Question

A current of 6.15×10⁴ A is passed through an electrolysis cell containing molten MgCl₂ for 6.50 days.

(a) How many grams of magnesium are produced?

_____g

(b) How many liters of chlorine are collected, if the gas is at a temperature of 273 K and a pressure of 1.00 atm?

_____L

Answer 1

MgCl2 ------------------> Mg^2+ (aq) + 2Cl^-(aq0

Mg^2+ (aq) + 2e^- ---------------------> Mg(s)

             z   = 2

W    = MCt/ZF

F     = 96500c

t        = 6.5days   = 6.5*24*60*60   = 561600sec

M     = 24g/mole

   c= 6.15*10^4   = 61500c

W    = 24*61500*561600/2*96500   = 4.3*10^6 g

b.   2Cl^- -------------> Cl2 + 2e^-

W    = MCt/ZF

    W/M   = Ct/ZF

n   = Ct/ZF

        = 61500*561600/2*96500   = 178955moles

PV = nRT

V = nRT/P

     = 178955*0.0821*273/1   = 4010972L >>>answer

      n   =