N2 (g) + O2 (g) --> 2NO (g)

Question

Question A. How many grams of nitric oxide can be produced when 35.0 g of nitrogen reacts?

 

Question B. How many grams of nitric oxide can be produced when 35.0 g of oxygen reacts?

 

Question C. Based on your answers in A and B, predict the amount of nitric oxide that can be produced when 35.0 g of nitrogen is reacted with 35.0 g of oxygen.

 

Question D. Explain the reasoning used in Question C.

Answer 1

a) 35.0 g N₂ x (1 mol N₂/28 g N₂) x (2 mol NO/1 mol N₂) x (30 g NO/1 mol NO) =

75 g NO

b) 35.0 g O₂ x (1 mol O₂/32 g O₂) x (2 mol NO/1 mol O₂) x (30 g NO/1 mol NO) =

65.625 g NO

c) 65.625 g NO

d) Since we know how much NO is produced for 35.0 g of N₂ and 35.0 g of O₂, the true amount produced will be the lower amount, because of that reactant being the limiting reagent (which in this case, is O₂). Therefore, 65.625 g NO will be produced. Another way to think about it is that there isn't enough O₂ to react with the 35.0 g of N₂ that would've given you 75 g NO.