Le Chatelier's principle states that changes in pressure are attributable to changes in volume. If we increase the volume, the reaction will shift toward the side that has more moles of gas. If we decrease the volume, the reaction will shift toward the side that has less moles of gas. Since the product side has only two moles of gas, compared to the reactant side with four moles, the reaction would shift toward the product side, and more NH₃ would form.

Chemical equilibrium is defined as a state when the rates of the forward and reverse reactions are equal. Different reactions will have different concentrations of products are reactants, and concentration can vary depending on the process. Chemical equilibrium, however, is always the point at which there is no bias towards creating products or reactants.

If the forward reaction rate and reverse reaction rate are equal, then there is no net change in concentration of the reactants or products. This makes them appear to be stable.

When a reaction is at equilibrium, the concentrations of reactants and products are no longer increasing or decreasing; however, this does not mean that the forward and reverse reactions have stopped taking place. They are simply taking place at the same rate so that the concentrations of products and reactants do not change. Equilibrium is a dynamic process. Reactions are still taking place, but they offset one another in terms of rate. Essentially, every product that is created is immediately converted back to reactant by the reverse process, making the concentration of reactants and products appear constant.

Le Chatelier's principle states that a system will shift in a particular direction in order to reduce introduced stress to the system. In other words, if something is added to one side of the equation, the other side will consequently increase in order to restore equilibrium.

When gases are involved in the reaction, pressure increases on the side of the reaction with more moles of gas. Adding an additional amount of pressure will push the reaction toward the side with fewer moles of gas. This helps lower the pressure inside the container.

There are four moles of gas on the reactants side, and two moles on the products side. If pressure is increased, the system will shift to the right in order to adjust to the new pressure.

Le Chatelier's principle states that a system will shift in a particular direction in order to reduce introduced stress to the system. In other words, if something is added to one side of the equation, the other side will consequently increase in order to restore equilibrium.

The above reaction is exothermic, meaning that heat is released from the system. As a result, heat is considered a product.

By removing nitrogen or hydrogen gas, the system would shift to the left in order to create more reactants. If temperature is decreased, the system will create more heat by shifting to the right. Not only will this create more heat, but it will also create more ammonia, as they are both products of the reaction.

We can set up the equilibrium expression by placing the products, raised to the power of their coefficients, in the numerator and reactants, raised to the power of their coefficients, in the denominator:

We are given the value of the equilibrium constant and the equilibrium concentration of . Using stoichiometric coefficients, we can determine that a variable concentration, , of  will be present at equilibrium, and  of  will be present at equilibrium. Plugging in:

Simplify:

Now we can solve for  (which is the equilibrium concentration of , as we assigned) by dividing both sides by 4 and then taking the cube root.

Rounding to 2 sig figs (to match the two numbers we were given by the problem), we get: