Predict the shift of equilibrium for each of the following conditions in the following reaction involving gaseous reactants and products:
N2 + 3H2 = 2NH3 + heat
To predict the shift of equilibrium for each condition, we need to consider Le Chatelier's principle, which states that when a system in equilibrium experiences a change, it will adjust to counteract that change and restore equilibrium. In this reaction, we have gaseous reactants and products, so changes in pressure, temperature, and concentration will affect the equilibrium position.
1. Increase in pressure:
When the pressure is increased, the reaction will shift in the direction that reduces the number of gaseous molecules. In this case, there are a total of 4 moles of gaseous molecules on the left side (N2 + 3H2) and 2 moles on the right (2NH3). To reduce the number of gaseous molecules, the equilibrium will shift to the left (reverse reaction) and decrease the pressure. As a result, the reaction will produce more N2 and H2, reducing the amount of NH3.
2. Decrease in pressure:
Conversely, when the pressure is decreased, the reaction will shift in the direction that increases the number of gaseous molecules. The equilibrium will shift to the right (forward reaction) to increase the pressure. More NH3 will be produced at the expense of N2 and H2.
3. Increase in temperature:
When the temperature is increased, the reaction will shift in the endothermic direction to absorb the excess heat. In this case, the forward reaction (2NH3 + heat) is endothermic, meaning it absorbs heat. Therefore, increasing the temperature will shift the equilibrium to the right, favoring the formation of NH3.
4. Decrease in temperature:
Conversely, when the temperature is decreased, the reaction will shift in the exothermic direction to generate more heat. In this case, the reverse reaction (N2 + 3H2) is exothermic, meaning it releases heat. So, decreasing the temperature will shift the equilibrium to the left, favoring the formation of N2 and H2.
It's important to note that changes in concentration can also affect the equilibrium position. However, for this particular question, the concentration of the reactants and products is not given.