Hydrogen cyanide, HCN, is prepared from ammonia, air and natural gas (CH4) by the following process.

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Hydrogen cyanide, HCN, is prepared from ammonia, air and natural gas (CH4) by the following process. 2NH3(g) + 3O2(g) + 2CH4(g)$\overset{\quad pt\quad}{\rightarrow}$2HCN(g) + 6H2O(g) If a reaction vessel contains 11.5 g NH3, 10.0 g O2, and 10.5 g CH4, then what is the maximum mass, in grams, of hydrogen cyanide that could be made, assuming the reaction goes to completion?

Accepted Answer

$2NH_{3}(g) + 3O_{2}(g) + 2CH_{4}(g)\overset{\quad Pt\quad}{\rightarrow}2HCN(g) + 6H_{2}O(g)$

$\frac{n_{NH_{3}}}{2} = \frac{11.5/17}{2} = 0.338;\frac{n_{O_{2}}}{3} = \frac{10/32}{3} = 0.104;\frac{n_{CH_{4}}}{2} = \frac{10.5/16}{2} = 0.328$

Hence, O₂ is limiting reagent. Mass of HCN formed = $\frac{2}{3} \times \frac{10}{32} \times 27$= 5.625 g

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