A) calculate the mass of li formed by electrolysis of molten licl by a current of 8.2 104 a flowing for a period of 14 hr. assume the electrolytic cell is 70. percent efficient. (b) what is the energy requirement for this electrolysis per mole of li formed if the applied emf is +8.4 v? answer in kwh/mol

a)

= 210,000 gram or 210 Kg  

Explanation:

14 hr is equivalent to;

= 14 × 3600 s

But; 

8.2x10^4 A = 8.2x10^4 Coulomb /second = 8.2x10^4 C/s  

1 Faraday = 96485C  

Molar mass of Li: 6.941 g/mol  

Therefore;

{(8.2x10^4 C/s)×(14×3600s)×(6.941 g/mol)/(96485C/mol)}×70%  

= 2.1x10^5 gram  or 210 kg

b.  Answer;

= 0.23 kWh/mol

Explanation and solution;

Energy per mole is given by;

(96485C/mol) × (8.4V) = 8.10x10^5 (J/mol)  

= 8.10x10^5 (Ws/mol)  

Divide by 3600s/h to get:  

= 8.10x10^5 (Ws/mol)

= 225 Wh/mol

= 0.23 kWh/mol

the electron configuration that you gave me has 16 electrons ergo it has 16 protons ergo it is the element sulfur.