Final answer:
The mass of nitrogen monoxide (NO) formed when ammonia reacts with oxygen can be calculated using mass-mass stoichiometry. The problem requires determining the limiting reactant and using the balanced chemical reaction to find the theoretical yield of NO.
Step-by-step explanation:
The student asked about the mass of nitrogen monoxide (NO) that would form when 4500 kg of ammonia (NH3) reacts with 7500 kg of oxygen (O2). This question relates to the field of stoichiometry, specifically mass-mass stoichiometry. This area of study involves calculating the masses of reactants and products in chemical reactions. The balanced chemical equation for the reaction provided is 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l). Using this equation, we can determine the theoretical yield of NO based on the limiting reactant, which is the reactant that will be completely consumed first in the reaction.
To solve this problem, we start by converting the masses of NH3 and O2 into moles, using their respective molar masses. We then compare the mole ratio of the reactants with the stoichiometry of the balanced equation to find the limiting reactant. Once we determine the limiting reactant, we use its mole quantity to calculate the moles of NO that can be formed. Finally, we convert these moles of NO back into mass, giving us the mass of nitrogen monoxide produced.