Question

Two compartments of 1000 liters each are filled with gas mixtures and separated by a thin wall. On the left is air containing a concentration of 0.45 M of HCl gas. On the right is air with 0.27 M ammonia gas. Both compartments are are 25 degrees celsius and 1 atmosphere total pressure. The wall is destroyed and a white fog of solid ammonium chloride is formed that slowly precipitates into a dust of the floor of the containers. How many moles and grams of HCl are in the left compartment before the wall is punctured?
What is the final pressure of the gas in the container? What is the limiting reactant? What is the mass of the solid ammonium chloride formed?

Answer 1

There is something wrong with the given conditions, because the maximum moles you can have in each compartment is 40.9, due to the ideal gas equation:

In each compartment your statement says there are almost 10 times of moles. So I'll solve it without assuming the total pressure of 1 atm

You have 1000L in each compartment, you can calculate number of moles, using the concentration:

Limiting reactant, you need to write the reaction:

the molar ratio is 1:1

so your limiting reactant is the ammonia, all of it is reacting while some of the HCl remains:

Ammonia reacting---->270moles

HCl remaining---->450-270=180moles

NH4Cl formed----->270 moles

the final pressure of the remainig gas is the pressure of the HCl using the gas equation, and the volume of 2000 since the 2 compartments are together now.

Mass of the ammonium chloride: