Question

for the chemical reaction
2H₂O₂ (l) +N₂H₄(l)--->4H₂O(g)+N₂(g)


determine how many grams of N2 are produced from the reaction of 8.62 g of H2O2 and 6.95 g of N2H4.

Answer 1

Mass of H₂O₂ = 8.62 g

Molar mass of H₂O₂ = 34.0147 g/mol

Moles of H₂O₂ = mass/ Molar mass = 8.62 g/(34.0147 g/mol) = 0.253 mol

Mass of N₂H₄ = 6.95 g

Molar mass of N₂H₄ = 32.0452 g/mol

Moles of N₂H₄ = 6.95g/ (32.0452 g/mol) = 0.217 mol

From reaction,

2 mol of H₂O₂ reacts with 1 mol of N₂H₄

Thus, 0.253 mol of H₂O₂ reacts with 0.253*1/2 = 0.127 mol of N₂H₄

So, H₂O₂ is a limiting reagent.

2 mol of H₂O₂ produces 1 mol of N₂

Thus, moles of N₂ produced from 0.253 mol of H₂O₂ = 0.127 mol

Molar mass of N₂ = 28.0134 g/mol

Mass of N₂ produced = moles* molar mass = 0.127 mol*28.0134 g/mol = 3.55g