a) Calculate the number of moles of nitrogen dioxide, NO2, that could be prepared from 79.0 mol of nitrogen oxide and 82.0 mol of oxygen.
2NO(g)+O2(g)⟶ 2NO2(g)
b) Identify the limiting reagent and the excess reagent in the reaction. What would happen to the potential yield of NO2 if the amount of NO were increased?
c) What if the amount of O2 were increased?
for every mole of O2, one needs 2 moles NO, and gets 2 mole of NO2
82 moles of O2 would require 164 mole NO, which is not there.
So NO is the limiting reactant.
79 moles NO>>>>79 moles NO2
Adding more NO>>>>making more NO2
adding more O2, no effect.
Thank you!
a) To calculate the number of moles of nitrogen dioxide, NO2, that could be prepared, we need to determine which reactant is the limiting reagent.
Using the balanced equation:
2NO(g) + O2(g) ⟶ 2NO2(g)
We can calculate the moles of NO2 produced from each reactant:
Moles of NO2 from NO = 2 moles of NO2 / 2 moles of NO = 1 mole of NO2 per mole of NO
Moles of NO2 from O2 = 2 moles of NO2 / 1 mole of O2 = 2 moles of NO2 per mole of O2
From the given information:
Moles of NO = 79.0 mol
Moles of O2 = 82.0 mol
To determine the limiting reagent, we compare the moles of NO2 produced from each reactant:
Moles of NO2 from NO = 1 mole of NO2 per mole of NO × 79.0 mol of NO = 79.0 mol of NO2
Moles of NO2 from O2 = 2 moles of NO2 per mole of O2 × 82.0 mol of O2 = 164.0 mol of NO2
The limiting reagent is the reactant that produces fewer moles of NO2. In this case, the limiting reagent is NO, as it produces only 79.0 mol of NO2.
Therefore, the number of moles of nitrogen dioxide that could be prepared is 79.0 mol.
b) The limiting reagent is NO, and the excess reagent is O2.
If the amount of NO is increased, it would not affect the potential yield of NO2 because the reaction is limited by the amount of NO available. Increasing the amount of NO beyond its stoichiometric ratio will not result in a higher yield of NO2.
c) If the amount of O2 is increased, the limiting reagent would still be NO since it produces fewer moles of NO2. Increasing the amount of O2 beyond its stoichiometric ratio will not affect the potential yield of NO2 either, as the reaction is limited by the amount of NO available.
a) To calculate the number of moles of nitrogen dioxide (NO2) that can be prepared, we need to determine the limiting reagent first. The limiting reagent is the reactant that is completely consumed and limits the amount of product formed.
To find the limiting reagent, we compare the stoichiometric ratio of the reactants to the given moles of each reactant.
From the balanced equation:
2 NO(g) + O2(g) ⟶ 2 NO2(g)
The stoichiometric ratio between nitrogen oxide (NO) and nitrogen dioxide (NO2) is 2:2, which simplifies to 1:1. This means that for every 2 moles of NO, we get 2 moles of NO2.
Therefore, for 79.0 moles of nitrogen oxide (NO), we can expect to get 79.0 moles of nitrogen dioxide (NO2).
Similarly, for 82.0 moles of oxygen (O2), we can expect to get 82.0/2 = 41.0 moles of NO2.
Comparing the moles obtained from each reactant, we see that the limiting reagent is oxygen (O2) because it produces fewer moles of NO2 than nitrogen oxide (NO).
So, the maximum number of moles of nitrogen dioxide (NO2) that can be prepared is 41.0 moles.
b) The limiting reagent is the reactant that determines the maximum amount of product that can be formed. In this case, we determined that the limiting reagent is oxygen (O2).
The excess reagent is the reactant that is left over after the limiting reagent is completely consumed. In this case, the excess reagent is nitrogen oxide (NO), as there are more moles of NO than can be reacted with the available oxygen.
If the amount of NO were increased, it would not affect the potential yield of NO2 because oxygen is still the limiting reagent. The reaction can only proceed at the rate determined by the amount of oxygen available, so increasing the amount of NO would not increase the amount of NO2 produced.
c) If the amount of O2 were increased, it would not affect the potential yield of NO2 either. As we determined earlier, oxygen is the limiting reagent. Increasing its amount beyond the required stoichiometry will not change the maximum amount of NO2 that can be produced.