Question

Neglect overpotential and determine the minimum potential required to electrolyze molten CuCl2. Correct: Your answer is correct. How grams of Cu would be deposited and how many liters of Cl2 gas would be produced at 76 oC and 2.33 atm by passing a current of 22.0 A for 12.0 hrs? g Cu L Cl2

Answer 1

1)

Electrolysis equation is:

Cu2+ + 2e- ------> Cu

1 mol of Cu requires 2 mol of electron

1 mol of electron = 96485 C

So,1 mol of Cu requires 192970 C

let us calculate the charge passed:

t = 12.0 hr = 12.0*3600 s = 4.32*10^4 s

time, t = 4.32*10^4s

Q = I*t

= 22A * 4.32*10^4s

= 9.504*10^5 C

mol of Cu plated = 9.504*10^5/192970 = 4.925 mol

Molar mass of Cu = 63.55 g/mol

mass of Cu = number of mol * molar mass

= 4.925 * 63.55

= 313 g

Answer: mass of Cu = 313 g

2)

CuCl2 —> Cu + Cl2

mol of Cl2 produced = mol of Cu = 4.925 mol

Given:

P = 2.33 atm

n = 4.925 mol

T = 76.0 oC

= (76.0+273) K

= 349 K

use:

P * V = n*R*T

2.33 atm * V = 4.925 mol* 0.08206 atm.L/mol.K * 349 K

V = 60.5 L

Answer: 60.5 L