For the chemical reaction shown, 2H2O2(l)+N2H4(l)⟶4H2O(g)+N2(g) determine how many grams of N2 are produced from the reaction of 8.08 g of H2O2 and 5.73 g of N2H4.

Question

For the chemical reaction shown,

2H2O2(l)+N2H4(l)⟶4H2O(g)+N2(g)

determine how many grams of N₂ are produced from the reaction of 8.08

g of H₂O₂ and 5.73

g of N₂H₄.

N₂ produced:______?_________g

Answer 1

8.08g H₂O₂ x 1 mole H₂O₂ x 1 mole N₂ x 28g N_{2 =} 3.33g of N₂

34.02g H₂O₂ 2 mole H₂O₂ 1 mole N₂

5.73g N₂H₄ x 1 mole N₂H₄ x 1 mole N₂ x 28g N_{2 =} 5.01g of N₂

32.05g N₂H₄ 1 mole N₂H4 1 mole N₂

The lowest amount tells you the maximum amount (theoretical yield) of the product that can be produced.

Therefore the amount of N₂ that can be produced in this reaction is 3.33g.