# GIven, 2NH_3(g)+2CH_4(g)+3O_2(g)rarr2HCN(g)+6H_2O(g)... ...what mass of hydrocyanic acid would result from a 203.6*g mass of ammonia?

May 1, 2017

I gets..........over $300 \cdot g$ of $H C \equiv N$ given QUANTITATIVE reaction.

#### Explanation:

You have given the stoichiometric equation:

$2 N {H}_{3} \left(g\right) + 2 C {H}_{4} + 3 {O}_{2} \left(g\right) \rightarrow 2 H C N \left(g\right) + 6 {H}_{2} O \left(g\right)$

$\text{Moles of ammonia} = \frac{203.6 \cdot g}{17.03 \cdot g \cdot m o {l}^{-} 1} = 11.9 \cdot m o l$.

And now attend! The stoichiometry CLEARLY indicates that a given molar quantity of ammonia will give an EQUIMOLAR quantity of hydrogen cyanide. And given quantitative reaction, we should, with respect to hydrogen cyanide, get a mass of............

11.9*molxx27.03*g*mol^-1=??g

I think this is the old $\text{Andrussow Process}$ which is performed to this day.