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

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Jakobe Henry

Chemistry

14 December, 12:14

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

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Leonard Mckenzie · Answer 1

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)