Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would increase the molar concentration at equilibrium of the product N2O4(g)?
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Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would increase the molar concentration at equilibrium of the product N2O4(g)?Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would increase the molar concentration at equilibrium of the product N2O4(g)?Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would increase the molar concentration at equilibrium of the product N2O4(g)?Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would increase the molar concentration at equilibrium of the product N2O4(g)?Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would increase the molar concentration at equilibrium of the product N2O4(g)?Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would increase the molar concentration at equilibrium of the product N2O4(g)?Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would increase the molar concentration at equilibrium of the product N2O4(g)?Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would increase the molar concentration at equilibrium of the product N2O4(g)?
To determine the changes that would increase the molar concentration at equilibrium of the product N2O4(g), we need to look at the stoichiometry of the equation and the Le Chatelier's principle.
In the given equation, 2NO2(g) ⇌ N2O4(g), we can see that the reaction is in equilibrium with both reactant and product gases present.
According to Le Chatelier's principle, changes in the conditions of a system at equilibrium will cause the system to shift in a way that minimizes the effect of the change. Let's consider the following changes:
1. Increasing the concentration of NO2(g):
According to the equation, the formation of N2O4(g) requires the reactant NO2(g). If we increase the concentration of NO2(g), the system will shift to the right to counteract the change and restore equilibrium. This will result in an increase in the molar concentration of the product N2O4(g).
2. Decreasing the concentration of NO2(g):
Conversely, if we decrease the concentration of NO2(g), the system will try to compensate by shifting to the left to produce more reactant NO2(g). As a result, the molar concentration of the product N2O4(g) will decrease.
3. Increasing the pressure:
Since there are fewer moles of gas on the product side (N2O4), increasing the pressure will favor the side with fewer moles of gas. The system will shift to the right, increasing the molar concentration of N2O4(g).
4. Decreasing the pressure:
Conversely, if we decrease the pressure, the system will shift to the side with more moles of gas to restore equilibrium. In this case, it will shift to the left, decreasing the molar concentration of N2O4(g).
Therefore, based on the given equation, increasing the concentration of NO2(g) or increasing the pressure would increase the molar concentration at equilibrium of the product N2O4(g).