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An intermediate reaction used in the production of nitrogen containing fertilizers is that b/w NH3 and O2
4NH3(g) + 5O2(g)--> 4NO(g) + 6H2O(g)
A 150.0-L reaction chamber is charged with reactants to the following partial pressures at 500 degrees C: P(sub NH3)= 1.3 atm, P(sub O2)= 1.5 atm. What is the limiting reactant?

I'm having trouble getting to moles of my reactants from the information given. Can I assume that both gases have a volume of 150.0-L since gases assume the volume of the container? Or do I need to get the moles in a different way? I tried to use
V= nRT/P for each gas to get the volumes, but the number of moles is unknown.

P is the partial pressure given.
V is 150 L for both gases.
n can be calculated.
R is 0.08206 L*atm/mol*K
T is 273+500.

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