the total energy requirement for this electrolysis if the applied emf is + 5.20 V?
I keep getting 1100 kWh, but it’s saying that it’s incorrect.
I did (1.6 x 10^5g)(1 mol Ca/40.078 g Ca)(2 mol e-/1 mol Ca)(96,485 C/1 mol e-)
(770, 377, 763.4 V)(5.20 V)(1 J/1C-V)(1 kWh)(3.6 x 10^6 J)=1100 kWh
What am I doing wrong?
What mass of calcium can be produced by this process if a current of 8500 A is applied for 39 h? Assume that the electrolytic cell is 65% efficient. I found the mass to equal 1.6 x10^5g Ca, and that is correct.
It’s part B that I’m struggling with. What is the total energy requirement for this electrolysis if the applied emf is + 5.20 V?
I keep getting 1100 kWh, but it’s saying that it’s incorrect.
I did (1.6 x 10^5g)(1 mol Ca/40.078 g Ca)(2 mol e-/1 mol Ca)(96,485 C/1 mol e-)
(770, 377, 763.4 V)(5.20 V)(1 J/1C-V)(1 kWh)(3.6 x 10^6 J)=1100 kWh
What am I doing wrong?
Answers
This was for online homework that was due tonight, and the answer is .43 kWh, but I'd still like to know how to get this answer. Thank you!!