What would happen if O2 were added to N2(g) + O2(g) 2NO(g) at equilibrium?

To determine what would happen if O2 were added to the reaction N2(g) + O2(g) -> 2NO(g) at equilibrium, we need to consider Le Chatelier's principle. According to this principle, if a system at equilibrium is subjected to a change, it will react in a way that minimizes the effect of that change.

In this case, O2 is being added to the system, which means the concentration of O2(g) will increase. As a result, the system will no longer be at equilibrium, and the concentration of O2 will be higher than the original equilibrium concentration.

To understand how the system will react to this increase in O2, we need to look at the balanced equation. In the forward reaction, N2 and O2 combine to form 2NO. Therefore, adding more O2 will shift the equilibrium position to the right, favoring the formation of more NO.

As a result, the system will try to counteract the increase in O2 concentration by producing more NO. This means the concentrations of N2 and O2 will decrease, while the concentration of NO will increase until a new equilibrium is established.

In summary, if O2 is added to the reaction N2(g) + O2(g) -> 2NO(g) at equilibrium, the system will react by producing more NO to minimize the effect of the change. The concentrations of N2 and O2 will decrease, while the concentration of NO will increase until a new equilibrium is reached.

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