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.

Question

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?

Answer 1

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.

Answer 2

Thank you!