Ammonia, NH3, and oxygen can be reacted together in the presence of a catalyst to form only nitrogen(II) oxide and water. The number of moles of oxygen consumed for each mole of NO that is produced is?
Write the equation. Balance it. Use an arrow. The coefficients will tell you the ratio you want.
To determine the number of moles of oxygen consumed for each mole of nitrogen(II) oxide (NO) that is produced, we need to examine the balanced chemical equation for the reaction between ammonia (NH3), oxygen (O2), and the catalyst:
4 NH3 + 5 O2 → 4 NO + 6 H2O
According to the balanced equation, for every 4 moles of ammonia, 5 moles of oxygen are required to produce 4 moles of nitrogen(II) oxide.
So, the number of moles of oxygen consumed for each mole of NO that is produced is 5.
To arrive at this answer, it is essential to examine the balanced chemical equation, which represents the stoichiometry of the reaction.