A mixture of ammonia and oxygen is prepared by combining 0.330 L of NH3 (measured at 0.710 atm and 22°C) with 0.200 L of O2 (measured at 0.740 atm and 51°C).

Question

How many milliliters of N2 (measured at 0.740 atm and 100. °C) could be formed if the following reaction occurs?

4NH3(g) + 3O2(g) -----> 2N2(g) + 6H2O(g)

Answer 1

figure the moles of NH3 and O2 at the temp, pressures given.

THen the ratio in the balanced equation is for every mole of NH3, you have to have .75 moles of O2. Do you have enough or too much O2? If too much, then the reacdtion is limited by NH3, and you get .5 moles of N2 for each NH3 mole.
If you have too little O2, then yo will get for each O2 mole, 2/3 mole of N2

then convert the moles of N2 to volume using the ideal gas law.