Question

A mixture of reactants and products for the reaction shown below is at

equilibrium in a 5.0 L container. What would most likely happen to the
equilibrium if the volume of the container were reduced to 3.0 L?
N (9) + 3H₂(9)
A₂NH,
TH(9)
A. The concentrations of N₂, H₂, and NH₃ would decrease until
equilibrium was reached again.
B. More N₂, H₂, and NH₃ would be produced until a new equilibrium
position was reached.
C. More NH₃ would be produced until a new equilibrium position was
reached.
D. More Ny and H₂ would be produced until a new equilibrium
position was reached."

Answer 1

If the volume of the container is reduced from 5.0 L to 3.0 L, the equilibrium would shift to favor the production of more NH₃.

Step-by-step explanation:

If the volume of the container is reduced from 5.0 L to 3.0 L, the equilibrium of the reaction N₂ + 3H₂ ⇌ 2NH₃ would shift to the side with fewer moles of gas. In this case, the forward reaction produces more moles of gas than the reverse reaction, so the equilibrium would shift to the right, favoring the production of more NH₃. Therefore, the answer is C. More NH₃ would be produced until a new equilibrium position was reached.