What would happen if N2 were added to N2(g) + O2(g) ⇌ 2NO (g) at equilibrium?
Answer (2)
Adding N2 to the reaction N2(g) + O2(g) ⇌ 2NO(g) at equilibrium shifts the equilibrium to the right, increasing the concentration of NO produced. This occurs due to Le Chatelier's principle, where the system adjusts to counteract the added N2. The new equilibrium will show higher levels of both NO and adjusted levels of N2 and O2.
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When you add N 2 to the system at equilibrium given by the following reaction:
N 2 ( g ) + O 2 ( g ) ⇌ 2 NO ( g )
The system will respond according to Le Chatelier's Principle. This principle states that if a change is imposed on a system at equilibrium, the system will adjust itself to counteract that change and restore a new equilibrium.
Here's what's likely to happen step-by-step:
Addition of N 2 : By adding more N 2 , you are increasing the concentration of one of the reactants.
Shift in the Equilibrium: According to Le Chatelier's Principle, the system will attempt to reduce the effect of this change by shifting the equilibrium position to the right, towards the products, in order to consume the added N 2 . This shift will form more NO , resulting in:
A decrease in N 2 and O 2 concentrations as they are converted to NO .
An increase in the concentration of NO .
New Equilibrium Established: The system will eventually reach a new equilibrium state where the forward and reverse reactions occur at the same rates again, albeit with different concentrations of the reactants and products compared to the initial state.
Conclusion:
Adding N 2 will lead to more NO being formed and less of N 2 and O 2 as the system tries to re-establish equilibrium. This does not mean "more N 2 and O 2 would form"; rather, the opposite occurs.
