Question

An electrolysis cell is used to produce sodium from molten sodium chloride. How many kilograms of sodium are produced each hour if the cell operates with a supplied current of 1000 Amperes? (Faraday’s Constant, F = 96,500 C mol-1)

Answer 1

2 NaCl (s)  $\small \rightarrow$ 2 Na (s) + Cl₂ (g)

Using Faraday law of electrolysis

W = $\small \frac{E\times i \times t}{F}$

W is mass of product formed

E = gram equivalent mass of product formed

i is current in amp

t is time in sec.

given ,

i = 1000 amp

t = 1 hour = 3600 sec

F = 96500 C mol^-1

E of Sodium = 23 g/ eqv

therefore,

W = $\small \frac{23 \times 1000 \times 3600}{96500}$

or, W = 858.03 g

or, W = 858.03 (g) $\small \times$  _{$\small \frac{1( Kg) }{1000 (g) }$}

or, W = 0.858 Kg.

hence 0.858 Kg of sodium is produced per hour.