Question

electrolysis of hot aqueous solution of NaCl gives NaClO4 how many Faraday are required to obtain 1000 gm of NaClO4​

Answer 1

Answer : The charge required will be, 6305117 C

Explanation :

As we know that if 'n' electrons are involved in the reaction, then the charge required for the reaction of 1 mole of substance by (n × Faraday).

1 Faraday = 96500 C

The balanced chemical reaction will be,

$NaCl+4H_2O\rightarrow NaClO_4+4H_2$

The half-balanced reaction will be,

$2H^{+}+2e^-\rightarrow H_2$

First we have to calculate the moles of $NaClO_4$.

$\text{Moles of }NaClO_4=\frac{\text{Mass of }NaClO_4}{\text{Molar mass of }NaClO_4}=\frac{1000g}{122.44g/mole}=8.1673mole$

Now we have to calculate the moles of $H_2$.

From the balanced chemical reaction we conclude that,

As, 1 mole of $NaClO_4$ react to gives 4 moles of $H_2$

So, 8.1673 mole of $NaClO_4$ react to gives 8.1673 × 4 = 32.669 moles of $H_2$

Now we have to calculate the number of Faraday are required.

From the half-balanced chemical reaction, we conclude that

The number of electrons (n) in the reaction are 2.

The quantity of charge required for the reduction of 1 mole of $2H^{+}$ = $2\times F$

The quantity of charge required for the reduction of 32.669 mole of $2H^{+}$ = $32.669\times 2\times F=65.338F=65.338\times 96500C=6305117C$

Therefore, the charge required will be, 6305117 C