What would happen if O2 were added to N2(g) + O2(g) 2NO(g) at equilibrium?
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N2 + O2 ==> 2NO, adding O2 at equilibrium would make the reaction shift to the right.
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If O2 is added to the reaction N2(g) + O2(g) ⇌ 2NO(g) at equilibrium, the system will shift in order to reestablish equilibrium. To predict how the system will respond, we need to consider Le Chatelier's principle.
Le Chatelier's principle states that if a system at equilibrium is subjected to a change, it will adjust in a way that minimizes the effect of that change. In this case, adding O2 will increase the concentration of O2, causing a disturbance in the equilibrium.
Since the forward reaction (N2 + O2 ⇌ 2NO) consumes O2, an increase in its concentration will push the reaction towards the right to consume the additional O2. This means that the reaction will shift to produce more NO.
Conversely, the increase in O2 concentration will also lead to an increase in the concentration of products (NO). According to Le Chatelier's principle, the system will react in a way that opposes this increase. Consequently, the reaction will shift in the reverse direction to consume some of the additional NO molecules and produce more N2 and O2.
In summary, adding O2 to the reaction at equilibrium will cause the system to shift to the right, increasing the concentration of NO, while also causing a partial reverse reaction to reduce the concentrations of N2 and O2. This adjustment will result in a new equilibrium being established with higher concentrations of NO, but with lesser concentrations of N2 and O2.