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?

N.(g) + 3H2(g)

22NH3(g)

The system will shift to the left producing more moles of gases trying to maintain the original pressure of the system

Explanation:

Based on LeChatelier's principle, a change in temperature, pressure, volume or concentration on a system result in an opposing change trying to maintain the initial equilibrium conditions.

In the reaction:

N₂(g) + 3H₂(g) ⇄ 2NH₃(g)

4 moles of gas reacts producing 2 moles of gas.

In a gas reaction, the system will try to maintain the total pressure.

If the volume of the container increases, the system will shift to the side of the reaction that has more moles of gases in order to maintain the pressure.

That means if in the reaction the volume of the container increase from 2.0L to 4.0L the system will shift to the left producing more moles of gases trying to maintain the original pressure of the system.