[brainz2]

Hi everyone,
I would greatly appreciate it if you can tell me how you work these problems out:

Given reaction 2NH3(g) + 3Cl2 (g) → N2(g) +6HCl (g), you react 5.0 L of NH3 with 5.0L of Cl2 measured at the same conditions in a closed container.  Calculate the ratio of pressures in the container (P final/ P initial).  Answer is 1.33.  How do you get this?

A mixture is prepared from 15.0L of ammonia and 15.0L chlorine measured at the same conditions, these compounds react according to the following equation:
2NH3(g) + 3Cl2 (g) → N2(g) + 6HCl (g)
When the reaction is completed, what is the volume of each gas (NH3, Cl2, N2, HCl respectively)? Assume the final volumes are measured under identical conditions.
Answer is 5.00L, 0.00L, 5.00L, 30.0L.  How do you get this?

Thx.

[Borek]

Looks like a simple stoichiometry with limiting reagents to me. Just remember that identical volumes of gases contain identical number of moles.

[brainz2]

What I can't figure out is how does one find what the limiting reactant is?  For some reason, I'm still in the clouds with that one.  I know that once I figure that out, all these problems will be simple...Thx.

[Borek]

limiting reagents

[brainz2]

Figured it out. Thx.