Question

A mixture of hydrazine (N2H4) and hydrogen peroxide(H2O2) is used as fuel for rocket engines. These two substances react as shown by the equation N2H4 +2H2O2 --> N2 +4H2O What mass of N2H4 in grams is needed to react with completely with 35.0g of H2O2? List all mole to mole realationships and show all work

Answer 1

The reaction that is given is

N2H4+ 2H2O2 --->N2+ 4H2O

Molecular weights : N2H4= 2*14+4*1 =32, H2O2= 2*1+ 2*16= 34, N2= 2*14= 28 and H2O= 2*1+16=18

Mole= Mass/ Molecular weigt

Moles of H2O2 in 35 gms = 35/34=1.029412

As per the reaction, 2 mole of hydrogen peroxide (H2O2) requires 1 moles of hydrazine (N2H4) for complete reaction to produce 1 mole of Nitrogen (N2) and 4 moles of Water (H2O)

1.029412 moles of H2O2 requires 1*1.029412/2 moles of N2H4=0.514706 moles of N2H4

Mass of H2O2= Moles* Molecular weight= 0.514706*32=16.47 gms