Agas contains a mixture of nh3(g) and n2h4(g), both of which react with o2(g) to form no2(g) and h2o(g). the gaseous mixture (with an initial mass of 61.00 g) is reacted with 10.00 moles o2, and after the reaction is complete, 4.062 moles o2 remains. calculate themass percent of n2h4(g) in the original gaseous mixture.

Mass percent of N2H4 in original gaseous mixture = 31.13 %

Explanation:

Given:

Initial mass of gaseous mixture = 61.00 g

Initial mole of oxygen = 10.0 mol

Moles of oxygen remaining after the reaction = 4.062 mol

Moles of oxygen used = 10.0 - 4.062 = 5.938 mol

Total oxygen used in both the reactions = 10.0 parts

out of 10 parts, 3 part react with N2H4.

Now, consider the reaction of N2H4

3 moles of O2 react with 1 mole of N2H4

1.78 moles of oxygen will react with 1.78/3 = 0.5933 mol of N2H4

Molecular mass of N2H4 = 32 g/mol

Total mass = 61.0 g

the reaction mixture contains some ammonia, plus a lot of unreacted nitrogen and hydrogen. the mixture is cooled and compressed, causing the ammonia gas to condense into a liquid. the liquefied ammonia is separated and removed. the unreacted nitrogen and hydrogen are then recycled back into the reactor .

can you attach the