Question

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

equilibrium in a 1.0 L container. What would happen to the equilibrium if argon gas were added to the container?
N2(g)+ 3H2(g) -> 2NH3(9)

A. More N2 and Hy would be produced until equilibrium was reached.
B. Less N2, H2, and NH3 would be produced until equilibrium was
reached.
C. More NH3 would be produced until equilibrium was reached.
D. The concentrations of N2, H2, and NH3 would remain the same.

Answer 1

D. The concentrations of N2, H2, and NH3 would remain the same.

Step-by-step explanation:

• In reversible reactions, equilibrium is a point in which the rate of forward reaction is equal to that of reverse reaction.
• Given the equation;

N₂(g)+ 3H₂(g) → 2NH₃(g) is a equilibrium at a constant volume of 1.0 L

• Addition of Argon gas which an inert gas dose not affect the equilibrium of the reaction.
• This is because the addition of an inert gas at constant volume only causes an increase in the total pressure of the system while the concentrations of the reactants and products remain constant, therefore not affecting the equilibrium.