How would an increase in pressure affect the following reaction? N2 (g) + O2 (g) Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2NO (g) The equilibrium would shift to the right. The eq
How would an increase in pressure affect the following reaction?
N2 (g) + O2 (g) Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2NO (g)
The equilibrium would shift to the right.
The equilibrium would shift to the left.
There would be no change to equilibrium.
The effect on equilibrium cannot be determined.
How would an increase in pressure affect the following reaction?
N2 (g) + O2 (g) Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2NO (g)
The equilibrium would shift to the right.
The equilibrium would shift to the left.
There would be no change to equilibrium.
The effect on equilibrium cannot be determined.
1 Answer
There would be no change to (position of) equilibrium.
Explanation:
When any attempt is made to apply a change to an equilibrium system, the position of the equilibrium shifts so as to negate or nullify the effect of the change. This is the principle of Le Chatalier.
Your question asks what effect an "increase in pressure" would have, and I assume you mean total pressure, rather than partial pressure of one of the reacting species.
If you mean total pressure, the answer is that there would be no change to the equilibrium. An increase of pressure can drive gaseous equilibria positions to the side of the reaction that has fewer moles. But in this case, there is the same number of moles on both sides of the reaction. So the position will not change.
