Final answer:
When ammonium carbonate decomposes, it produces ammonia and carbon dioxide in a 2:1 molar ratio, with the concentration of ammonia being twice that of carbon dioxide. Stoichiometry is crucial in understanding the relationship between reactants and products in decomposition reactions, which is applicable to various chemical processes.
Step-by-step explanation:
When ammonium carbonate decomposes, it forms ammonia and carbon dioxide gases. According to stoichiometry, the decomposition of ammonium carbamate produces a 2:1 molar ratio of ammonia to carbon dioxide. Thus, at equilibrium, the concentration of ammonia will be twice that of carbon dioxide. This same principle of stoichiometry applies in other decomposition reactions, such as when ammonium nitrate decomposes into dinitrogen monoxide and water, or when calcium carbonate decomposes to produce lime (CaO) and carbon dioxide.
Consider, for example, the decomposition reaction of ammonium nitrate (NH4NO3), which yields dinitrogen monoxide (N2O) and water (H2O). The stoichiometry of this reaction indicates the ratio of products formed from a given mass of reactant. By understanding the stoichiometric relationships in these reactions, one can perform calculations related to equilibrium constants, volumes of gases produced, and masses of reactants and products.