Final answer:
To determine the maximum mass of ammonia that can be formed when 85 g of NH4Cl reacts with 130 g of Ca(OH)2, stoichiometry is used to identify the limiting reactant and calculate the moles of ammonia produced, which is then converted to grams.
Step-by-step explanation:
If 85 g of NH4Cl reacts with 130 g of Ca(OH)2, we need the balanced chemical reaction to find out the maximum mass of ammonia that can be formed. The balanced chemical reaction for the formation of ammonia in this case usually looks something like this:
2NH4Cl + Ca(OH)2 → 2NH3 + CaCl2 + 2H2O
We would use stoichiometry to determine the limiting reactant, which is the reactant that will be completely consumed first during the reaction and dictates the maximum amount of product that can be produced. In this scenario, however, the chemical equation provided in the question is not given, so I can't complete the calculation.
Generally, once you've identified the limiting reactant, you would use its amount in moles along with the stoichiometry of the reaction to calculate the moles of ammonia produced. Then, you'll convert the moles of ammonia to grams using its molar mass (17.03 g/mol). This gives you the maximum mass of ammonia that could be formed from the reaction.