Ammonia is created in the Haber process in a rigid container (nitrogen gas plus hydrogen gas react to form ammonia gas). 10 moles of hydrogen gas are mixed with 5 moles of nitrogen gas. The initial pressure exerted on the container is 10 atm.
A) Assuming the reaction runs to completion, what will the pressure (in atm) on the vessel be after the reaction takes place?

5.56 atm

Explanation:

N₂(g) + 3H₂(g) → 2NH₃(g)

10 moles of hydrogen gas was mixed with 5 moles of nitrogen gas.

we need to determine the limiting reagent

from the equation

1 mole of nitrogen requires 3 mole of hydrogen to produce 2 mole of ammonia

looking the reaction hydrogen is the limiting reagent because 5 moles of nitrogen will require 15 moles of hydrogen

1 mole of nitrogen 3 moles of hydrogen 2 moles of ammonia

x moles of nitrogen 10 moles of hydrogen y moles of ammonia

10 / 3 moles of nitrogen is needed = 3.33 moles

10 × 2 / 3 moles of ammonia is produced = 6.667 moles

initial mole of nitrogen - consumed amount = residue

5 - 3.33 moles = 1.67 moles of nitrogen remained

total moles remaining = 1.67 moles of nitrogen + 6.667 mole of ammonia produced = 8.337 moles

now pressure is directly proportional to number of moles

15 moles 10 atm

8.337 moles will yield = 8.337 moles × 10 atm / 15 moles = 5.56 atm

i think it's letter a.