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.)

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)

Any photo? or something

Mgo2 is the oxidation state of manganese oxide