Final answer:
The question contains a possible typo regarding reaction products. Using typical stoichiometry techniques, one can determine the mass of the water produced from given masses of reactants by using molecular weights and mole ratios from a balanced chemical equation, but the original question does not provide enough information to solve directly.
Step-by-step explanation:
The question is asking how many grams of water are produced from a given amount of carbon dioxide (CO2) and ammonia (NH3). This reaction is not fully described, but assuming it follows the typical combustion of a hydrocarbon or related reaction, it would produce water and another compound (commonly carbon dioxide or nitrogen oxides when dealing with hydrocarbons and nitrogen-containing substances, respectively). To accurately determine the mass of water produced, we would need a balanced chemical equation which includes the amounts of CO2 and NH3.
However, considering this is an apparent hypothetical situation or typo in the question, we can refer to similar stoichiometry problems based on the creation of NH3 from N2 and H2 to demonstrate how the law of conservation of mass applies. In such problems, one may calculate the mass of products formed from the mass of reactants using molecular weights and mole ratios as determined by the balanced chemical equation.
For example, the balanced equation N2 + 3H2 → 2NH3 allows us to determine that 2 moles of NH3 are produced for every 1 mole of N2 reacted. Using molecular weights (17.03 g/mol for NH3, 28.02 g/mol for N2), someone can calculate the mass of NH3 produced from a given mass of N2 and vice versa.