consider the reaction 2N2O(g) == O2(g)+2N2(g).which of the following will cause a shift in the equilibrium to the left?
To determine what will cause a shift in the equilibrium to the left, we need to understand Le Chatelier's principle. According to this principle, if a stress or change is applied to a system at equilibrium, the system will adjust in a way that counteracts that change.
In the case of this reaction, 2N2O(g) ⇌ O2(g) + 2N2(g), a shift to the left means that the reactants are favored, resulting in an increase in the concentration of N2O and a decrease in the concentration of O2 and N2.
Here are a few factors that can cause a shift to the left:
1. Increase in pressure: If the pressure is increased, the system will try to decrease the pressure by favoring the side with fewer moles of gas. In this case, the left side has two moles of gas (2N2O), while the right side has three moles of gas (O2 + 2N2). Therefore, an increase in pressure will cause a shift to the left.
2. Decrease in temperature: If the temperature is decreased, the system will try to add heat by favoring the exothermic direction, which is the left side in this case (2N2O). Therefore, a decrease in temperature will cause a shift to the left.
3. Addition of an inert gas: Adding an inert gas, such as helium (He), which does not participate in the reaction, will increase the total pressure without affecting the concentrations of the reactants or products. Therefore, it will not cause a shift in the equilibrium.
4. Removal of O2 or N2: Removing either O2 or N2 from the reaction mixture will disrupt the equilibrium and cause a shift to the left, favoring the reactants.
5. Catalyst: Adding a catalyst does not cause a shift in the equilibrium position. Instead, it increases the rate at which equilibrium is attained but does not change the distribution of reactants and products.
In summary, an increase in pressure, a decrease in temperature, or the removal of O2 or N2 will cause a shift in the equilibrium of this reaction to the left, favoring the reactants (2N2O).
A shift in the equilibrium to the left means that the reaction will favor the formation of more N2O(g) and less O2(g) and N2(g). The factors that could cause this shift include:
1. Decreasing the concentration of N2O(g): If the concentration of N2O(g) is reduced through, for example, removing some of it from the reaction mixture, the equilibrium will shift to the left to produce more N2O(g) to restore the balance.
2. Increasing the concentration of O2(g) or N2(g): By increasing the concentration of either O2(g) or N2(g), the equilibrium will shift to the left to consume some of these gases and produce more N2O(g).
3. Decreasing the concentration of the reactant gases: A decrease in the concentration of the reactant gases, N2O(g), O2(g), or N2(g), will shift the equilibrium to the left to compensate for the loss.
4. Decreasing the temperature: Lowering the temperature will favor the exothermic direction of the reaction, which is the formation of N2O(g). The equilibrium will shift to the left to produce more N2O(g) and less O2(g) and N2(g).
5. Adding a catalyst: Adding a catalyst won't directly shift the equilibrium position, but it will speed up the reaction. It will only affect the rate at which the reaction reaches equilibrium, not the position of equilibrium itself.
Therefore, the factors that will cause a shift in the equilibrium to the left are: decreasing the concentration of N2O(g), increasing the concentration of O2(g) or N2(g), decreasing the concentration of the reactant gases, decreasing the temperature, and adding a catalyst.
possibilities not listed.
Note the correct spelling of chemistry.