Final answer:
To find the mass of nitrogen monoxide formed, we need to determine the limiting reactant and use stoichiometry to calculate the mass. The mass of nitrogen monoxide formed is 4500 kg.
Step-by-step explanation:
To find the mass of nitrogen monoxide (NO) formed, we need to determine the limiting reactant and use stoichiometry to calculate the mass.
We can start by finding the number of moles of ammonia (NH₃) and oxygen (O₂) using their molar masses. Then, we compare the moles of each reactant to determine the limiting reactant (the reactant that is completely consumed).
Once we have the limiting reactant, we can use the balanced equation to determine the moles of nitrogen monoxide (NO) produced. Finally, we convert the moles of NO to grams using its molar mass.
In this case, the balanced equation is:
4NH₃ + 5O₂ → 4NO + 6H₂O
According to the equation, 4 moles of ammonia reacts with 5 moles of oxygen to produce 4 moles of nitrogen monoxide. Therefore, we set up a proportion to find the moles of NO produced:
(4 moles NH₃ / 4 moles NO) = (4500 kg NH₃ / x)
By solving for x, we find that 4500 kg of ammonia would produce 4500 kg of nitrogen monoxide. So, the mass of nitrogen monoxide formed is 4500 kg.