hydrazine is used as a rocket fuel find the number of oxygen required to oxide 1.7 gram of hydrazine
The chemical formula for hydrazine is N2H4. When hydrazine is oxidized, it forms nitrogen gas (N2) and water (H2O).
To find the number of oxygen atoms required to oxidize 1.7 grams of hydrazine, we need to determine the molar mass of hydrazine.
The molar mass of N2H4 is:
(2 x atomic mass of nitrogen) + (4 x atomic mass of hydrogen)
= (2 x 14.01 g/mol) + (4 x 1.01 g/mol)
= 28.02 g/mol + 4.04 g/mol
= 32.06 g/mol
Now, we need to calculate the number of moles of hydrazine in 1.7 grams:
Number of moles = Mass / Molar mass
= 1.7 g / 32.06 g/mol
≈ 0.053 mol
According to the balanced equation for the oxidation of hydrazine, the ratio of oxygen to hydrazine is 1:1. Since there is 1 oxygen atom in 1 molecule of H2O, the number of oxygen atoms required will be the same as the number of hydrazine molecules.
The number of oxygen atoms required to oxidize 1.7 grams of hydrazine is approximately 0.053 x 6.022 x 10^23 (Avogadro's number) = 3.197 x 10^22 atoms.