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Novay_Z [31]
3 years ago
14

Hydrogen cyanide is prepared commercially by the reaction of methane, ch4(g), ammonia, nh3(g), and oxygen, o2(g), at high temper

ature. the other product is gaseous water. (a) write a chemical equation for the reaction. (use the lowest possible coefficients. include states-of-matter under the given reaction conditions in your answer.)
Chemistry
1 answer:
Flauer [41]3 years ago
6 0
Following the description for the synthesis of Hydrogen Cyanide, the molecular reaction is

CH₄(g) + NH₃(g + O₂(g) →  HCN(g) + H₂O(g)

According to Dalton's Atomic Theory, in on of his postulates, compounds are characterized as having a fixed ratio of number of individual elements. During a chemical reaction, the compounds exchange elements while obeying the fixed ratio. This law is defined as the Law of Definite Proportions. Thus, it is essential to balance a chemical reaction. Make sure that the element has the same number of atoms, represented by the stoichiometric coefficients, on both sides of the reaction. It is actually a trial-and-error process. For this reaction, the balanced chemical reaction is

2 CH₄(g) + 2 NH₃(g + 3 O₂(g) →  2 HCN(g) + 6 H₂O(g)
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