What would happen if you increased the temperature of a system that contained nitrogen, hydrogen, and ammonia? According to Le Châtelier's principle, if you added heat to the system, the equilibrium would shift in the direction that removes heat from the system. The system would favor the reverse reaction, which is endothermic. So by increasing the temperature, you would decrease the amount of ammonia.
Suppose you increased the pressure of the system. According to Le Châtelier's principle, if you increased the pressure, the equilibrium would shift in the direction that decreases the pressure of the system. In order to decrease pressure, the system would favor the reaction that produces fewer gas molecules. You can see that the left side of the equation has four gas molecules, while the right side has two. So by increasing the pressure, you would shift the equilibrium to the right, producing more ammonia.
A change in concentration of the reactants or products can also affect equilibrium. Suppose you removed ammonia from the nitrogen-hydrogen-ammonia system. Le Châtelier's principle tells you that the equilibrium would shift in the direction that produces ammonia. In order to produce ammonia, the system would favor the forward reaction.
Figure 27 Operating an ammonia plant at relatively low temperature, high pressure, and low ammonia concentration maximizes the amount of ammonia produced.
Reviewing Concepts
What happens when a physical change does not go to completion? What happens when a reaction does not go to completion?
Once a chemical reaction has reached equilibrium, how does the system respond to change?
What does the double-ended arrow indicate in the following chemical equation?
For which of the following reactions are both reactants and products likely to be found when the reaction appears to be complete? Explain.
Inferring Suppose the following reaction is allowed to come to equilibrium.
How will increasing the pressure on this system affect the amount of N2O4 formed?
Using Models At 0°C, liquid water is in equilibrium with ice. Make a drawing of water molecules at this temperature, and describe what is happening.
Phase Changes Write an equation for a system in which the sublimation and deposition of water have reached equilibrium. Use what you studied in Section 3.3 to explain what changes are happening.