120 grams of N2h4 reacts with 140.0 grams 0f H2O2 to produce HNO3 and H2O. how many grams of HNO3 are produced? {N=14.0 ; H=1.00; O=16.0

Answer 1

1). Write a correctly balanced equation:

N₂H₄ + 7H₂O₂ ==> 2HNO₃ + 8H₂O ... balanced equation (not that easy to balance)

2). Find the limiting reactant (divide mols of each by the corresponding coefficient):

mols N₂H₄ = 120 g N₂H₄ x 1 mol N₂H₄ / 32.04 g = 3.75 mols N₂H₄ (÷1 -> 3.75)

mols H₂O₂ = 140.0 g H₂O₂ x 1 mol H₂O₂ / 34.01 g = 4.12 mols H₂O₂ (÷7 -> 0.588)

H₂O₂ is the limiting reactant and will determine the amount of HNO₃ produced

3). Determine theoretical yield of HNO3:

4.13 mols H₂O₂ x 2 mols HNO₃ / 7 mols H₂O₂ x 63 g HNO₃/ mol HNO₃ = 74 g HNO₃ produced (2 sig. figs.)