# Question 1d1c4

Jun 11, 2017

It is seen from the given balanced equation of the repacement reaction that every mole of ${\left(C {H}_{2}\right)}_{n}$ requires total $2 n m o l$ ${F}_{2}$.Here $n$ mol goes to replace hydrogen and $n$ mol goes to form $2 n$ mol $H F$ and thus one mole of ${\left(C {F}_{2}\right)}_{n}$ is formed.

Molar masses of

${F}_{2} \to 38 g \text{/} m o l$

${\left(C {F}_{2}\right)}_{n} \to 50 n g \text{/} m o l$

Fluorine required for the production of $50 n g$ ${\left(C {F}_{2}\right)}_{n}$ is 2n mol or $76 n g$

So to prodoce 1kg ${\left(C {F}_{2}\right)}_{n}$ we rrequire $\frac{76 n}{50 n} k g = 1.52 k g$ Fluorine, if not recovered from $H F$ produced as byproduct.

As 50% ${F}_{2}$ goes to form the byproduct $H F$,then its recovery will diminsh the net consumption by 50% and the consumption of Flurine for productio of 1kg ${\left(C {F}_{2}\right)}_{n}$ then will be 50%of1.52kg=0.76kg#