Predict how each of the following changes will affect the following reaction involving gaseous reactants and products: 2NO2 = N2O4 + heat
a. the temperature is increased.
b. the pressure is increase.
c. N2O4 is removed from the equilibrium mixtur.
d. NO2 is added to the equilibrium mixture.
a. Increase NO2
b. Increase the N2O4
c. reduce No2
d. increase N2O4
To predict how the given changes will affect the reaction, we need to understand the principles of Le Chatelier's Principle. According to this principle, if a system at equilibrium is subjected to a change in temperature, pressure, or concentration, it will adjust in a way to counteract the change and restore equilibrium.
Now let's analyze each of the changes and its effect on the given reaction:
a. If the temperature is increased:
When the temperature is increased, the equilibrium will shift in the endothermic direction (the direction that absorbs heat) to counteract the increase in temperature. In this case, the forward reaction is endothermic (heat is a product), so increasing the temperature will favor the formation of products N2O4. Therefore, the equilibrium will shift to the right, resulting in an increase in the concentration of N2O4.
b. If the pressure is increased:
For gaseous reactions, changes in pressure can affect the equilibrium based on the number of moles of gas on each side of the reaction. In this case, the forward reaction has two moles of gas (2NO2), whereas the reverse reaction has one mole of gas (N2O4). If the pressure is increased, the equilibrium will shift in the direction that reduces the number of moles of gas. Therefore, the equilibrium will shift to the left, resulting in a decrease in the concentration of products N2O4.
c. If N2O4 is removed from the equilibrium mixture:
Removing a reactant will cause the equilibrium to shift in the forward direction to replace what was removed. In this case, removing N2O4 will cause the equilibrium to shift to the right to compensate for the loss of N2O4. As a result, more N2O4 will be formed, and the concentration of N2O4 will increase.
d. If NO2 is added to the equilibrium mixture:
Adding a reactant will cause the equilibrium to shift in the reverse direction to counteract the increase in concentration. In this case, adding NO2 will shift the equilibrium to the left to reduce the excess NO2. Therefore, the concentration of N2O4 will decrease.
Remember, these predictions are based on Le Chatelier's Principle and assume that the given reaction is at equilibrium initially.
a. When the temperature is increased, the equilibrium will shift in the endothermic direction to absorb the added heat. In this reaction, heat is on the right side of the equation, so an increase in temperature will favor the formation of products. As a result, the equilibrium will shift to the right, increasing the amount of N2O4 and decreasing the amount of NO2.
b. When the pressure is increased, the equilibrium will shift in the direction that produces fewer moles of gas. In this reaction, the number of moles of gas decreases from left to right, so an increase in pressure will favor the production of reactants. Therefore, the equilibrium will shift to the left, decreasing the amount of N2O4 and increasing the amount of NO2.
c. When N2O4 is removed from the equilibrium mixture, the equilibrium will shift to replace what has been removed. In this reaction, removing N2O4 will cause the equilibrium to shift to the right to produce more N2O4. Consequently, the amount of N2O4 will increase, and the amounts of NO2 will decrease.
d. When NO2 is added to the equilibrium mixture, the equilibrium will shift to the left to consume the added reactant. This reaction produces NO2, so adding NO2 will shift the equilibrium to decrease the amount of NO2. As a result, the amount of NO2 will decrease, and the amount of N2O4 will increase.