If 250. L of nitrogen reacts with 582 L of hydrogen by the reaction:
N2 + 3H2 (g)→ 2NH3(g)
how much nitrogen is unreacted ? All gases are at the same temperature and pressure
First we need to know how much moles we have of each substance.
- There is 250 L of Nitrogen. The density of Nitrogen is 1.251 g/L. This gives the Nitrogen a mass of (250 * 1.251 =) 312.75 grams. The molecular weight of N2 is (14.007 * 2 =) 28.014. This makes the amount of Nitrogen (312.75 / 28.014 =) 11.164 moles.
- There is 582 L of Hydrogen. The density of Hydrogen is 0.08988 g/L. This gives the Hydrogen a mass of (582 * 0.08988 =) 52.31016. The molecular weight is (1.008 * 2 =) 2.016. This makes the amount of Hydrogen (52.31016 / 2.016 =) 25.9475 moles.
Now that we know that, you already gave us the reaction:
N2 + 3H2 (g)→ 2NH3(g)
So the gasses react in a proportion of 1:3. We know that all the Hydrogen will react. With 25.9475 moles of Hydrogen, we'll have (25.9475 / 3 =) 8.6492 moles of Nitrogen react. This leaves us with (11.164 – 8.6492 =) 2.5148 moles of Nitrogen.
Now calculate back:
2.5148 * 2.016 = 5.0698 grams
5.0698 / 1.251 = 4.0526 Liters
So 4.05 Liters of Nitrogen is unreacted.