Final answer:
The precise calculation of kilograms of NO2 produced from 75.0 kg of hydrazine requires a balanced chemical equation, which is not provided in the question. The reaction between nitrogen and hydrogen to produce ammonia is represented by N2 + 3H2 → 2NH3 and stoichiometry is used to determine the mass of ammonia produced and the limiting reactant.
Step-by-step explanation:
To determine how many kilograms of NO2 are produced from the reaction of 75.0 kg of the limiting reagent, we need to write a balanced chemical equation for the reaction of hydrazine (N2H4) with oxygen (O2). However, the provided information seems insufficient for an exact calculation because the question does not specify the balanced equation for the hydrazine and oxygen reaction. The text instead includes different chemical reactions involving ammonia, nitric oxide, and nitrogen dioxide, none of which directly provide the stoichiometry for the reaction of hydrazine with oxygen to form nitrogen dioxide (NO2).
Similarly, for the second part of the question, it is necessary to have a balanced chemical equation to determine the amount of ammonia produced from reacting nitrogen and hydrogen. The balanced equation is N2 + 3H2 → 2NH3. Using stoichiometry, we can calculate the mass of ammonia produced and identify the limiting reactant.