30 atmospheres of N2 react with 60 atmospheres H2 at 100 degrees C in a 10 liter volume. The reaction goes to completions. The resulting ammonia is than cooled to -35 degrees C, where it is stored as a liquid with a density of 700 kg/m3. What is the volume of liquid ammonia that is produced during this reaction?
I think the wording in this problem is flawed. I interpret the problem as asking what is volume NH3 PRODUCED and not what is stored but I think the author of the problem probably wants the volume of the liquid NH3 when stored.
..........N2 + 3H2 ==> 2NH3
mols N2 to start, use PV = nRT and solve for n = number of mols.
Do the same for mols H2 initially. Find the limiting regent which appears to be N2. Calculate mols NH3 produced at 100 C. Then if you want to convert to volume at -35 C, convert mols NH3 to grams (grams = mols x molar mass), then mass = volume x density and solve for mols.
Post your work if you get stuck.