Question

The annual production of Cl2 is about 45 millions tons per year. Assume that a typical plant is operational 90 % of the year. The operating voltage of a cell is 3.4 V (considerably higher than the equilibrium voltage)
(a) Write down the half-cell reaction for the oxidation chloride to form chlorine.
(b) Determine the total current worldwide needed to gener- ate the global supply of Cl2.
(c) Calculate the electrical power needed to produce the global supply of chlorine using electrolysis.

Answer 1

Answer:

a) CI^-  ⇒ CI2 + 2e^-

b) 4.2 * 10^9  amperes

c) 1.4 * 10^10 watts

Explanation:

Given data:

Annual production of C12 = 45 millions tons per year

Typical plant operational percentage = 90%

Operating voltage of a cell = 3.4 v

A) Half-cell reaction for oxidation chloride to form chlorine

     CI^-  ⇒ CI2 + 2e^-

B) Calculate the total current worldwide needed to generate the global supply of CI 2

Total current = $\frac{Q}{t}$ = $\frac{1.2*10^{17} }{2.84*10^7}$ = 4.2 * 10^9  amperes

Q = charge , t = time

C ) Calculate electrical power need to produce global supply of chlorine using electrolysis

P = V*I

  = 3.4 * 4.2 * 10^9

  = 1.4 * 10^10 watts