How long must a constant current of 50.0 a be passed through an electrolytic cell containing aqueous cu2 + ions to produce 5.00 moles of copper metal? how long must a constant current of 50.0 a be passed through an electrolytic cell containing aqueous cu2 + ions to produce 5.00 moles of copper metal? 5.36 hours 2.68 hours 0.373 hours 0.187 hours?

When the reaction equation is:

Cu 2 + (aq) + 2 e - → Cu (S)

from the reaction equation, we can see that each 1 mole of Cu 2 + need 2 moles e-

So, the moles of e - when we have 5 moles copper = 5 * 2 = 10 moles

by using this formula we can get the time directly:

time (per sec) = moles of e - * faraday's constant * current

= 10 moles * 96500 coul/mol * 1 sec / 50 coul

= 19300 sec

= 19300 / (60*60) = 5.36 Hours

∴ the answer will be a) 5.36 Hours