Chemistry question involving Conversion of Gases in terms of Liters?

Question

The direct conversion of H2 and N2 gases at high pressure using a catalyst is:

N2 + 3H2 <--> 2NH3

How many liters of 2NH3 can be obtained using 27.7L of N2 and 102.3L of H2? Assuming complete conversion and constant pressure of 500 atm and constant temperature of 500 K.

I'm really stuck on this problem, any help would be appreciated.

Thanks, I was thinking too much into the question instead of considering limiting reagents.

Answer 1

The ratio is 1:3:2 for the gases. Using that ratio we see that the limiting reactant is the N2 (27.7 L) because 3 X 27.7 is less than 102.3 L of the H2. Since 1 L N2 gives 2 L of NH3, then 27.7 L of N2 will give 55.4 L of NH3.