Answer:
1. Add N2O and
3. Remove N2
Explanation:
In equilibrium, there is a balance between the concentrations of the reactants and products. If more reactants are added, the equilibrium will shift to the right, favoring the forward reaction. This cause an increase in the concentration of the product and the equilibrium constant is unchanged.
Products can also be removed in order to increase the amount of products formed, forward reaction. This shifts the equilibrium to the right.
In the reaction 2N2O <-----> O2 + 2N2, adding N2O to the mixture favors the forward reaction and more products are formed, equilibrium shifts to the right.
Also, removing the product formed favors the forward reaction as more products will be formed in order to achieve equilibrium. The equilibrium therefore shifts to the right.
The following options that will cause the equilibrium to shift to the right side are the addition of N2O, removal of O2, removal of N2.
According to Le Cateliers Principle, addition of reactants will tend to cause a shift of the equilibrium to the right while the removal of products will cause a shift in the equilibrium to the right side.
From the given reaction:
2N2O(g) ⇌ O2(g) + 2N2(g)
Therefore, the removal of O2 and N2 will cause the equilibrium to shift to the right side, and also the addition of N2O will also cause the equilibrium to shift to the right side.
Therefore, the following options that will cause the equilibrium to shift to the right side are the addition of N2O, removal of O2, removal of N2.
Learn more about Le Cateliers Principle here:
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