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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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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)

The balanced equation for the preparation of hydrogen cyanide is given as 2 moles of methane reacts with 2 moles of ammonia and 3 moles of oxygen to give 2 moles of hydrogen cyanide and 2 moles of water.

What is a chemical equation?

A chemical reaction is the formulation of the compounds with the reaction of reactants.

The chemical equation is written by following the law of conservation, as mass can neither be created nor be destroyed in a chemical reaction.

Thus, the coefficient in the balanced chemical equation represents the moles of each element in the product and the reactant side.

The chemical equation for the production of hydrogen cyanide has been given as:

2 moles of ammonia and 3 moles of oxygen to give 2 moles of hydrogen cyanide and 2 moles of water.

Learn more about the chemical equations, here:

https://brainly.com/question/20492533

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