Question

A mixture of reactants and products for the reaction shown below is at
equilibrium in a 2.0 L container. What would most likely happen to the
equilibrium if the volume of the container were increased to 4.0 L?
N₂(g) + 3H₂(g)—2NH₂(g)
A. More NH3 would be produced.
B. Less N₂, H₂, and NH3 would be produced.
C. More N₂, H₂, and NH3 would be produced.
D. More N₂ and H₂ would be produced.

Answer 1

If the volume of the container were increased to 4.0 L, more N₂ and H₂ would be produced (Option D)

What is chemical equilibrium?

This is simply defined as a state in a chemical system where there is no observable change in the properties of the system with time.

Principle of chemical equilibrium

A French scientist postulated a principle which helps us to understand a chemical system in equilibrium.

The principle states as follow:

If a an external constraint such as change in temperature, pressure or concentration is imposed on a system in equilibrium, the equilibrium will shift so as to neutralize the effect.

How to determine what will happen if the volume of the container is increased from 2 L to 4 L

From the principle given above, we can see that volume does not affect equilirium position.

However, from Boyle's law, we understood that pressure and volume are in invest relationship.

Thus, increasing volume simply means decreasing pressure.

A decrease in pressure will favors the side where there is an increase in volume.

Let us consider the equation from the question:

N₂(g) + 3H₂(g) <=> 2NH₃(g)

• Volume of reactants = 1 + 3 = 4 L
• Volume of products = 2 L

Thus, we can conclude that increasing the volume (i.e decreasing the pressure) of the reaction will favors the backward reaction, hence, more N₂ and H₂ would be produced.

Learn more about chemical equilibrium:

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