Hydrazine (N2H4), a rocket fuel , reacts with oxygen to form nitrogen gas and water vapor. The reaction is represented with the equation: N2H4(l) + O2(g) → N2(g) + 2H2O(g) How many grams of hydrazine are needed to produce 96.0g water?
The given equation is: N2H4(l) + O2(g) → N2(g) + 2H2O(g)
From the periodic table: mass of nitrogen = 14 grams mass of hydrogen = 1 gram mass of oxygen = 16 grams Therefore: molar mass of N2H4 = 2(14) + 4(1) = 32 grams mass of water = 2(1) + 16 = 18 grams
From the balanced equation: 1 moles of N2H4 produces 2 moles of H2O. 32 grams of N2H4 produce 18*2=36 grams of water To know the mass of N2H4 needed to produce 96 grams of water, all you need to do is cross multiplication as follows: mass of N2H4 = (96*32) / 36 = 85.3334 grams
